ACID-BASE TITRATIONS: DETERMINATION OF CARBONATE BY TITRATION WITH HYDROCHLORIC ACID BACKGROUND
|
|
- Alexandra Elliott
- 7 years ago
- Views:
Transcription
1 #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 acid is prepared, standardized against pure sodium carbonate, and used to determine the percentage of carbonate in a sample. An aqueous solution of hydrochloric acid is almost completely dissociated into hydrated protons and chloride ions. Therefore, in a titration with hydrochloric acid the active titrant species is the hydrated proton. This species is often written H 3 O +, although the actual form in solution is more correctly (H 2 O) n H +. For convenience we designate it simply H +. Carbonate in aqueous solution acts as a base; that is, it is able to accept a proton to form bicarbonate ion. CO H + <==========> HCO - 3 (1) Bicarbonate is able to combine with another proton to form carbonic acid: HCO H + <==========> H 2 CO 3 (2) Equilibrium expressions for the dissociation of bicarbonate and carbonic acid may be written K 2 = [H+ ] [CO 2-3 ] [HCO - 3 ] (3) and K 1 = [H+ ] [HCO - 3 ] [H 2 CO 3 ] (4) where K 1 and K 2 are the first and second acid dissociation constants for H 2 CO 3 ; the experimentally determined values are K 1 = 3.5 x 10-7 and K 2 = 5 x When successive protonation reactions such as (1) and (2) occur, the extent to which the first reaction proceeds before the second begins depends on the
2 28 #3. Acid- Base Titrations difference between the two acid dissociation constants. By combination of Equations (3) and (4) with those for charge and mass balance, [H + ] can be calculated for any ratio of hydrochloric acid to initial carbonate concentration, that is, at any point on a titration curve of carbonate with hydrochloric acid. Because complete and rigorous solution is time consuming, here only procedures for calculating the ph at several convenient points in a titration of 0.1 M sodium carbonate with 0.1 M hydrochloric acid (Figure 1) are covered briefly. An analytical textbook should be consulted for a more detailed discussion of this topic. ph at Point A in Figure 1. At point A no acid has been added, and only sodium carbonate is present in solution. The ph is determined by the extent of carbonate reaction with water to give HCO - 3 and OH- 1 : CO H 2 O <==========> HCO OH- (5) Here water acts as an acid, providing a proton to carbonate ion, the base. The equilibrium constant for this reaction may be written Figure 1. Curve for the titration of carbonate with hydrochloric acid. K b = [HCO- 3 ] [OH- ] [CO 2-3 ] (6) Multiplying the right side of Equation (6) by [H + ]/[H + ], we see that K b is equal to K w /K 2, where K w is the dissociation constant for water. K w = [H + ] [OH - ] = at 25 C (7) 1 Reactions of ions of a solute with water often are called hydrolysis reactions. They are more properly considered, however, as simply another example of a Bronsted acid-base reaction in which water acts as an acid or a base.
