Analytical Chemistry

Size: px
Start display at page:

Download "Analytical Chemistry"

Transcription

1 Analytical Chemistry Lecture No. 4 Date :16 /12/ 2012 Dr. Mohammed Hamed Buffers solutions: - buffers are solutions that resist changing ph when small amounts of acid or base are added they resist changing ph by neutralizing added acid or base The components of a buffer solution :- It is a mixture of weak acid and its salt:- CH 3 COOH is weak acid, CH 3 COONa is Salt of weak acid The Mechanisms of buffer solution to remain stable: - If base is added (OH - ): It will be buffered by the following reaction CH 3 COOH + OH CH 3 COO - + H 2 O So the ph will not change. the weak acid present in the buffer mixture can neutralize added base. - If acid (H + ) is added: it will be buffered by the following reaction, CH 3 COO - + H CH 3 COOH The ph will not alter significantly because the CH 3 COOH formed is a weak acid. Two important characteristics of a buffer include: 1. ph Range The ph range is the range of ph values over which a buffer system works effectively. The ph range of an acid or base can be seen as the region of little ph change vs. volume of base/acid added on a titration curve It is best to choose an acid with a pka close to the desired ph. 2. Buffering Capacity The buffering capacity of a buffered solution represents the amount of acid or base that can be absorbed by the solution without a significant change in ph. A buffer with a large capacity contains large concentrations of buffering components. Therefore the capacity of a buffered solution is determined by the magnitudes of [HA] and [A - ].

2 Many organic acids are weak acids. Weak acids do not completely dissociate in water. The dissociation of an organic acid is described by the following reaction: AH H + + A - weak acid conjugate base CH 3 COOH CH3COO - + H + weak acid conjugate base H 2 PO H 3 PO 4 + H + weak base conjugate acid One can analyze the strength of a weak acid. This means that the amount of hydrogen ion released can be determined. To do this, one can use the following expression: Ka=[H + ] [A - ] / [HA] where K a is defined as the acid dissociation constant. The larger the value of K a, the stronger the acid is. Because K a values vary over a wide range, they are usually expressed using a logarithmic scale: pka = - log Ka The hydrogen ion is one of the most important ions in biological systems. The concentration of this ion affects most cellular processes. For example, the structure and function of most biological macromolecules and the rates of most biochemical reactions are strongly affected by [H + ]. The ph scale has been devised as a convenient method of expressing hydrogen ion concentration. ph has been defined as the negative logarithm of the hydrogen ion concentration: ph = - log [H + ] The Henderson-Hasselbalch equation provides a convenient way to think about buffers and ph: ph = pka + log[a-] / [HA] If one were examining the dissociation of acetic acid, the Henderson- Hasselbalch relationship, then, would be: ph = pka + log[ch3coo - ] / [CH3COOH]

3 The Henderson-Hasselbalch equation can be used to determine if an aqueous solution of a conjugate acid/base pair is functioning as a buffer. If the concentration of the weak acid is equal to that of its conjugate base, the ratio of these two components is one. When this is the case, the Henderson-Hasselbalch equation reduces to ph = pka because the log(1) is equal to zero. When the ph of the solution is equal to the pka of the ionizing group, the solution is functioning at maximum buffering capacity (best buffer). An aqueous solution of a conjugate acid/base pair functions as a good buffer when the ratio of the conjugate base to weak acid ranges from 1:9 to 9:1. Substituting these ratios into the Henderson-Hasselbalch equation, one finds that this aqueous solution functions as a good buffer when the ph of the solution is within approximately one ph unit of the ionizing group s pka. ph = pka + 1 because the log (1/9) is and the log of (9/1) is Using the Henderson-Hasselbalch Equation Example :- How would you prepare 10mL of a 0.01M phosphate buffer, ph 7.40, from stock solutions of 0.10M KH 2 PO 4 and 0.25M K 2 HPO 4? pka of KH 2 PO 4 = The following approach may be helpful in solving this type of buffer problem in which both the conjugate acid and base are added separately. Please note that the numbers are not rounded off until the very end and are rounded based on the limits of the pipets, cylinders, etc. that are required to accurately measure the calculated volumes. 1. Use the Henderson Hasselbalch equation to find the ratio of A - to HA. ph = pka + log [A - ] / [HA] 7.40 = log [A - ] / [HA] 0.20 = log [A - ] / [HA] = [A - ] / [HA]* *Since [A - ] / [HA] = , we can say that [A - ] / [HA] = / 1. In this case [A - ] = ; [HA] = Calculate the decimal fraction (part/whole) of each buffer component.

4 A - = / ( ) = / = HA = / = Find the molarity (M) of each component in the buffer by simply multiplying the molarity of the buffer by the decimal fraction of each component. M A - = 0.01M x = M M HA = 0.01M x = M 4. Calculate the moles of each component in the buffer. Moles = Molarity x Liters of buffer moles A - = M x 0.01L = x 10-5 moles moles HA = M x 0.01L = x 10-5 moles 5. Calculate the volume of each stock solution required to make the buffer Liters of stock = moles of the buffer component / Molarity of the stock L A - = x 10-5 moles / 0.25 M = x 10-4 L = 245μL L HA = x 10-5 moles / 0.10 M = x 10-4 L = 387μL 6. To prepare this buffer, one would use appropriately-sized pipets to measure and transfer each component to a 10mL volumetric flask and bring the solution to volume with dh 2 O. Hydrolysis of Salt Salt : an ionic compound, the product of an acid base neutralization reaction: acid + base water + a salt HCl + NaOH H 2 O + NaCl One way to predict the behavior of a salt in water. A salt may be thought of as the product of a reaction between an acid and a base. 1. When the parent acid and base are strong, a water solution of the salt is neutral. 2. When a salt is formed from the reaction between a weak acid and a strong base, a water solution of that salt will be basic. 3. When a salt is formed from a strong acid and a weak base, a water solution of the salt will be acidic.

