Chapter 16. Properties of Bases 5/21/2013. also known as alkalis taste bitter solutions feel slippery. change color of vegetable dyes

Size: px
Start display at page:

Download "Chapter 16. Properties of Bases 5/21/2013. also known as alkalis taste bitter solutions feel slippery. change color of vegetable dyes"

Transcription

1 Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; Bruce E. Bursten Chapter 16 John D. Bookstaver St. Charles Community College St. Peters, MO 2006, Prentice Hall, Inc. Properties of sour taste react with active metals recall the activity series (any metals above H are active ) 2 Al (s) + 6 HCl (aq) 2 AlCl 3 (aq) + 3 H 2 (g) corrosive has the ability to eat away/destroy other substances react with carbonates (containing CO 2-3 ) produce CO 2 gas marble, baking soda, chalk, limestone CaCO 3 (A) + 2 HCl (aq) CaCl 2 (aq) + CO 2 (g) + H 2 O (l) change color of vegetable dyes blue litmus paper turns red react with bases to form ionic salts (ionic compounds) Properties of also known as alkalis taste bitter solutions feel slippery Many soaps are manufactured with the use of bases change color of vegetable dyes different color than acid red litmus paper turns blue react with acids to form ionic salts (ionic compounds) This is known as neutralization 1

2 What are? There are several different ways to define the terms acid base Each definition comes from a different acid/base theory: Arrhenius Theory Brønsted-Lowry Theory Lewis Theory Arrhenius Theory Acid: when dissolved in water, the hydrogen ion concentration increases (basically, an Arrhenius acid produces H + ions) Ex) HCl (aq) H + (aq) + Cl (aq) HCl is an acid b/c it is ionized (molecular acid that is pulled apart by water) to form H + Base: when dissolved in water, the hydroxide ion concentration increases (basically, an Arrhenius base produces OH ions) Ex) NaOH (aq) Na + (aq) + OH (aq) NaOH is a base b/c it dissociates (ionic compound breaking up into its ions) to form OH Problems with Arrhenius Theory Does not explain why molecular substances, like NH 3, some ionic compounds, like Na 2 CO 3 or Na 2 O, are bases since they do not contain OH ions, they can t be considered Arrhenius bases Does not explain why molecular substances, like CO 2, dissolve in water to form acidic solutions since it doesn t even contain H + ions it can t be considered an Arrhenius acid Does not explain acid-base reactions that take place outside of aqueous solutions 2

3 Hydronium Ion: H 3 O + the H + ions produced by the acid are so reactive they cannot exist in water H + ions are just protons w/ no valence electrons!!! To be more stable, H + ions react with water molecule(s) to produce hydronium ions, H 3 O + Note: for our purposes, H + H 3 O + will be used interchangeably Brønsted-Lowry Theory The Brønsted-Lowry theory looks at the entire acid-base chemical reaction In an acid-base reaction, an H + is transferred from the acid to the base Broader, more general, definition than Arrhenius does not have to take place in aqueous solution Brønsted-Lowry & Brønsted-Lowry acids are H + donors (aka: proton donors) Must have a removable (acidic) hydrogen because of the molecular structure, often one H in the molecule is easier to transfer than others (this is known as the ionizable hydrogen ) Brønsted-Lowry bases are H + acceptors (aka: proton acceptors) Must have a lone pair/ nonbonding pair of electrons because of the molecular structure, often one atom in the molecule is more willing to accept 9 H + transfer than others 3

4 Brønsted-Lowry Acid/Base Rxns Ex) HCl (aq) + H 2 O (l) Cl (aq) + H 3 O + (aq) acid base HCl transfers an H + to H 2 O, forming H 3 O + ions water acts as base, accepting H + Ex) NH 3 (aq) + H 2 O (l) NH 4 + (aq) + OH (aq) base acid NH 3 (aq) is a Brønsted-Lowry base because NH 3 accepts an H + from H 2 O (it is also an Arrhenius base because it forms OH ) water acts as acid, donating H + Amphiprotic Molecules Amphiprotic (or amphoteric) means have qualities of both substance can act as both an acid a base depending what it is reacting with After Donated H+ Amphoteric Molecule After Accepted H+ OH H 2 O H 3 O + CO 3 2 HCO 3 H 2 CO 3 SO 4 2 HSO 4 H 2 SO 4 Brønsted-Lowry Reversible Acid-Base Reactions Brønsted-Lowry theory allows A-B rxns to be reversible (shown w/ double-sided arrows) General A-B rxn: H A + :B :A + H B + the original base has an extra H + after the reaction, so it will act as an acid in the reverse process the original acid has a lone pair of electrons after the reaction, so it will act as a base in the reverse process :A + H B + H A + :B 4

5 Conjugate Pairs In a Brønsted-Lowry Acid-Base reaction, the original base becomes an acid in the reverse reaction, the original acid becomes a base in the reverse process each reactant the product it becomes are called a conjugate pair the original base becomes the conjugate acid; the original acid becomes the conjugate base Conjugate Pairs Brønsted-Lowry Acid-Base Reactions H A + :B :A + H B + acid base conjugate conjugate base acid HCHO 2 + H 2 O CHO 2 + H 3 O + acid base conjugate conjugate base acid H 2 O + NH 3 OH + NH + 4 acid base conjugate conjugate base acid 5