3 #3. Acid - Base Titrations 29 and K 2 is the second dissociation constant for carbonic acid [Equation 3]. If the initial concentration of carbonate and the values of K w and K 2 are known, [OH - ] can be calculated from K w K 2 = [HCO - 3 ] [OH- ] [CO 2- (8) 3 ] Assume that the equilibrium for Equation (5) lies far to the left, so that the carbonate ion concentration is still essentially 0.1 M. Since bicarbonate and hydroxide are formed in equimolar amounts, [HCO - 3 ] = [OH - ] (9) Substitution of numerical values and Equation (9) in Equation (8) gives x = [OH- ] (10) and [OH - ] = 4.5 x 10-3 M (11) From Equation (7) [H + ] = x 10-3 = 2.2 x M (12) so the ph is In our use of Equation (6) we assume that the reaction HCO H 2O <=========> H 2 CO 3 + OH- (13) does not occur to an appreciable extent; that it does not can be verified by substituting the value for [H + ] found in Equation (12) in Equation (4) and
4 30 #3. Acid- Base Titrations calculating [H 2 CO 3 ]. If [H 2 CO 3 ] is found to be greater than 5% of the total carbonate concentration, the [H + ] calculated from Equations (6) and (7) will be appreciably in error. In this case the expression should be solved either exactly, by including all species (which is tedious), or by successive approximations. Calculation shows that [H 2 CO 3 ] at Point A is negligibly small, so our assumption is valid. The additional assumption that [CO 2-3 ] is essentially 0.1 M also is confirmed because Equations (9) and (11) show that [HCO - 3 ] is less than 5% of [CO 2-3 ]. Note from this discussion that K w K = K b, or K w = K 2 K b. Thus, if Ka for an acid 2 HA is known, K b for the corresponding base A - can be calculated in aqueous solutions. An acid HA and base A - are called a conjugate acid-base pair; HA is the conjugate acid of A - and A - the conjugate base of HA. ph at Point B. At Point B in Figure 1, 1 2 mole of hydrochloric acid has been added for each mole of carbonate. The solution now contains an equimolar mixture of carbonate and bicarbonate. We can calculate the ph at this point by rearranging Equation (3) to [H + ] = [HCO- 3 ] K 2 [CO 2-3 ] (14) Since the bicarbonate and carbonate concentrations are equal, the hydrogen ion concentration is equal to K 2, and the ph is Accurate calculations of concentrations of species during titrations must include the effect of dilution by the titrant, but thus far those caused by the addition of hydrochloric acid have not been considered. To correct calculations of concentrations of the major components for dilution, multiply each calculated concentration by the factor V/(V + ν), where V is the volume of the original solution and ν is the volume of hydrochloric acid added at any point. Although in the present example the effect is slight, in many systems the correction is significant.
5 #3. Acid - Base Titrations 31 ph at Point C. The first equivalence point (C in Figure 1) is reached when 1 mole of hydrochloric acid per mole of carbonate has been added. This solution contains only sodium bicarbonate; [H + ] is calculated by [H+] = K 1 K 2 = (3.5 x 10-7 ) (5 x ) = 4.2 x 10-9 M (15) and the ph is 8.4. ph at Point D. Protonation of half the bicarbonate gives an equimolar solution of bicarbonate and carbonic acid (Point D). This is again a buffer system, this time involving the first dissociation constant of carbonic acid. The calculation is handled in the same way as for Point B, with K 1 used in place of K 2, to yield a ph of 6.5. ph at Point E. At the second equivalence point (E) the ph is determined by the extent of dissociation of carbonic acid, the principal species present, and [H + ] is calculated from Equation (4): K 1 = 3.5 x 10-7 = [H + ] [HCO - 3 ] (0.1) [50/( )] = [H+ ] (16) Therefore, [H + ] = 1.07 x 10-4 M = (17) the ph is 3.97, or rounding to 2 significant figures, 4.0. Detection of the Equivalence Point Either the first or second equivalence point (C or E in Figure 1) can be used for carbonate analysis. In neither case is the ph change large in the region of the equivalence point. An uncertainty of 0.1 ph unit at either end point results in an uncertainty of about 1% in the amount of hydrochloric acid required. The error can be reduced if the titration is carried to a preselected indicator color. When a solution is titrated to the second equivalence point, a better approach is to take advantage of the dissociation of carbonic acid into a solution of carbon dioxide in water. Shaking or boiling a solution of carbonic acid causes the equilibrium to be H 2 CO 3 <=========> H 2 O + CO 2 (g) (18)
6 32 #3. Acid- Base Titrations driven to the right through loss of carbon dioxide. If a carbonate or bicarbonate solution is titrated to just before the equivalence point at ph 4 and then shaken or boiled, 2 the ph will rise to about 8 as the concentration of carbonic acid drops (dotted line in Figure 2). The ph is no longer controlled by dissociation of a relatively large concentration of carbonic acid but by a small concentration of bicarbonate. When the titrations continued, the ph goes down sharply because the amount of carbonic acid formed is small and the buffering effect negligible (dashed line in Figure 2). Standard Solutions Some standard solutions can be prepared directly by weighing or measuring carefully a definite quantity of a pure substance, dissolving it in a suitable solvent, and diluting it to a known volume. None of the strong acids, however, is convenient to handle and measure accurately in concentrated form. Therefore a solution of approximately the desired molarity is prepared, and the exact value is determined by standardization against a primary-standard base. Figure 2. Effect of removal of carbon dioxide on ph change the second equivalence point in a titration of carbonate with hydrochloric acid. Band indicates region of change of indicator color. Primary standards are stable, nonhygroscopic substances that react quantitatively and are easy to purify and handle. A high equivalent weight is advantageous because weighing errors are minimized. Among the excellent primary standards available are potassium acid phthalate, benzoic acid, oxalic 2 In mammals the CO 2 produced through biological oxidation is carried by the blood to the lungs, where it is exchanged for oxygen. Part of the CO 2 is present in the blood as H 2 CO 3. Since the time available in the lungs for exchange is short, the dissociation of H 2 CO 3 to CO 2 and H 2 O is accelerated by the enzyme carbonic acid anhydrase, a zinc-containing protein of high molecular weight. Thus nature need not resort to either boiling or shaking.