5 4. When a salt is formed from a weak acid and a weak base, a water solution of the salt could be acidic, basic or neutral depending on the nature of the ions. 1-Hydrolysis of the Salt of Strong Acid and Strong Base The strength of the acid is determined by how far the equilibrium lies to the right. Qualitatively, this may be judged by the K a of the acid. A large K a indicates a strong acid; a small K a indicates a weak acid. Strong acids, such as HCl, have K a values in the vicinity of infinity. This implies that the dissociation of HCl is virtually complete, and the equilibrium lies completely to the right, therefore, the concentration of the acid equals the concentration of hydronium ions produced. strong bases, such as NaOH, will dissociate completely. The concentration of OH - in solution will be equal to the concentration of the strong base. A typical strong acid problem might be: What is the ph of a M HCl solution? Since HCl is a strong acid, the hydronium ion concentration will be equal to the HCl concentration: [H 3 O + ] = M The ph can be found by taking the negative log of the hydronium ion concentration: ph = -log[h 3 O + ] = -log(0.010) = 2.00 A typical strong base problem might be: What is the ph of a M NaOH solution? Since NaOH is a strong base, the hydroxide ion concentration will be equal to the NaOH concentration: [OH - ] = M The ph can be found by first finding the poh by taking the negative log of the hydroxide ion concentration, and then converting the ph to poh. To find the poh: poh = -log[oh - ] = -log(0.010) = 2.00 The ph can then be calculated from the equation ph + poh = 14: ph = = 12.00

6 2- Hydrolysis of the Salt of Weak Acid and Strong Base This salt will hydrolyze to form a basic solution. The salt sodium acetate will ionize into sodium ions and acetate ions. The sodium ion does not undergo hydrolysis but the acetate ion will react with free hydrogen ions forming acetic acid. Na + C 2 H 3 O HOH <====> HC 2 H 3 O 2 + Na + OH This reaction causes a shift in the [H ]/[OH ] by removing [H ]. This salt is classified as a basic salt because the acetate ion, by definition, is a weak Bronsted-Lowry base (proton acceptor). The solution of such a salt is basic in nature. The anion of the salt is reactive. It reacts with water to form a weak acid and OH - ions. A - + H 2 O; HA + OH - Weak acid for example, the salt CH 3 COONa. It ionises in water completely to give CH 3 COO - and Na + ions. CH 3 COO - ions react with water to form a weak acid, CH 3 COOH and OH - ions. CH 3 COO - + H 2 O CH 3 COOH + OH - C(1-x) Cx Cx Thus, OH - ion concentration increases, the solution becomes alkaline. Applying law of mass action, K h = [CH 3 COOH][OH - ]/[CH 3 CO - ] = (Cx Cx)/C(1-x) = (Cx 2 )/(1-x) )... (i) Other equations present in the solution are: CH 3 COOH CH 3 COO - + H +, K a = [CH 3 COO - ][H + ]/[CH 3 COOH]... (ii) H 2 O H + + OH -, K w = [H + ][OH - ]... (iii) From eqs. (ii) and (iii), log [OH - ] = log K w - log K a + log[salt]/[acid] -poh = -pk w + pk a + log[salt]/[acid]

7 pk w - poh = pk a + log[salt]/[acid] ph = pk a + log[salt]/[acid] Considering eq. (i) again, K h = cx 2 /(1-x) or K h = Ch 2 /(1-h) When h is very small, (1-h) 1 or h 2 = K h /C or h = K h /C [OH - ] = h C = (CK h ) = (C*K w /K a ) [H + ] = K w /[OH - ] = K w / (C*K w /K a ) = (K a *K w )/K c -log [H + ] = -1/2log K w - 1/2log K a + 1/2log C ph = 1/2pK w + 1/2pK a + 1/2log C = 7 + 1/2pK a + 1/2log C. 3- Hydrolysis of the Salt of a Strong Acid and a Weak Base The solution of such a salt is acidic in nature. The cation of the salt which has come from weak base is reactive. It reacts with water to form a weak base and H + ions. B + + H 2 O BOH + H + Weak base Consider, for example, NH 4 Cl. It ionises in water completely into NH 4 and Cl ions. ions react with water to form a weak base (NH 4 OH) and H + ions. NH H 2 O NH 4 OH + H + C(1-x) Cx Cx Thus, hydrogen ion concentration increases and the solution becomes acidic. Applying law of mass action,

8 K h = [H x ][NH 4 OH]/[NH 4 + ]=(Cx.Cx)/C(1-x) = (x 2 C)/((1-x))... (i) where C is the concentration of salt and x the degree of hydrolysis. Other equilibria which exist in solution are NH 4 OH NH OH -, K b = [NH + 4][OH - ]/[NH 4 Oh]... (ii) H 2 O H + + OH -, K b = [H + ][H - ]... (iii) From eqs. (II) and (iii) K w /K b =[H + ][NH 4 OH]/[NH 4 + ] =K h... (iv) [H + ] = [H + ][NH 4 + ]/[NH 4 OH] = K w /K b [NH 4 + ]/[NH 4 OH] log [H + ] = log K w - log K b + log[salt]/[base] -ph = -pk w + pk b + log[salt]/[base] pk w - ph = pk b + log[salt]/[base] poh = pk b + log[salt]/[base] Relation between Hydrolysis constant and Degree of hydrolysis The extent to which hydrolysis proceeds is expressed as the degree of hydrolysis and is defined as the fraction of one mole of the salt that is hydrolysed when the equilibrium has been attained. It is generally expressed as h or x. h = (Amount of salt hydrolysed)/(total salt taken) Considering again eq. (i), K h = x 2 C/(1-x) or K h = h 2 C/(1-h) When h is very small (1-h) 1, H 2 = K h 1/c or h = (K h /C) = (K w /K b * C) [H + ] = h C = (C*K h )/K b

9 log [H + ] = 1/2 log K w + 1 1/2log C - 1/2log K b ph = 1/2pK w - 1/2 log C - 1/2 pk b = 7-1/2 pk b - 1/2log C 4-Hydrolysis of the Salt of Weak Acid and a Weak Base The ions of this type of salt will hydrolyze to form a solution that may be acidic, basic, or neutral, depending on the strength (ionization constant) of the weak acid and weak base that formed the salt. If the ionization constant of the weak acid is greater Maximum hydrolysis occurs in the case of such a salt as both the cation and anion are reactive and react with water to produce H + and OFT ions. The solution is generally neutral but it can be either slightly acidic or slightly alkaline if both the reactions take place with slightly different rates. Consider, for example, the salt CH 3 COONH 4. It gives CH 3 COO - and ions in solution. Both react with water. Other equilibria which exist in solution are: CH 3 COOH CH 3 COO - + H +, K a = [CH 3 COO - ][H + ]/[CH 3 COOH]... (i) NH 4 OH NH OH -, Kb = [NH + 4] [OH - ]/[NH 4 OH]... (ii) H 2 O H + + OH -, K w = [H + ][OH - ]... (iii) From Eqs. (i), (ii) and (iii), K h = Kw/K a.k b = [CH 3 COOH][NH 4 OH]/[CH 3 COO - ][NH + 4]... (iv) Let C be the concentration and h be the degree of hydrolysis