6 Conjugate Pairs Practice Determine the acid, base, conjugate acid, conjugate base in the following reaction: H 2 O + H 2 SO 4 HSO 4 + H 3 O + base acid conjugate conjugate base acid Arrow Conventions chemists commonly use two kinds of arrows in reactions to indicate the degree of completion of the reactions a single arrow indicates all the reactant molecules are converted to product molecules at the end a double arrow indicates the reaction is in equillibrium. The reaction stops when some of the reactant molecules have been converted into products. Some reactant molecules remain some products molecules have formed Looks like in these notes Strong or Weak a strong acid is a strong electrolyte practically all the acid molecules ionize ( ) a strong base is a strong electrolyte practically all the base molecules form OH ions, either through dissociation or reaction with water ( ) a weak acid is a weak electrolyte only a small % of the molecules ionize ( ) a weak base is a weak electrolyte only a small % of the base molecules form OH ions ( ) 6

7 Autoionization of Water As we have seen, water is amphoteric. In pure water, a few molecules act as bases a few act as acids. about 1 out of every 10 million water molecules form ions through a process called autoionization H 2 O(l) + H 2 O(l) H 3 O + (aq) + OH (aq) all aqueous solutions contain both H 3 O + OH the concentration of H 3 O + OH are equal in pure water (which is neutral) Ion Product of Water the product of the H 3 O + OH concentrations is a constant number the number is called the ion product constant of water (K w ) At 25ºC, [H 3 O + ] [OH ] = [H + ] [OH ] = K w = 1 x if you measure one of the concentrations (H + or OH ), you can calculate the other as [H 3 O + ] increases the [OH ] must decrease so the product stays constant inversely proportional Acidic Basic Solutions all aqueous solutions contain both H + OH ions neutral solutions [H + ] = [OH ] = 1 x 10-7 acidic solutions [H + ] is greater than [OH ] [H + ] > 1 x 10-7 ; [OH ] < 1 x 10-7 basic solutions [OH ] is greater than [ 3 O + ] [OH ] > 1 x 10-7 ; [H + ] < 1 x 10-7 Be careful! We are dealing with NEGATIVE exponents. the larger the negative exponent, the SMALLER the number actually is! 7

8 Concentration Calculation Practice Calculate the [OH ] at 25ºC when the [H + ] = 1.5 x 10-9 M, determine if the solution is acidic, basic, or neutral 1.0 x M = [OH ] [H + ] 1.0 x M = [OH ] [1.5 x 10-9 M] [OH ] = 6.67 x10-6 M The solution is basic [OH ] > [H + ] ph ph is a measure of how acidic or basic a solution is ph = log [H + ]; [H + ] = 10 ph Ex) ph water = log [1.0 x 10-7 M] = 7 Similarly, [H + ] water = 10 7 = 1.0 x 10-7 M need to know the [H + ] concentration to find ph ph An acid has a higher [H + ] than pure water, so its ph is < 7 A base has a lower [H 3 O + ] than pure water, so its ph is >7 8

9 ph the lower the ph, the more acidic the solution the higher the ph, the more basic the solution 1 ph unit corresponds to a factor of 10 difference in acidity normal range 0 to 14 ph 0 is [H + ] = 1 M, ph 14 is [OH ] = 1 M ph can be negative (very acidic) or larger than 14 (very alkaline) ph of Common Substances Substance ph 1.0 M HCl M HCl 1.0 stomach acid 1.0 to 3.0 lemons 2.2 to 2.4 soft drinks 2.0 to 4.0 plums 2.8 to 3.0 apples 2.9 to 3.3 cherries 3.2 to 4.0 unpolluted rainwater 5.6 human blood 7.3 to 7.4 egg whites 7.6 to 8.0 milk of magnesia (sat d Mg(OH) 2 ) 10.5 household ammonia 10.5 to M NaOH 14 Other p Scales The p in ph tells us to take the negative log of the quantity (in this case, hydrogen ions). Some similar examples are poh = log [OH ] pk w = log K w 9

10 poh another way of expressing the acidity/basicity of a solution is poh poh = -log [OH ]; [OH ] = 10 -poh poh measures are the exact opposite of ph: poh < 7 is basic, poh > 7 is acidic poh = 7 is neutral Watch This! Because [H 3 O + ] [OH ] = K w = , we know that log [H 3 O + ] + log [OH ] = log K w = or, in other words, ph + poh = pk w = The Acid/ Base Square 10

11 Relationships: ph, poh, [H + ], [OH ] ph: [H + ]: H + H + H+ H + H+ OH OH - OH - OH - - OH - [OH - ]: poh: EQUATIONS TO REMEMBER! [H + ][OH ] = 1 x = k w ph = -log[h + ] [H + ] = 10 -ph poh = -log[oh - ] [OH ] = 10 -poh ph + poh = 14 How Do We Measure ph? For less accurate measurements, one can use Litmus paper Red paper turns blue above ~ph = 8 Blue paper turns red below ~ph = 5 An indicator 11

12 How Do We Measure ph? For more accurate measurements, one uses a ph meter, which measures the voltage in the solution. Strong You will recall that the seven strong acids are HCl, HBr, HI, HNO 3, H 2 SO 4, HClO 3, HClO 4. These are, by definition, strong electrolytes exist totally as ions in aqueous solution. For the monoprotic strong acids, [H 3 O + ] = [acid]. Strong Strong bases are the soluble hydroxides, which are the alkali metal heavier alkaline earth metal hydroxides (Ca 2+, Sr 2+, Ba 2+ ). Again, these substances dissociate completely in aqueous solution. 12

13 Dissociation Constants For a generalized acid dissociation, HA(aq) + H 2 O(l) A (aq) + H 3 O + (aq) the equilibrium expression would be K c = [H 3 O + ] [A ] [HA] This equilibrium constant is called the acid-dissociation constant, K a. Dissociation Constants The greater the value of K a, the stronger the acid. Calculating K a from the ph The ph of a 0.10 M solution of formic acid, HCOOH, at 25 C is Calculate K a for formic acid at this temperature. We know that K a = [H 3 O + ] [COO ] [HCOOH] 13