7 #3. Acid - Base Titrations 33 acid dihydrate, and sulfamic acid for standardizing bases and sodium oxalate, tris(hydroxymethyl)aminomethane, 4-amino pyridine, and sodium carbonate for standardizing acids. Pure anhydrous sodium carbonate, besides having all the properties of a suitable primary-standard base, has the added advantage in this experiment of being the same compound as the substance determined. This tends to compensate for determinate errors in end-point selection. PROCEDURE Reagent List: Unknown Sample - must be mixed thoroughly and dried HCl concentrated - approx. 12M sodium carbonate (Na 2 CO 3 ) - must be dried Bromocresol Green - indicator Put a little less than 1 liter of distilled water into a clean 1-liter bottle. Calculate the volume of 12 M HCl required to prepare 1 liter of 0.2 M HCl, and measure this quantity into a small graduated cylinder. Transfer it to the bottle and mix thoroughly. Label. Standardization of HCl with Primary-Standard Na 2 CO 3 Dry 1.5 to 2.0 g of pure Na 2 CO 3 in a glass weighing bottle or vial at 150 to 160 C for at least 2 hr. 3, 4 Allow to cool, in a desiccator if necessary, and then weigh by difference (to the nearest 0.1 mg) three or four 0.35 to 0.45 g portions of the dry material into clean 200-ml conical (Erlenmeyer) flasks. Add about 50 ml of distilled water to each and swirl gently to dissolve the salt. Add 4 drops of bromocresol green indicator and titrate with the HCl solution to an intermediate green color. At this point stop the titration and boil the solution gently for a minute or two, taking care that no solution is lost during the process. Cool the solution to room temperature, wash the flask walls with distilled water from a wash bottle, and then continue the titration to the first appearance of yellow. Just 3 Na 2 CO 3 tends to absorb H 2 O from the air to form Na 2 CO 3.H 2 O, and CO 2 to form NaHCO 3. At least several hours of drying at 140 C is necessary to remove all H 2 O and CO 2. 4 Use a pencil or felt marking pen to label the container with the name or sample number of the contents and with your locker number. The container may be placed inside a small glass beaker, and a watch glass, raised with several bent portions of glass rod, placed on top for protection. Avoid leaving chemicals or equipment in the drying oven longer than necessary, this not only causes crowding, but increases the chance of equipment being broken or samples contaminated by spilled chemicals.