10 K h = h 2 /(1-h) 2 When h is small, (1-h) 1. K h = h 2 h = Kh = K w /K a* K b [H + ] K a h = K a K w /K a* K b = K w * K a /K b -log [H + ] = -1/2log K a - 1/2log K w + 1/2log K b ph = 1/2pK a + 1/2pK w - 1/2pK b = 7 + 1/2pK a - 1/2pK b When pk a = pk b, ph = 7, i.e., solution will be neutral in nature. When pk a > pk b. The solution will be alkaline as the acid will be slightly weaker than base and ph value will be more than 7. In case pk a < pk b, the solution will be acidic as the acid is relatively stronger than base and ph will be less than 7.

3 The Preparation of Buffers at Desired ph

3 The Preparation of Buffers at Desired ph 3 The Preparation of Buffers at Desired ph Objectives: To become familiar with operating a ph meter, and to learn how to use the Henderson-Hasselbalch equation to make buffer solutions at a desired ph

More information

Q.1 Classify the following according to Lewis theory and Brønsted-Lowry theory.

Q.1 Classify the following according to Lewis theory and Brønsted-Lowry theory. Acid-base A4 1 Acid-base theories ACIDS & BASES - IONIC EQUILIBRIA 1. LEWIS acid electron pair acceptor H, AlCl 3 base electron pair donor NH 3, H 2 O, C 2 H 5 OH, OH e.g. H 3 N: -> BF 3 > H 3 N BF 3 see

More information

ph: Measurement and Uses

ph: Measurement and Uses ph: Measurement and Uses One of the most important properties of aqueous solutions is the concentration of hydrogen ion. The concentration of H + (or H 3 O + ) affects the solubility of inorganic and organic

More information

Q.1 Classify the following according to Lewis theory and Brønsted-Lowry theory.

Q.1 Classify the following according to Lewis theory and Brønsted-Lowry theory. Acid-base 2816 1 Acid-base theories ACIDS & BASES - IONIC EQUILIBRIA LEWIS acid electron pair acceptor H +, AlCl 3 base electron pair donor NH 3, H 2 O, C 2 H 5 OH, OH e.g. H 3 N: -> BF 3 > H 3 N + BF

More information

Chapter 17. The best buffer choice for ph 7 is NaH 2 PO 4 /Na 2 HPO 4. 19)

Chapter 17. The best buffer choice for ph 7 is NaH 2 PO 4 /Na 2 HPO 4. 19) Chapter 17 2) a) HCl and CH 3 COOH are both acids. A buffer must have an acid/base conjugate pair. b) NaH 2 PO 4 and Na 2 HPO 4 are an acid/base conjugate pair. They will make an excellent buffer. c) H

More information

Review for Solving ph Problems:

Review for Solving ph Problems: Review for Solving ph Problems: Acid Ionization: HA H 2 O A - H 3 O CH 3 COOH H 2 O CH 3 COO - H 3 O Base Ionization: B H 2 O BH OH - 1) Strong Acid complete dissociation [H ] is equal to original [HA]

More information

CHAPTERS 15 FAKE TEST QUESTIONS. 1. According to the Brønsted Lowry definition, which species can function both as an acid and as a base?

CHAPTERS 15 FAKE TEST QUESTIONS. 1. According to the Brønsted Lowry definition, which species can function both as an acid and as a base? You might need to know the following K values: CHAPTERS 15 FAKE TEST QUESTIONS CH 3 COOH K a = 1.8 x 10 5 Benzoic Acid K a = 6.5 x 10 5 HNO 2 K a = 4.5 x 10 4 NH 3 K b = 1.8 x 10 5 HF K a = 7.2 x 10 4

More information

Titrations. Acid-Base Indicators and Titration Curves. Shapes of Titration Curves. A titration curve is a graphical history of a titration

Titrations. Acid-Base Indicators and Titration Curves. Shapes of Titration Curves. A titration curve is a graphical history of a titration Acid-Base Indicators and Titration Curves Titrations In a titration a solution of accurately known concentration is added gradually added to another solution of unknown concentration until the chemical

More information

Acids and Bases: A Brief Review

Acids and Bases: A Brief Review Acids and : A Brief Review Acids: taste sour and cause dyes to change color. : taste bitter and feel soapy. Arrhenius: acids increase [H ] bases increase [OH ] in solution. Arrhenius: acid base salt water.

More information

ACID-BASE TITRATIONS

ACID-BASE TITRATIONS ACID-BASE TITRATIONS 1 In this exercise you will use Excel to construct titration curves for a titration between a strong acid and strong base and between a weak acid and strong base. To set up a spreadsheet

More information

Chemical equilibria Buffer solutions

Chemical equilibria Buffer solutions Chemical equilibria Buffer solutions Definition The buffer solutions have the ability to resist changes in ph when smaller amounts of acid or base is added. Importance They are applied in the chemical

More information

Note: (H 3 O + = hydronium ion = H + = proton) Example: HS - + H 2 O H 3 O + + S 2-

Note: (H 3 O + = hydronium ion = H + = proton) Example: HS - + H 2 O H 3 O + + S 2- AcidBase Chemistry Arrhenius acid: Substance that dissolves in water and provides H + ions Arrhenius base: Substance that dissolves in water and provides OH ions Examples: HCl H + and Cl Acid NaOH Na +

More information

An acid is a substance that produces H + (H 3 O + ) Ions in aqueous solution. A base is a substance that produces OH - ions in aqueous solution.

An acid is a substance that produces H + (H 3 O + ) Ions in aqueous solution. A base is a substance that produces OH - ions in aqueous solution. Chapter 8 Acids and Bases Definitions Arrhenius definitions: An acid is a substance that produces H + (H 3 O + ) Ions in aqueous solution. A base is a substance that produces OH - ions in aqueous solution.