14 Calculating K a from the ph The ph of a 0.10 M solution of formic acid, HCOOH, at 25 C is Calculate K a for formic acid at this temperature. To calculate K a, we need the equilibrium concentrations of all three things. We can find [H 3 O + ], which is the same as [HCOO ], from the ph. Calculating K a from the ph ph = log [H 3 O + ] 2.38 = log [H 3 O + ] 2.38 = log [H 3 O + ] = 10 log [H3O+] = [H 3 O + ] = [H 3 O + ] = [HCOO ] Calculating K a from ph Now we can set up a table [HCOOH], M [H 3 O + ], M [HCOO ], M Initially Change At Equilibrium = =

15 Calculating K a from ph K a = [ ] [ ] [0.10] =

Chapter 16. Some Definitions. Some Definitions. What Happens When an Acid Dissolves in Water? 27/07/2014. If it can be either HCO 3 HSO 4 H 2 O

Chapter 16. Some Definitions. Some Definitions. What Happens When an Acid Dissolves in Water? 27/07/2014. If it can be either HCO 3 HSO 4 H 2 O Chemistry, The Central Science, 11th edition Theodore L. Brown, H. Eugene LeMay, Jr., Bruce E. Bursten Some Definitions Chapter 16 AP Chemistry 2014-15 North Nova Education Centre Mr. Gauthier Arrhenius

More information

Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten. Acids and Bases

Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten. Acids and Bases Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Acids and Bases Three definitions of acid Who Theory: Acid= When Arrhenius increases H + 1880

More information

Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten. Chapter 16.

Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten. Chapter 16. Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; Bruce E. Bursten Chapter 16 Some Definitions Arrhenius Acid: Substance that, when dissolved in water, increases the

More information

Chapter 15: Acids and Bases I. Chem 102 Dr. Curtis

Chapter 15: Acids and Bases I. Chem 102 Dr. Curtis Chapter 15: Acids and Bases I Chem 102 Dr. Curtis Acids and Bases Acids Sour taste vinegar Dissolve many metals Ability to neutralize bases Strong or Weak Bases Bitter taste caffeine, poisons from plants

More information

Acids & Bases. Mr. Matthew Totaro Legacy High School AP Chemistry Pearson Education, Inc.

Acids & Bases. Mr. Matthew Totaro Legacy High School AP Chemistry Pearson Education, Inc. Acids & Bases Mr. Matthew Totaro Legacy High School AP Chemistry 2012 Pearson Education, Inc. Properties of Acids Sour taste React with active metals i.e., Al, Zn, Fe, but not Cu, Ag, or Au corrosive 2

More information

Unit 7: Acids & Bases

Unit 7: Acids & Bases Definitions of Acids & Bases Unit 7: Acids & Bases Chapter 16 Arrhenius Acid: Substance that, when dissolved in water, increases the concentration of hydrogen ions. Base: Substance that, when dissolved

More information

Chapter 13. Acids and Bases. Introduction. Acids and Bases Affect Our Lives. Chapter 13 Topics What are Acids and Bases?

Chapter 13. Acids and Bases. Introduction. Acids and Bases Affect Our Lives. Chapter 13 Topics What are Acids and Bases? Introduction Chapter 13 Acids and Bases How do acids and bases differ from other substances? What determines the ph of a solution? 1 2 Copyright The McGraw-Hill Companies, Inc. Permission required for

More information

Talk in. Arrhenius Acid- Base Definition and ph

Talk in. Arrhenius Acid- Base Definition and ph Talk in. Arrhenius Acid Base Definition and ph When we think of acids, we typically think of the Arrhenius definition. Svante Arrhenius (18591927) Arrhenius Acid = Any compound that increases the hydronium

More information

Acids and Bases: Definitions. Brønsted-Lowry Acids and Bases. Brønsted-Lowry Acids and Bases CHEMISTRY THE CENTRAL SCIENCE

Acids and Bases: Definitions. Brønsted-Lowry Acids and Bases. Brønsted-Lowry Acids and Bases CHEMISTRY THE CENTRAL SCIENCE CHEMISTRY THE CENTRAL SCIENCE Professor Angelo R. Rossi Department of Chemistry Spring Semester Acids and Bases: Definitions Arrhenius Definition of Acids and Bases Acids are substances which increase

More information

Acids and Bases. PreAP Chemistry Chap. 14

Acids and Bases. PreAP Chemistry Chap. 14 Acids and Bases PreAP Chemistry Chap. 14 Introduction to Acids and Bases Acids and bases are both aqueous solutions. A substance (solid or liquid) may be identified as an acid or base BUT, does not have

More information

Chapter 16 Acid-Base Equilibria. Acids and Bases. What happens when an acid dissolves in water? Acid and base strength. Conjugate acids and bases

Chapter 16 Acid-Base Equilibria. Acids and Bases. What happens when an acid dissolves in water? Acid and base strength. Conjugate acids and bases 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

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

ACIDS AND BASES. In aqueous solution bases have the following properties: bitter taste soapy feeling turn red litmus paper blue neutralise acids

ACIDS AND BASES. In aqueous solution bases have the following properties: bitter taste soapy feeling turn red litmus paper blue neutralise acids acid H appears in the formula base contains OHˉ group acid + base salt + H 2 O HCl + NaOH NaCl + H 2 O ACIDS AND BASES In aqueous solution acids have the following properties: sour taste turn blue litmus

More information

Chapter 15 Acids- Bases. The Nature of Acids and Bases. Some Common Acid. Principles of Chemistry A Molecular Approach, 1 st Ed. Nivaldo J.

Chapter 15 Acids- Bases. The Nature of Acids and Bases. Some Common Acid. Principles of Chemistry A Molecular Approach, 1 st Ed. Nivaldo J. Chapter 15 -Acids and Bases Principles of Chemistry A Molecular Approach, 1 st Ed. Nivaldo J. Tro Dr. Azra Ghumman Memorial University of Newfoundland The Nature of Acids and Bases Properties of Acids:

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

10.1 & 10.2 ACIDS AND BASES

10.1 & 10.2 ACIDS AND BASES 10.1 & 10.2 ACIDS AND BASES PROPERTIES OF ACIDS AND BASES Acids Bases ph Electrical conductivity Taste Feel Colour with litmus paper Colour with phenolphthalein PROPERTIES OF ACIDS AND BASES Acids Bases

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

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

Chapter 15: Properties of Acids. Properties of Bases

Chapter 15: Properties of Acids. Properties of Bases : Properties of Acids An acid is any substance that releases hydrogen ions, H +, into water. Blue litmus paper turns red in the presence of hydrogen ions. Blue litmus is used to test for acids. Acids have

More information

Aqueous Equilibria: Chemistry of the Water World. Chapter Outline

Aqueous Equilibria: Chemistry of the Water World. Chapter Outline Aqueous Equilibria: Chemistry of the Water World Chapter Outline 15.1 Acids and Bases: The BrØnsted Lowry Model 15.2 Acid Strength and Molecular Structure 15.3 ph and the Autoionization of Water 15.4 Calculations

More information

[H + ] =10 ph poh = -Log [OH - ] [OH - ]=10 poh

[H + ] =10 ph poh = -Log [OH - ] [OH - ]=10 poh Self Ionization of Water H 2 O H + + OH - Acids & Bases ph poh [H + ] [OH - ] Pure Water [H + ] = [OH - ], remember: [ ] means concentration 1 x 10 7 = 1 x 10 7 [H + ] > [OH - ], there is an acidic solution

More information

Acids and Bases: A Brief Review, see also pp and pp Brønsted-Lowry Acids and Bases 143. The H + Ion in Water

Acids and Bases: A Brief Review, see also pp and pp Brønsted-Lowry Acids and Bases 143. The H + Ion in Water Quiz number 5 will be given in recitation next week, Feb 26Mar 2 on the first part of Chapter 16, to be covered in lectures this week. 16.1 Acids and Bases: A Brief Review 16.2 BronstedLowry Acids and

More information

Chapter 18. Acids and Bases

Chapter 18. Acids and Bases Chapter 18 Acids and Bases Warm Up Name any acids that you have at home. What are they usually used for? Name any bases that you have at home. What are they usually used for? Today s Agenda QOTD: What

More information

Reactions in Solution (Acids and Bases): Chapter 10. Chapter Outline. Chapter Outline

Reactions in Solution (Acids and Bases): Chapter 10. Chapter Outline. Chapter Outline Reactions in Solution (Acids and Bases): Chapter 0 Chapter Outline Properties of Aqueous Solutions of Acids and Bases The Arrhenius Theory The Hydronium Ion (Hydrated Hydrogen Ion) The BrØnstedLowry Theory

More information

Brønsted-Lowry Acid/Base. 1. What's the Brønsted definition of an acid?...of a base?

Brønsted-Lowry Acid/Base. 1. What's the Brønsted definition of an acid?...of a base? Brønsted-Lowry Acid/Base Name 1. What's the Brønsted definition of an acid?...of a base? 2. In 1923, Johannes Brønsted (Danish) and Thomas Lowry (British) independently expanded definition of Arrhenius

More information

Acids and Bases. Chapter 15. Acids. Bases. A Brønsted acid is a proton donor A Brønsted base is a proton acceptor

Acids and Bases. Chapter 15. Acids. Bases. A Brønsted acid is a proton donor A Brønsted base is a proton acceptor Acids and Bases Chapter 15 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 Acids Have a sour taste. Vinegar owes its taste to acetic acid. Citrus fruits contain

More information

CHAPTER 18 ACID-BASE EQUILIBRIA

CHAPTER 18 ACID-BASE EQUILIBRIA CHAPTER 18 ACID-BASE EQUILIBRIA Section 18.1: Acids and Bases in Water Water (H 2 O) the most important molecule on earth. Even in pure water, there are small amounts of ions from the equilibrium below

More information

Name Class Date. In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question.

Name Class Date. In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question. Assessment Chapter Test A Chapter: Acids and Bases In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question. 1. Which of the properties

More information

Chapter 15: Acids and Bases

Chapter 15: Acids and Bases Chapter 15: Acids and Bases Essentials of General Chemistry Ebbing Gammon Ragsdale 2nd Edition Dr. Azra Ghumman Memorial University of Newfoundland 1 Acids and Bases 15.1 Arrhenius Concept of Acids and

More information

ACIDS, BASES, AND SALTS

ACIDS, BASES, AND SALTS Name Date Class 19 ACIDS, BASES, AND SALTS SECTION 19.1 ACID BASE THEORIES (pages 587 593) This section compares and contrasts acids and bases as defined by the theories of Arrhenius, Brønsted-Lowry, and

More information

Table 1. give a slippery feel. produce a piercing pain in a wound. are colorless when placed in phenolphthalein (an indicator).