More information

Chapter 17. How are acids different from bases? Acid Physical properties. Base. Explaining the difference in properties of acids and bases

Chapter 17. How are acids different from bases? Acid Physical properties. Base. Explaining the difference in properties of acids and bases Chapter 17 Acids and Bases How are acids different from bases? Acid Physical properties Base Physical properties Tastes sour Tastes bitter Feels slippery or slimy Chemical properties Chemical properties

More information

Chem101: General Chemistry Lecture 9 Acids and Bases

Chem101: General Chemistry Lecture 9 Acids and Bases : General Chemistry Lecture 9 Acids and Bases I. Introduction A. In chemistry, and particularly biochemistry, water is the most common solvent 1. In studying acids and bases we are going to see that water

More information

Name period Unit 9: acid/base equilibrium

Name period Unit 9: acid/base equilibrium Name period Unit 9: acid/base equilibrium 1. What is the difference between the Arrhenius and the BronstedLowry definition of an acid? Arrhenious acids give H + in water BronstedLowry acids are proton

More information

Chapter 14 - Acids and Bases

Chapter 14 - Acids and Bases Chapter 14 - Acids and Bases 14.1 The Nature of Acids and Bases A. Arrhenius Model 1. Acids produce hydrogen ions in aqueous solutions 2. Bases produce hydroxide ions in aqueous solutions B. Bronsted-Lowry

More information

Topic 18 Acids and Bases. 18.1 Exercises

Topic 18 Acids and Bases. 18.1 Exercises Topic 18 Acids and Bases 18.1 Exercises 1. Define: (a) ph The negative log of the hydrogen ion concentration in a solution. i.e. ph = log[h 3 O + ] (b) poh The negative log of hydroxide ion concentration

More information

Write the acid-base equilibria connecting all components in the aqueous solution. Now list all of the species present.

Write the acid-base equilibria connecting all components in the aqueous solution. Now list all of the species present. Chapter 16 Acids and Bases Concept Check 16.1 Chemists in the seventeenth century discovered that the substance that gives red ants their irritating bite is an acid with the formula HCHO 2. They called

More information

Copyright 2009 by Pearson Education, Inc. Upper Saddle River, New Jersey 07458 All rights reserved.

Copyright 2009 by Pearson Education, Inc. Upper Saddle River, New Jersey 07458 All rights reserved. Sample Exercise 17.1 Calculating the ph When a Common Ion is Involved What is the ph of a solution made by adding 0.30 mol of acetic acid and 0.30 mol of sodium acetate to enough water to make 1.0 L of

More information

Acid-Base Chemistry. Brønsted-Lowry Acids & Bases

Acid-Base Chemistry. Brønsted-Lowry Acids & Bases Acid-Base Chemistry ν There are a couple of ways to define acids and bases ν Brønsted-Lowry acids and bases ν Acid: H + ion donor ν Base: H + ion acceptor ν Lewis acids and bases ν Acid: electron pair

More information

We remember that molarity (M) times volume (V) is equal to moles so this relationship is the definition of the equivalence point.

We remember that molarity (M) times volume (V) is equal to moles so this relationship is the definition of the equivalence point. Titrations Titration - a titration is defined as the determination of the amount of an unknown reagent (analyte) through the use of a known amount of another reagent (titrant) in an essentially irreversible

More information

Acids and Bases. Chapter 16

Acids and Bases. Chapter 16 Acids and Bases Chapter 16 The Arrhenius Model An acid is any substance that produces hydrogen ions, H +, in an aqueous solution. Example: when hydrogen chloride gas is dissolved in water, the following

More information

UNIT (6) ACIDS AND BASES

UNIT (6) ACIDS AND BASES UNIT (6) ACIDS AND BASES 6.1 Arrhenius Definition of Acids and Bases Definitions for acids and bases were proposed by the Swedish chemist Savante Arrhenius in 1884. Acids were defined as compounds that

More information

Chapter 14: Acids and Bases

Chapter 14: Acids and Bases Ch 14 Page 1 Chapter 14: Acids and Bases Properties of Acids Sour taste React with some metals Turns blue litmus paper red React with bases Some Common Acids HCl, hydrochloric acid H 2 SO 4, sulfuric acid

More information

4. Acid Base Chemistry

4. Acid Base Chemistry 4. Acid Base Chemistry 4.1. Terminology: 4.1.1. Bronsted / Lowry Acid: "An acid is a substance which can donate a hydrogen ion (H+) or a proton, while a base is a substance that accepts a proton. B + HA

More information

Since we will be dealing with aqueous acid and base solution, first we must examine the behavior of water.

Since we will be dealing with aqueous acid and base solution, first we must examine the behavior of water. Acids and Bases Know the definition of Arrhenius, Bronsted-Lowry, and Lewis acid and base. Autoionization of Water Since we will be dealing with aqueous acid and base solution, first we must examine the

More information

Chapter 9 Lecture Notes: Acids, Bases and Equilibrium

Chapter 9 Lecture Notes: Acids, Bases and Equilibrium Chapter 9 Lecture Notes: Acids, Bases and Equilibrium Educational Goals 1. Given a chemical equation, write the law of mass action. 2. Given the equilibrium constant (K eq ) for a reaction, predict whether

More information

This value, called the ionic product of water, Kw, is related to the equilibrium constant of water

This value, called the ionic product of water, Kw, is related to the equilibrium constant of water HYDROGEN ION CONCENTRATION - ph VALUES AND BUFFER SOLUTIONS 1. INTRODUCTION Water has a small but definite tendency to ionise. H 2 0 H + + OH - If there is nothing but water (pure water) then the concentration

More information

Volumetric Analysis. Lecture 5 Experiment 9 in Beran page 109 Prelab = Page 115

Volumetric Analysis. Lecture 5 Experiment 9 in Beran page 109 Prelab = Page 115 Volumetric Analysis Lecture 5 Experiment 9 in Beran page 109 Prelab = Page 115 Experimental Aims To prepare and standardize (determine concentration) a NaOH solution Using your standardized NaOH calculate

More information

QUESTION (2012:3) (a) (i) Complete the table below showing the conjugate acids and bases. CO 3 H 2 O OH HCN CN -

QUESTION (2012:3) (a) (i) Complete the table below showing the conjugate acids and bases. CO 3 H 2 O OH HCN CN - QUESTION (2012:3) (i) Complete the table below showing the conjugate acids and bases. Conjugate acid Conjugate base - HCO 3 2 CO 3 H 2 O OH HCN CN - (ii) HPO 4 2 (aq) Write equations for the reactions