Table 1. give a slippery feel. produce a piercing pain in a wound. are colorless when placed in phenolphthalein (an indicator). Acid/Base Basics How does one define acids and bases? In chemistry, acids and bases have been defined differently by two sets of theories. One is the Arrhenius definition, which revolves around the idea

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

ACID-BASE NEUTRALIZATION

ACID-BASE NEUTRALIZATION ACID-BASE NEUTRALIZATION ACID-BASE NEUTRALIZATION REACTIONS A second type of chemical reaction that occurs in aqueous solution is an acid-base neutralization reaction So, what are acids and bases? ACIDS

More information

Acids and Bases Chapter 15

Acids and Bases Chapter 15 Acids Acids and Bases Chapter 15 Topics: p scale, Strengths of Acids and Bases, Ionization Constants of Weak Acids and Bases; Properties of Salts ave a sour taste. Vinegar owes its taste to acetic acid.

More information

Name Date Class STUDY GUIDE FOR CONTENT MASTERY. Acids and Bases: An Introduction In your textbook, read about the properties of acids and bases.

Name Date Class STUDY GUIDE FOR CONTENT MASTERY. Acids and Bases: An Introduction In your textbook, read about the properties of acids and bases. Acids and Bases Section 19.1 Acids and Bases: An Introduction In your textbook, read about the properties of acids and bases. For each description below, write acid if it tells about a property of an acid

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

Chemistry 51 Chapter 10 ACIDS & BASES. The most common definition of acids and bases was formulated by the Swedish chemist Svante Arrhenius in 1884.

Chemistry 51 Chapter 10 ACIDS & BASES. The most common definition of acids and bases was formulated by the Swedish chemist Svante Arrhenius in 1884. ACIDS & BASES Many common substances in our daily lives are acids and bases. Oranges, lemons and vinegar are examples of acids. In addition, our stomachs contain acids that help digest foods. Antacid tablets

More information

Chapter 10. Acids, Bases, and Salts

Chapter 10. Acids, Bases, and Salts 1 Chapter 10 Acids, Bases, and Salts 2 Ch 10.1 Arrhenius Acid-Base Theory (also in Chapter Medley) Arrhenius Acids produce Arrhenius Bases produce H + in water OH - in water HCl hydrochloric acid KOH HNO

More information

Equilibrium 1. Molecular Chapter Ionic (Weak Acid / Base ) - Chapter Ionic ( Insoluble Salts) - Chapter 17

Equilibrium 1. Molecular Chapter Ionic (Weak Acid / Base ) - Chapter Ionic ( Insoluble Salts) - Chapter 17 Equilibrium 1. Molecular ------------------- Chapter 15 2. Ionic (Weak Acid / Base ) - Chapter 16 3. Ionic ( Insoluble Salts) - Chapter 17 STRONG Acids & Bases 1. COMPLETELY IONIZED (a) HCl(aq) H + (aq)

More information

Solutions for Ch. 14 Acids and Bases Practice Questions

Solutions for Ch. 14 Acids and Bases Practice Questions s for Ch. 14 Acids and Bases Practice Questions 1. In the following reactions, label the Acid, Base, Conjugate Acid, and Conjugate Base. Also indicate the two conjugate acid-base pairs Plan Your Strategy

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

Chapter 16 questions. b) An Arrhenius acid turns red litmus blue. c) An Arrhenius acid tastes sour.

Chapter 16 questions. b) An Arrhenius acid turns red litmus blue. c) An Arrhenius acid tastes sour. Chapter 16 questions 1. Which of the following statements does not accurately describe a characteristic property of an Arrhenius acid? a) An Arrhenius acid is a substance that increases the concentration

More information

EXPERIMENT 11 Acids, Bases, and ph

EXPERIMENT 11 Acids, Bases, and ph EXPERIMENT 11 Acids, Bases, and ph INTRODUCTION The concept of acidity and alkalinity dates from ancient times. The word acid is derived from the Latin word acidus, meaning sour. A common acid, acetic

More information

Acids. Names of Some Common Acids. Names of Acids. Learning Check. Solution 8.1. Acids and Bases

Acids. Names of Some Common Acids. Names of Acids. Learning Check. Solution 8.1. Acids and Bases Chapter 8 Acids and Bases Acids 8.1 Acids and Bases Arrhenius acids produce H + ions in water. H 2 O HCl(g) H + (aq) + Cl - (aq) are electrolytes. have a sour taste. turn litmus red. neutralize bases.

More information

Chapter 16. Acid-Base Equilibria Acids and Bases: A Brief Review Brønsted-Lowry Acids and Bases. Conjugate Acid-Base Pairs

Chapter 16. Acid-Base Equilibria Acids and Bases: A Brief Review Brønsted-Lowry Acids and Bases. Conjugate Acid-Base Pairs 16.1 Acids and Bases: A Brief Review Arrhenius concept of acids and bases: an acid increases [H + ] and a base increases [OH ]. 16.2 Brønsted-Lowry Acids and Bases In the Brønsted-Lowry system, a Brønsted-Lowry

More information

Chapter 10 Test - AP Chemistry 2011/2012

Chapter 10 Test - AP Chemistry 2011/2012 DO NOT WRITE ON QUIZ/EXAM - USE SCANTRON AND #2 PENCIL TEST # A Chapter 10 Test - AP Chemistry 2011/2012 Multiple Choice Identify the choice that best completes the statement or answers the question. 1.

More information

ALE 11. Acids, Bases, poh and ph

ALE 11. Acids, Bases, poh and ph Name Chem 163 Section: Team Number: ALE 11. Acids, Bases, poh and ph (Reference: 18.1 18.3 Silberberg 5 th edition) Why is baking soda basic? The Model: Brønsted-Lowry Acids and Bases Nitric acid satisfies

More information

Arrhenius Model Acid. Base. Brønsted-Lowry Model Acid. Base. + H O: + H Cl: H O H + [ :Cl: ] -

Arrhenius Model Acid. Base. Brønsted-Lowry Model Acid. Base. + H O: + H Cl: H O H + [ :Cl: ] - Chapter 14 1. Students will be able to define an acid and base in terms of both the Arrhenius and the Bronsted-Lowry definitions and provide examples of each (including examples that follow the Bronsted-Lowry

More information

Unit 2 ACIDS AND BASES

Unit 2 ACIDS AND BASES Unit 2 ACIDS AND BASES Operational Definition One that is used to classify a substance Acids are aqueous solutions that: 1. turn blue litmus red (ph less than 7 at 25 C) 2. neutralize basic solutions 3.

More information

Things To Do Now: What s an Acid? What s a Base? 5/18/2015

Things To Do Now: What s an Acid? What s a Base? 5/18/2015 Things To Do Now: 1 Unit 13: Acids & Bases Lesson 13.1: Properties of Arrhenius Acids & Bases 2 What s an Acid? What s a Base? They ve been known for a long time. They were unexplained for a long time.

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

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

ACIDS AND BASES. Chapter 4 Section 4.4 Acid Base Reactions ( ) Chapter 18 Section 18.1, 18.2, 18.3 Naming Acids 70

ACIDS AND BASES. Chapter 4 Section 4.4 Acid Base Reactions ( ) Chapter 18 Section 18.1, 18.2, 18.3 Naming Acids 70 ACIDS AND BASES Chapter 4 Section 4.4 Acid Base Reactions (150 157) Chapter 18 Section 18.1, 18.2, 18.3 Naming Acids 70 Problems: Chapter 18: 5, 7, 21, 23, 24, 43, 44 Chapter 4: 49, 53, 54 Concepts: Definitions

More information

Chapter 16 Acid and Bases. There is an equilibrium between these two ions in water or in any aqueous solution:

Chapter 16 Acid and Bases. There is an equilibrium between these two ions in water or in any aqueous solution: 1 I. Acidic and Basic water solutions: Chapter 16 Acid and Bases A. Dissociation of water The H + ion (or the H 3 O + ion) is characteristic of acidic water solutions. The OH - ion gives basic solutions

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

React with carbonates, such, calcium carbonate and bicarbonates, such as, sodium bicarbonate, to produce carbon dioxide gas

React with carbonates, such, calcium carbonate and bicarbonates, such as, sodium bicarbonate, to produce carbon dioxide gas Acids and Bases Acids and bases are very important class of chemicals that we come across in our everyday lives that are essential in sustaining biological systems, but we never realize their importance

More information

Models of Acids and Bases. The reaction of an acid HA with water to form H 3 O+ and a conjugate base A-. Conjugate Acid/Base Pairs

Models of Acids and Bases. The reaction of an acid HA with water to form H 3 O+ and a conjugate base A-. Conjugate Acid/Base Pairs Models of Acids and Bases ACIDS and BASES Arrhenius Concept: Acids produce H in solution, bases produce OH ion. Brønsted-Lowry: Acids are H donors, bases are proton acceptors. Review Chapter 4 Acids &

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

Monday, April 16 th : A Day Tuesday, April 17 th : B Day Agenda

Monday, April 16 th : A Day Tuesday, April 17 th : B Day Agenda Monday, April 16 th : A Day Tuesday, April 17 th : B Day Agenda ACT Practice Passages 5 & 6 Hand back/go over Ch. 14 Tests Begin chapter 15: Acids & Bases 15.1: What Are Acids & Bases? Strong/weak acid,

More information

Chapter 15: Acids, Bases, and Salts. 15.1: Acids and Bases

Chapter 15: Acids, Bases, and Salts. 15.1: Acids and Bases Chapter 15: Acids, Bases, and Salts Name: 15.1: Acids and Bases Define an Acid: Define a Base: Ex of an acid in aqueous solution: Ex of a base in aqueous solution: List some of the properties of acids

More information

15.1 Acids - Bases in Water

15.1 Acids - Bases in Water 15.1 more equilibrium Dr. Fred Omega Garces Chemistry 201 Miramar College 1 Acids-Bases Characteristics Acids (Properties) Taste Sour Dehydrate Substances Neutralizes bases Dissolves metals Examples: Juices:

More information

CHEMISTRY NOTES CHAPTERS 20 AND 21. Acids and Bases - Neutralization

CHEMISTRY NOTES CHAPTERS 20 AND 21. Acids and Bases - Neutralization NOTES: Goals : To gain an understanding of : Properties of acids : Properties of bases : 1. The properties of acids and bases 2. ph and poh calculations 3. Definitions of acids and bases 4. Neutralization

More information

SECTION 19.1 ACID-BASE THEORIES (Pages )

SECTION 19.1 ACID-BASE THEORIES (Pages ) SECTION 19.1 ACID-BASE THEORIES (Pages 587-593) This section compares and contrasts acids and bases as defined by the theories of Arrhenius, Brønsted-Lowry, and Lewis. It also identifies conjugate acid

More information

Acid-Base Equilibrium. Introduction to Aqueous Acids. Models of Acids and Bases. Introduction to Aqueous Bases. Lewis Acids and Bases

Acid-Base Equilibrium. Introduction to Aqueous Acids. Models of Acids and Bases. Introduction to Aqueous Bases. Lewis Acids and Bases Acid-Base Equilibrium Dr. Ron Rusay Fall 2007 Introduction to Aqueous Acids Acids: taste sour and cause certain dyes to change color. Copyright 2003-2007 R.J. Rusay Introduction to Aqueous Bases Bases:

More information

Acids and Bases. How do acids and bases behave in water? Acid or Base Acetic acid HC 2. (aq) Vinegar Sour Red Yes Acid Benzoic acid HC 7

Acids and Bases. How do acids and bases behave in water? Acid or Base Acetic acid HC 2. (aq) Vinegar Sour Red Yes Acid Benzoic acid HC 7 Why? Acids and Bases How do acids and bases behave in water? Acids and bases play an important role in our lives. Numerous biological processes, industrial applications, and even environmental problems

More information

CHAPTER 10 Reactions in Aqueous Solutions I: Acids, Bases & Salts

CHAPTER 10 Reactions in Aqueous Solutions I: Acids, Bases & Salts CHAPTER 10 Reactions in Aqueous Solutions I: Acids, Bases & Salts 1. Properties of Aqueous Solutions of Acids & Bases 2. The Arrhenius Theory 3. The BrØnsted-Lowry Theory 4. The Lewis Theory 5. The Autoionization

More information

Bronsted Acids & Bases

Bronsted Acids & Bases Acids and Bases 1 Bronsted Acids & Bases Acid: substance capable of donating a proton (H + ). Base: substance capable of accepting a proton. (definition not dependent on OH - ) 2 Conjugate Pairs CH 3 COOH

More information

3. Bases are compounds that react with acids to form and a(n).

3. Bases are compounds that react with acids to form and a(n). Name ACIDS, BASES, AND SALTS 19 Period Date SECTION 19.1 ACID BASE THEORIES This section compares and contrasts acids and bases as defined by the theories of Arrhenius, Brønsted-Lowry, and Lewis. It also

More information

Name Date Class. Use the terms below to complete the passage. You may use each term more than once.

Name Date Class. Use the terms below to complete the passage. You may use each term more than once. Acids and Bases Acids and Bases: An Introduction In your textbook, read about the properties of acids and bases. For each description below, write acid if it tells about a property of an acid or base if

More information

Chapter 16 Acids and Bases

Chapter 16 Acids and Bases Chapter 16 Acids and Bases Properties of Acids and Bases 1. Circle the letters of all the terms that complete the sentence correctly. 2. The properties of acids include _. a. reacting with metals to produce

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

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

Ch Acids and Bases. Arrhenius Definition Acids produce hydrogen ions in aqueous solution. Bases produce hydroxide ions when dissolved in water.

Ch Acids and Bases. Arrhenius Definition Acids produce hydrogen ions in aqueous solution. Bases produce hydroxide ions when dissolved in water. Ch 15-16 Acids and Bases Arrhenius Definition Acids produce hydrogen ions in aqueous solution. Bases produce hydroxide ions when dissolved in water. Limits to aqueous solutions. Only one kind of base.

More information

Name: Class: Date: Multiple Choice Identify the letter of the choice that best completes the statement or answers the question.

Name: Class: Date: Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. Class: Date: Chapter 13 Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1. In the Brønsted-Lowry model an acid is a. a proton donor. b. a proton

More information

What are acids? 9: Charge transfer rxns: acids and bases and oxidation-reduction. Arrhenius definitions. What are bases? Arrhenius definitions

What are acids? 9: Charge transfer rxns: acids and bases and oxidation-reduction. Arrhenius definitions. What are bases? Arrhenius definitions What are acids? 9: Charge transfer rxns: acids and bases and oxidation-reduction Acids: sharp,sour taste, feel prickly on skin, react with metals to release H 2 (g), react with carbonates to release CO

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

ACIDS AND BASES. Chapter 14, 15

ACIDS AND BASES. Chapter 14, 15 ACIDS AND BASES Chapter 14, 15 PROPERTIES Properties of Acids Properties of Bases 1. Sour taste (vinegar, lemon) 1. Bitter taste (soaps, detergents) 2. ph paper turns red 2. ph paper turns blue 3. Acids

More information

CHEM&163 (S2016) Chapter 15 Acids and Bases Lecture Outline (M. Dunn)

CHEM&163 (S2016) Chapter 15 Acids and Bases Lecture Outline (M. Dunn) 1. Acid Base theory by Three Definitions Lecture Slide 2. Acid/Base Theory: Arrhenius Acids and Bases Acid: Released H + in water (H3O + ) Base: Releases OH - in water My notes/reminders etc. Bronsted-Lowry

More information

ACIDS AND BASES. Nonelectrolytes - substances which do not conduct electricity in water solutions.

ACIDS AND BASES. Nonelectrolytes - substances which do not conduct electricity in water solutions. ACIDS AND BASES Electrolytes substances which will conduct electricity when dissolved in water. Typical electrolytes are strong acids and salt solutions; e.g., NaCl(aq), HCl(aq), etc. Nonelectrolytes substances

More information

CHAPTER 9. ANS: a. ANS: d. ANS: c. ANS: a. ANS: c

CHAPTER 9. ANS: a. ANS: d. ANS: c. ANS: a. ANS: c CHAPTER 9 1. Which one of the following is the acid in vinegar? a. acetic acid b. citric acid c. muriatic acid d. ascorbic acid 2. Which is a basic or alkaline substance? a. gastric fluid b. black coffee

More information

If we write these equations in ionic form, in each case the net ionic equation is the same; H 3 O + (aq) + OH - (aq) H 2H 2 O(l)