More information

Notes on Unit 4 Acids and Bases

Notes on Unit 4 Acids and Bases Ionization of Water DEMONSTRATION OF CONDUCTIVITY OF TAP WATER AND DISTILLED WATER Pure distilled water still has a small conductivity. Why? There are a few ions present. Almost all the pure water is H

More information

TOPIC 11: Acids and Bases

TOPIC 11: Acids and Bases TOPIC 11: Acids and Bases ELECTROLYTES are substances that when dissolves in water conduct electricity. They conduct electricity because they will break apart into Ex. NaCl(s)! Na + (aq) + Cl - (aq), and

More information

ACID-BASE TITRATIONS: DETERMINATION OF CARBONATE BY TITRATION WITH HYDROCHLORIC ACID BACKGROUND

ACID-BASE TITRATIONS: DETERMINATION OF CARBONATE BY TITRATION WITH HYDROCHLORIC ACID BACKGROUND #3. Acid - Base Titrations 27 EXPERIMENT 3. ACID-BASE TITRATIONS: DETERMINATION OF CARBONATE BY TITRATION WITH HYDROCHLORIC ACID BACKGROUND Carbonate Equilibria In this experiment a solution of hydrochloric

More information

p3 Recognizing Acid/Base Properties when p11 Recognizing Basic versus Nonbasic

p3 Recognizing Acid/Base Properties when p11 Recognizing Basic versus Nonbasic General Chemistry II Jasperse Acid-Base Chemistry. Extra Practice Problems 1 General Types/Groups of problems: Conceptual Questions. Acids, Bases, and p1 K b and pk b, Base Strength, and using K b or p7-10

More information

Chapter 16 Acid-Base Equilibria

Chapter 16 Acid-Base Equilibria Chapter 16 Acid-Base Equilibria Learning goals and key skills: Understand the nature of the hydrated proton, represented as either H + (aq) or H 3 O + (aq) Define and identify Arrhenuis acids and bases.

More information

Similarities The ph of each of these solutions is the same; that is, the [H + ] is the same in both beakers (go ahead and count).

Similarities The ph of each of these solutions is the same; that is, the [H + ] is the same in both beakers (go ahead and count). Compare 1 L of acetate buffer solution (0.50 mol of acetic acid and 0.50 mol sodium acetate) to 1 L of HCl solution AcO - AcO - H+ Cl - AcO - AcO - Cl - Cl - AcO - Cl - Cl - Cl - Cl - AcO - AcO - AcO -

More information

Chem 116 POGIL Worksheet - Week 10 - Solutions Weak Acid and Base Equilibria

Chem 116 POGIL Worksheet - Week 10 - Solutions Weak Acid and Base Equilibria Chem 116 POGIL Worksheet - Week 10 - Solutions Weak Acid and Base Equilibria Key Questions 1. A 0.0100 M solution of a weak acid HA has a ph of 2.60. What is the value of K a for the acid? [Hint: What

More information

ACID-BASE REACTIONS/ THE PH CONCEPT.

ACID-BASE REACTIONS/ THE PH CONCEPT. Dr Mike Lyons School of Chemistry Trinity College Dublin. melyons@tcd.ie ACID-BASE REACTIONS/ THE PH CONCEPT. Chemistry Preliminary Course 2011 1 Lecture topics. 2 lectures dealing with some core chemistry

More information

Chemistry 201. Practical aspects of buffers. NC State University. Lecture 15

Chemistry 201. Practical aspects of buffers. NC State University. Lecture 15 Chemistry 201 Lecture 15 Practical aspects of buffers NC State University The everyday ph scale To review what ph means in practice, we consider the ph of everyday substances that we know from experience.

More information

Topic 5. Acid and Bases

Topic 5. Acid and Bases Topic 5 5-1 Acid and Bases Acid and Bases 5-2 There are a number definitions for aicd and bases, depending on what is convenient to use in a particular situation: Arrhenius and Ostwald: Theory of electrolyte

More information

CHM1 Review for Exam 12

CHM1 Review for Exam 12 Topics Solutions 1. Arrhenius Acids and bases a. An acid increases the H + concentration in b. A base increases the OH - concentration in 2. Strong acids and bases completely dissociate 3. Weak acids and

More information

Acid/Base Definition. Acid/Base Reactions. Major vs. Minor Species. Terms/Items you Need to Know. you need to memorize these!!

Acid/Base Definition. Acid/Base Reactions. Major vs. Minor Species. Terms/Items you Need to Know. you need to memorize these!! Acid/Base Reactions some covalent compounds have weakly bound H atoms and can lose them to water (acids) some compounds produce OH in water solutions when they dissolve (bases) acid/base reaction are very

More information

Acid/base Definitions. Acid/Base Definitions. Acid / Base Chemistry. Acid/Base Definitions. Identifying Acids and Bases

Acid/base Definitions. Acid/Base Definitions. Acid / Base Chemistry. Acid/Base Definitions. Identifying Acids and Bases Acids Identifying Acids and Bases Acid (anhydrides) contains H+ ions as the cation, with and other element as the anion Non-metal oxide H2SO4 HI P2O5 Bases Base (anhydrides) Contains OH- as the anion Combined

More information

6) Which compound is manufactured in larger quantities in the U.S. than any other industrial chemical?

6) Which compound is manufactured in larger quantities in the U.S. than any other industrial chemical? MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Which statement concerning Arrhenius acid-base theory is not correct? A) Acid-base reactions must

More information

Acid-Base (Proton-Transfer) Reactions

Acid-Base (Proton-Transfer) Reactions Acid-Base (Proton-Transfer) Reactions Chapter 17 An example of equilibrium: Acid base chemistry What are acids and bases? Every day descriptions Chemical description of acidic and basic solutions by Arrhenius

More information

Auto-ionization of Water

Auto-ionization of Water 2H 2 O H 3 O + + OH Hydronium ion hydroxide ion Q: But how often does this happen? This is the fundamental concept of all acid-base chemistry In pure water, how much of it is water and how much is ions?