If we write these equations in ionic form, in each case the net ionic equation is the same; H 3 O + (aq) + OH - (aq) H 2H 2 O(l) CHEM 1105 ACIDS AND BASES 1. Early Definitions Taste: Effect on Indicators: Neutralization: acids - sour; bases - bitter acids turn blue litmus red; bases turn red litmus blue phenolphthalein is colourless

More information

Acids, Bases, and Salts

Acids, Bases, and Salts Acids, Bases, and Salts Properties of Acids They taste sour (don t try this at home). They can conduct electricity. Can be strong or weak electrolytes in aqueous solution React with metals to form H 2

More information

Unit 9: Acids, Bases, & Salts

Unit 9: Acids, Bases, & Salts Unit 9: Acids, Bases, & Salts Unit Vocabulary: Amphoteric Arrhenius acid Arrhenius base Bronsted-Lowry acid Bronsted-Lowry base Electrolyte hydronium ion hydroxide ion indicator (acid/base) neutralization

More information

Chemistry Slide 1 of 35

Chemistry Slide 1 of 35 Chemistry 19.1 1 of 35 Acid-Base Theories Bracken Cave, near San Antonio, Texas, is home to twenty to forty million bats. Visitors to the cave must protect themselves from the dangerous levels of ammonia

More information

TYPES OF CHEMICAL REACTION

TYPES OF CHEMICAL REACTION TYPES OF CHEMICAL REACTION I. METATHESIS REACTIONS (or DOUBLE DISPLACEMENT RXNS) In these reactions the ions of the reactants are exchanged: A + B (aq) + C + D (aq) AD (?) + CB (?) Double Displacement

More information

Chapter 7: Phenomena. Chapter 7 Acids and Bases. Acids and Bases. Acids and Bases. Acids and Bases

Chapter 7: Phenomena. Chapter 7 Acids and Bases. Acids and Bases. Acids and Bases. Acids and Bases Chapter 7: Phenomena Phenomena: Scientists dissolved different substances in water and then measured the [H + ] and [OH - ] concentrations in each solution. What patterns do you notice about the substances?

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

Introduction. Acids and Bases

Introduction. Acids and Bases 1 Acids, Bases, Buffers and ph Introduction Purpose: To examine properties of acids and bases, buffers, and salt solutions, and use different methods to measure the ph of those solutions. Acids and Bases

More information

Conjugate Acid Base Pairs. Brønsted-Lowry Acids and Bases. Brønsted Lowry Acids & Bases HA + B: A - + BH + Chapter 2

Conjugate Acid Base Pairs. Brønsted-Lowry Acids and Bases. Brønsted Lowry Acids & Bases HA + B: A - + BH + Chapter 2 Brønsted Lowry Acids & Bases Acid-Base Chemistry & Organic Compounds Brønsted-Lowry Acid: Proton (H + ) Donor Brønsted-Lowry Base: Proton (H + ) Acceptor General reaction: HA + B: A - + BH + Chapter 2

More information

Chapter 15 Review. 2. Which is the formula for the hydronium ion? A. OH - B. H 2 O C. H 3 O + D. H 3 O - E. H 2 O +

Chapter 15 Review. 2. Which is the formula for the hydronium ion? A. OH - B. H 2 O C. H 3 O + D. H 3 O - E. H 2 O + Chapter 15 Review Student: 1. Which is not a characteristic property of acids? A. tastes sour B. turns litmus from blue to red C. reacts with metals to yield CO 2 gas D. neutralizes bases E. reacts with

More information

Notes: Acids and Bases

Notes: Acids and Bases Name Chemistry Pre-AP Notes: Acids and Bases Period I. Describing Acids and Bases A. Properties of Acids taste ph 7 Acids change color of an (e.g. blue litmus paper turns in the presence of an acid) React

More information

Arrhenius concept. Bronsted Lowry concept

Arrhenius concept. Bronsted Lowry concept Acids, Bases,, ph and Buffer There are three concepts of acids and bases in current use. Each has its own peculiar advantages. The student should understand all the three concepts: (a) Arrhenius concept,

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

Sodium hydroxide, a base, produces hydroxide ions in solution:

Sodium hydroxide, a base, produces hydroxide ions in solution: Assistant Lecture Aayad Amaar Acids and Bases The properties of acids and bases are related to their chemical structure. All acids have common characteristics that enable them to increase the hydrogen

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

Answers and Solutions to Text Problems

Answers and Solutions to Text Problems Acids and Bases 10 Answers and Solutions to Text Problems 10.1 According to the Arrhenius theory: a. acids taste sour. b. acids neutralize bases. c. acids produce H 3 O + ions in water. d. potassium hydroxide

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

ionic substances (separate) based on! Liquid Mixtures miscible two liquids that and form a immiscible two liquids that form a e.g.

ionic substances (separate) based on! Liquid Mixtures miscible two liquids that and form a immiscible two liquids that form a e.g. Unit 7 Solutions, Acids & Bases Solution mixture + solvent - substance present in the amount solute - in the solvent solvent molecules solute particles ionic substances (separate) based on! Liquid Mixtures

More information

H 2 O + HNO 3 H 3 O + + NO 3

H 2 O + HNO 3 H 3 O + + NO 3 Properties Unit 12 Acids & Bases electrolytes sour taste turn litmus red react with metals to form 2 gas vinegar, soda, citrus fruits electrolytes bitter taste turn litmus blue slippery feel ammonia, lye,

More information

Acids, Bases, and ph

Acids, Bases, and ph Acids, Bases, and ph by Dr. Lara Baxley Cuesta College, San Luis Obispo, CA Outline I. Acids II. Acids in Water III. Strong vs. Weak Acids IV. Bases V. The ph Concept VI. ph of Strong Acid and Strong Base

More information