More information

Acid-Base Equilibrium

Acid-Base Equilibrium AcidBaseEquil 1 Acid-Base Equilibrium See AqueousIons in Chemistry 1110 online notes for review of acid-base fundamentals! Acid- Base Reaction in Aqueous Salt Solutions Recall that use [ ] to mean concentration

More information

Worksheet 23 Strong Acid/Strong Base Titrations

Worksheet 23 Strong Acid/Strong Base Titrations Worksheet 2 Strong Acid/Strong Base Titrations A. Initial ph This is always determined based solely on the initial concentration of the acid or base being titrated. Every mole of acid or base will produce

More information

Chapter 19: Acids and Bases Homework Packet (50 pts) Name: Score: / 50

Chapter 19: Acids and Bases Homework Packet (50 pts) Name: Score: / 50 Chapter 19: Acids and Bases Homework Packet (50 pts) Topic pg Section 19.1 1-3 Section 19.2 3-6 Section 19.3 6-7 Section 19.4 8 Naming Acids 9 Properties of Acids/Bases 10-11 Conjugate Acid/Base Pairs

More information

CHEM 1212 Test II. MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

CHEM 1212 Test II. MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. CHEM 1212 Test II MULTIPLE CHOICE. Choose the one alternative that est completes the statement or answers the question. 1) At 1000 K, the equilirium constant for the reaction is K p = 0.013. 2NO (g) +

More information

Chapter 16: Acid-Base and Solubility Equilibria: Reactions in Soil and Water

Chapter 16: Acid-Base and Solubility Equilibria: Reactions in Soil and Water Chapter 16: Acid-Base and Solubility Equilibria: Reactions in Soil and Water Problems: 16.2-16.86 16.1 ACIDS AND BASES: THE BRØNSTED-LOWRY MODEL PROPERTIES OF ACIDS & BASES Acids produce hydrogen ions,

More information

Q1: What is the ph Scale? Q6: As acids become more acidic, their ph values

Q1: What is the ph Scale? Q6: As acids become more acidic, their ph values Q1: What is the ph Scale? Q6: As acids become more acidic, their ph values increase or decrease? Q2: The range of values of the ph scale is: Q7: As bases become more alkaline, their ph values increase

More information

NH 3 + H 2 O + OH - NH 4. Acid-Base Concepts -- Chapter 15 + H + Conjugate Acid-Base Pairs: - H + base. acid

NH 3 + H 2 O + OH - NH 4. Acid-Base Concepts -- Chapter 15 + H + Conjugate Acid-Base Pairs: - H + base. acid Acid-Base Concepts -- Chapter 15 1. Arrhenius Acid-Base Concept (last semester) Acid: H+ supplier Base: OH- supplier 2. Brønsted-Lowry Acid-Base Concept (more general) (a) Definition (H+ transfer) Acid:

More information

General Chemistry II Chapter 20

General Chemistry II Chapter 20 1 General Chemistry II Chapter 0 Ionic Equilibria: Principle There are many compounds that appear to be insoluble in aqueous solution (nonelectrolytes). That is, when we add a certain compound to water

More information

CHAPTER 16: ACIDS AND BASES

CHAPTER 16: ACIDS AND BASES CHAPTER 16: ACIDS AND BASES Active Learning: 4, 6, 14; End-of-Chapter Problems: 2-25, 27-58, 66-68, 70, 75-77, 83, 90-91, 93-104 Chapter 15 End-of-Chapter Problems: 69-74, 125, 129, 133 16.1 ACIDS AND

More information

Acid-Base Titrations Using ph Measurements

Acid-Base Titrations Using ph Measurements Acid-Base Titrations Using ph Measurements Introduction According to the Brønsted Lowry definition, an acid is a substance that donates a hydrogen ion and a base is a substance which will accept a hydrogen

More information

Topic 8 Acids and bases 6 hours

Topic 8 Acids and bases 6 hours Topic 8 Acids and bases 6 hours Hydronium ion (H3O + ) = more stable form of hydrogen ion (H + ) H + + H2O H3O + 8.1 Theories of acids and bases 2 hours 1. Arrhenius H-X / M-OH ACID a substance that dissociates

More information

Experiment 17: Potentiometric Titration

Experiment 17: Potentiometric Titration 1 Experiment 17: Potentiometric Titration Objective: In this experiment, you will use a ph meter to follow the course of acid-base titrations. From the resulting titration curves, you will determine the

More information

Equilibria Involving Acids & Bases

Equilibria Involving Acids & Bases Week 9 Equilibria Involving Acids & Bases Acidic and basic solutions Self-ionisation of water Through reaction with itself: The concentration of water in aqueous solutions is virtually constant at about

More information

Acid-Base Titrations. Setup for a Typical Titration. Titration 1

Acid-Base Titrations. Setup for a Typical Titration. Titration 1 Titration 1 Acid-Base Titrations Molarities of acidic and basic solutions can be used to convert back and forth between moles of solutes and volumes of their solutions, but how are the molarities of these

More information

AP FREE RESPONSE QUESTIONS ACIDS/BASES

AP FREE RESPONSE QUESTIONS ACIDS/BASES AP FREE RESPONSE QUESTIONS ACIDS/BASES 199 D A chemical reaction occurs when 100. milliliters of 0.200molar HCl is added dropwise to 100. milliliters of 0.100molar Na 3 P0 solution. (a) Write the two net

More information

ph. Weak acids. A. Introduction

ph. Weak acids. A. Introduction ph. Weak acids. A. Introduction... 1 B. Weak acids: overview... 1 C. Weak acids: an example; finding K a... 2 D. Given K a, calculate ph... 3 E. A variety of weak acids... 5 F. So where do strong acids

More information

Acids and Bases HW PSI Chemistry

Acids and Bases HW PSI Chemistry Acids and Bases HW PSI Chemistry Name 1) According to the Arrhenius concept, an acid is a substance that. A) is capable of donating one or more H + B) causes an increase in the concentration of H + in

More information

Properties of Aqueous Solutions of Acids and Bases. CHAPTER 10 Acids, Bases and Salts. Properties of Aqueous Solutions of Acids and Bases

Properties of Aqueous Solutions of Acids and Bases. CHAPTER 10 Acids, Bases and Salts. Properties of Aqueous Solutions of Acids and Bases CAPTER Acids, Bases and Salts Properties of Aqueous Solutions of Acids and Bases Strong and Weak Acids Acids are substances that generate in aqueous solutions. Strong acids ionize 0% in water. That is,

More information

AP Chemistry Summary Acids, Bases and Buffers Definitions:

AP Chemistry Summary Acids, Bases and Buffers Definitions: AP Chemistry Summary Acids, Bases and Buffers Definitions: Arrhenius: Acid - Produces H + ions in solution HCl H + (aq) + Cl - (aq) Base - Produces OH - ions in solution NaOH Na + (aq) + OH - (aq) Dissociation

More information

Titration curves. Strong Acid-Strong Base Titrations

Titration curves. Strong Acid-Strong Base Titrations Titration curves A titration is a procedure for carrying out a chemical reaction between two solutions by the controlled addition from a buret of one solution (the titrant) to the other, allowing measurements

More information

Chapter 15 Acids and Bases. Fu-Yin Hsu

Chapter 15 Acids and Bases. Fu-Yin Hsu Chapter 15 Acids and Bases Fu-Yin Hsu Stomach Acid and Heartburn The cells that line your stomach produce hydrochloric acid. To kill unwanted bacteria To help break down food To activate enzymes that break

More information

Chapter 2 Polar Covalent Bonds: Acids and Bases

Chapter 2 Polar Covalent Bonds: Acids and Bases John E. McMurry www.cengage.com/chemistry/mcmurry Chapter 2 Polar Covalent Bonds: Acids and Bases Modified by Dr. Daniela R. Radu Why This Chapter? Description of basic ways chemists account for chemical

More information

Chemical Reactions in Water Ron Robertson

Chemical Reactions in Water Ron Robertson Chemical Reactions in Water Ron Robertson r2 f:\files\courses\1110-20\2010 possible slides for web\waterchemtrans.doc Properties of Compounds in Water Electrolytes and nonelectrolytes Water soluble compounds

More information

CHAPTER 18 ACID-BASE EQUILIBRIA

CHAPTER 18 ACID-BASE EQUILIBRIA CHAPTER 18 ACID-BASE EQUILIBRIA 18.1 The Arrhenius definition classified substances as being acids or bases by their behavior in the solvent water. 18. All Arrhenius acids contain hydrogen and produce

More information

Acid Dissociation Constants and the Titration of a Weak Acid

Acid Dissociation Constants and the Titration of a Weak Acid Acid Dissociation Constants and the Titration of a Weak Acid One of the most important applications of equilibria is the chemistry of acids and bases. The Brønsted-Lowry acid-base theory defines an acid

More information

Health Science Chemistry I CHEM-1180 Experiment No. 12 Acids, Bases, ph, Hydrolysis and Buffers (Revised 05/27/2015)

Health Science Chemistry I CHEM-1180 Experiment No. 12 Acids, Bases, ph, Hydrolysis and Buffers (Revised 05/27/2015) Health Science Chemistry I CHEM-1180 Experiment No. 12 Acids, Bases, ph, Hydrolysis and Buffers (Revised 05/27/2015) Introduction Hydrogen Ion Concentration The acidity of aqueous solutions and its measurement

More information

Ch 8.5 Solution Concentration Units % (m/m or w/w) = mass of solute x 100 total mass of solution mass of solution = mass solute + mass solvent

Ch 8.5 Solution Concentration Units % (m/m or w/w) = mass of solute x 100 total mass of solution mass of solution = mass solute + mass solvent 1 Ch 8.5 Solution Concentration Units % (m/m or w/w) = mass of solute x 100 total mass of solution mass of solution = mass solute + mass solvent % (v/v) = volume of solute x 100 volume of solution filled

More information

Buffer solutions. Division of Radiooncology, Deutsches Krebsforschungszentrum, 69120 Heidelberg, Germany

Buffer solutions. Division of Radiooncology, Deutsches Krebsforschungszentrum, 69120 Heidelberg, Germany Buffer solutions WOLF D. KUHLMANN, M.D. Division of Radiooncology, Deutsches Krebsforschungszentrum, 69120 Heidelberg, Germany Aqueous buffer solutions and acid-base reactions Buffer solutions have the

More information

Chapter 8, Acid-base equilibria

Chapter 8, Acid-base equilibria Chapter 8, Acid-base equilibria Road map of acid-base equilibria On first encounter, the study of acid-base equilibria is a little like a strange land with seemingly confusing trails that make passage

More information

Equilibrium Constants The following equilibrium constants will be useful for some of the problems.

Equilibrium Constants The following equilibrium constants will be useful for some of the problems. 1 CH302 Exam 4 Practice Problems (buffers, titrations, Ksp) Equilibrium Constants The following equilibrium constants will be useful for some of the problems. Substance Constant Substance Constant HCO

More information

Electrical Conductivity of Aqueous Solutions

Electrical Conductivity of Aqueous Solutions Electrical Conductivity of Aqueous Solutions PRE-LAB ASSIGNMENT: Reading: Chapter 4.-4.3 in Brown, LeMay, Bursten & Murphy.. Using Table in this handout, determine which solution has a higher conductivity,.

More information

Unit Two: Acids and Bases

Unit Two: Acids and Bases Section One: Theoretical Stuff Unit Two: Acids and Bases The concept of acids and bases has existed for centuries. We can discuss them two ways, operational definitions and theoretical definitions. 1.

More information

Chem 1B Saddleback College Dr. White 1. Experiment 8 Titration Curve for a Monoprotic Acid

Chem 1B Saddleback College Dr. White 1. Experiment 8 Titration Curve for a Monoprotic Acid Chem 1B Saddleback College Dr. White 1 Experiment 8 Titration Curve for a Monoprotic Acid Objectives To learn the difference between titration curves involving a strong acid with a strong base and a weak

More information

Ch 15: Acids and Bases

Ch 15: Acids and Bases Ch 15: Acids and Bases A c i d s a n d B a s e s C h 1 5 P a g e 1 Homework: Read Chapter 15 Work out sample/practice exercises in the sections, Bonus problems: 39, 41, 49, 63, 67, 83, 91, 95, 99, 107,

More information

Experiment 6 Titration II Acid Dissociation Constant

Experiment 6 Titration II Acid Dissociation Constant 6-1 Experiment 6 Titration II Acid Dissociation Constant Introduction: An acid/base titration can be monitored with an indicator or with a ph meter. In either case, the goal is to determine the equivalence

More information

Spectrophotometric Determination of the pka of Bromothymol Blue

Spectrophotometric Determination of the pka of Bromothymol Blue Spectrophotometric Determination of the pka of Bromothymol Blue INRODUCION cidbase indicators are compounds that are simply weak acids (or bases) that exhibit different colors depending on whether they

More information

Chapter 16 Acid-Base Equilibria. Most solutions that occur in nature are slightly acidic. One reason for this is that when carbon

Chapter 16 Acid-Base Equilibria. Most solutions that occur in nature are slightly acidic. One reason for this is that when carbon Chapter 16 Acid-Base Equilibria Most solutions that occur in nature are slightly acidic. One reason for this is that when carbon dioxide dissolves in water, it forms carbonic acid, H 2 CO 3. Basic solutions

More information

Answer Key, Problem Set 5 (With explanations)--complete

Answer Key, Problem Set 5 (With explanations)--complete Chemistry 122 Mines, Spring 2016 Answer Key, Problem Set 5 (With explanations)complete 1. NT1; 2. NT2; 3. MP; 4. MP (15.38); 5. MP (15.40); 6. MP (15.42); 7. NT3; 8. NT4; 9. MP; 10. NT5; 11. NT6; 12. MP;

More information

To see how this data can be used, follow the titration of hydrofluoric acid against sodium hydroxide below. HF (aq) + NaOH (aq) H2O (l) + NaF (aq)

To see how this data can be used, follow the titration of hydrofluoric acid against sodium hydroxide below. HF (aq) + NaOH (aq) H2O (l) + NaF (aq) Weak Acid Titration v120413 You are encouraged to carefully read the following sections in Tro (2 nd ed.) to prepare for this experiment: Sec 4.8, pp 158-159 (Acid/Base Titrations), Sec 16.4, pp 729-43

More information

Suggested Problems: p. 625-627 #58, 59, 65, 69, 74, 80, 85, 86, 90, 92, 93, 98, 99

Suggested Problems: p. 625-627 #58, 59, 65, 69, 74, 80, 85, 86, 90, 92, 93, 98, 99 Chemistry I Accelerated Study Guideline - Chapter 19 Acids, Bases and Salts ------------------------------------------------------------------------------ By the end of this unit, the skills you should

More information

Practical Lesson No 4 TITRATIONS

Practical Lesson No 4 TITRATIONS Practical Lesson No 4 TITRATIONS Reagents: 1. NaOH standard solution 0.1 mol/l 2. H 2 SO 4 solution of unknown concentration 3. Phenolphthalein 4. Na 2 S 2 O 3 standard solution 0.1 mol/l 5. Starch solution

More information

Chemistry 3202. Unit 2 Acids and Bases

Chemistry 3202. Unit 2 Acids and Bases Chemistry 3202 Unit 2 Acids and Bases Definitions of Acids and Bases An operational definition is one that is based on the observable properties, behaviours or uses of an entity. The earliest definitions

More information

1. Read P. 368-375, P. 382-387 & P. 429-436; P. 375 # 1-11 & P. 389 # 1,7,9,12,15; P. 436 #1, 7, 8, 11

1. Read P. 368-375, P. 382-387 & P. 429-436; P. 375 # 1-11 & P. 389 # 1,7,9,12,15; P. 436 #1, 7, 8, 11 SCH3U- R.H.KING ACADEMY SOLUTION & ACID/BASE WORKSHEET Name: The importance of water - MAKING CONNECTION READING 1. Read P. 368-375, P. 382-387 & P. 429-436; P. 375 # 1-11 & P. 389 # 1,7,9,12,15; P. 436

More information

EXPERIMENT 4 Acid Strength

EXPERIMENT 4 Acid Strength EXPERIMENT 4 Acid Strength Introduction Many common substances are either acids or bases. Some acids, like stomach acid are necessary for our health, while others, like sulfuric acid are dangerous and

More information

Acids and Bases. An Introduction. David A Katz Department of Chemistry Pima Community College, Tucson, AZ, USA

Acids and Bases. An Introduction. David A Katz Department of Chemistry Pima Community College, Tucson, AZ, USA Acids and Bases An Introduction David A Katz Department of Chemistry Pima Community College, Tucson, AZ, USA Properties of Acids 1. Sour taste (examples: vinegar, citric acid, lemon juice) 2. Turns litmus

More information

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. CHE 1400 - Spring 2015 - Chapter 7 Homework 7 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1)According to Arrhenius, an acid and a base will react

More information

Acids and Bases CHAPTER 12. Opening Essay

Acids and Bases CHAPTER 12. Opening Essay CHAPTER 12 Acids and Bases Opening Essay Formerly there were rather campy science-fiction television shows in which the hero was always being threatened with death by being plunged into a vat of boiling

More information

4.1 Stoichiometry. 3 Basic Steps. 4. Stoichiometry. Stoichiometry. Butane Lighter 2C 4 H 10 + 13O 2 10H 2 O + 8CO 2

4.1 Stoichiometry. 3 Basic Steps. 4. Stoichiometry. Stoichiometry. Butane Lighter 2C 4 H 10 + 13O 2 10H 2 O + 8CO 2 4. Stoichiometry 1. Stoichiometric Equations 2. Limiting Reagent Problems 3. Percent Yield 4. Limiting Reagent Problems 5. Concentrations of Solutes 6. Solution Stoichiometry 7. ph and Acid Base Titrations

More information

6 Reactions in Aqueous Solutions

6 Reactions in Aqueous Solutions 6 Reactions in Aqueous Solutions Water is by far the most common medium in which chemical reactions occur naturally. It is not hard to see this: 70% of our body mass is water and about 70% of the surface

More information

I. ACID-BASE NEUTRALIZATION, TITRATION

I. ACID-BASE NEUTRALIZATION, TITRATION LABORATORY 3 I. ACID-BASE NEUTRALIZATION, TITRATION Acid-base neutralization is a process in which acid reacts with base to produce water and salt. The driving force of this reaction is formation of a

More information

stoichiometry = the numerical relationships between chemical amounts in a reaction.

stoichiometry = the numerical relationships between chemical amounts in a reaction. 1 REACTIONS AND YIELD ANSWERS stoichiometry = the numerical relationships between chemical amounts in a reaction. 2C 8 H 18 (l) + 25O 2 16CO 2 (g) + 18H 2 O(g) From the equation, 16 moles of CO 2 (a greenhouse

More information

Neutralizing an Acid and a Base

Neutralizing an Acid and a Base Balancing Act Teacher Information Objectives In this activity, students neutralize a base with an acid. Students determine the point of neutralization of an acid mixed with a base while they: Recognize

More information