8 34 #3. Acid- Base Titrations before the end point the titrant is best added in fractions of a drop. 5 Record the buret reading and add to it the buret calibration correction. Calculate the molarity of the HCl solution. The procedure outlined in the discussion of calculations below may be used as a guide. Relative deviations of 1 individual values from the average should not exceed about 2 parts per Determination of Carbonate in a Sample Mix the sample VERY THOROUGHLY and then dry it in a weighing bottle or small beaker for at least 2 hours at 150 to 160 C. Weigh into clean 200-ml conical flasks, to the nearest 0.1 mg, 0.35 to 0.45 g samples and titrate as in the standardization procedure. Calculate and report the percentage of Na 2 CO 3 in the sample. Use the Q test as the criterion for rejection of suspect experimental data. Either the median or the average may be reported. When the median is chosen the median value for the molarity of the HCl should be used in the calculations rather than the average value. CALCULATIONS The percentage of Na 2 CO 3 in a sample can be calculated in two steps: (1) the determination of the molarity of the HCl titrant from the standardization titrations and (2) the calculation of the percentage of Na 2 CO 3 from titrations of the sample. 1. Molarity of HCl. In titrations of Na 2 CO 3 with HCl to the ph 4 end point, 2 moles of HCl are added for each mole of Na 2 CO 3 : 2HCl + NaCO 3 <=========> H 2 CO 3 + 2NaCl (19) The HCl molarity is obtained from the following relations: MHCl = moles HCl liter = moles Na 2 CO 3 x 2 (ml HCl/1000) 5 To deliver amounts less than 1 drop from a buret, first let a droplet form on the tip, and then touch the tip momentarily to the inside wall of the flask. Rinse the wall with a small amount of distilled water from a wash bottle to ensure that the titrant is washed into the solution. Do not rinse the tip of the buret.
9 #3. Acid - Base Titrations 35 = (wt of Na 2 CO 3 ) x 2 (mol wt Na 2 CO 3 ) (ml HCl/1000) (20) The factor 2 required because each mole of Na 2 CO 3 reacts quantitatively with 2 moles of HCl. 2. Percentage of Na 2 CO 3 in Sample. The percentage of Na 2 CO 3 in the sample is calculated as follows: %Na 2 CO 3 = wt of Na 2 CO 3 in sample g sample x 100 = (moles Na 2CO 3 )(mol. wt. Na 2 CO 3 ) wt of sample x 100 (21) = (ml HCl) (molarity HCl) (mol wt Na 2CO 3 ) 1000 x 2 x wt. of sample x 100 Remember: Poor results are often caused by errors in calculation rather than by faulty laboratory technique. Check all calculations before reporting results.
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 informationExperiment 7: Titration of an Antacid
1 Experiment 7: Titration of an Antacid Objective: In this experiment, you will standardize a solution of base using the analytical technique known as titration. Using this standardized solution, you will
More informationVolumetric 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 informationTo determine the equivalence points of two titrations from plots of ph versus ml of titrant added.
Titration Curves PURPOSE To determine the equivalence points of two titrations from plots of ph versus ml of titrant added. GOALS 1 To gain experience performing acid-base titrations with a ph meter. 2
More informationSTANDARDIZATION OF A SODIUM HYDROXIDE SOLUTION EXPERIMENT 14
STANDARDIZATION OF A SODIUM HYDROXIDE SOLUTION EXPERIMENT 14 OBJECTIVE The objective of this experiment will be the standardization of sodium hydroxide using potassium hydrogen phthalate by the titration
More informationDetermination of the Amount of Acid Neutralized by an Antacid Tablet Using Back Titration
Determination of the Amount of Acid Neutralized by an Antacid Tablet Using Back Titration GOAL AND OVERVIEW Antacids are bases that react stoichiometrically with acid. The number of moles of acid that
More informationAcid Base Titrations
Acid Base Titrations Introduction A common question chemists have to answer is how much of something is present in a sample or a product. If the product contains an acid or base, this question is usually
More informationTo 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 informationAcid 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 informationMASSACHUSETTS INSTITUTE OF TECHNOLOGY Department of Chemistry 5.310 Laboratory Chemistry THE POTENTIOMETRIC TITRATION OF AN ACID MIXTURE 1
MASSACHUSETTS INSTITUTE OF TECHNOLOGY Department of Chemistry 5.310 Laboratory Chemistry EXPERIMENT #5 THE POTENTIOMETRIC TITRATION OF AN ACID MIXTURE 1 I. PURPOSE OF THE EXPERIMENT In this experiment
More informationProperties of Acids and Bases
Lab 22 Properties of Acids and Bases TN Standard 4.2: The student will investigate the characteristics of acids and bases. Have you ever brushed your teeth and then drank a glass of orange juice? What
More informationAn 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 informationDissolving of sodium hydroxide generates heat. Take care in handling the dilution container.
TITRATION: STANDARDIZATION OF A BASE AND ANALYSIS OF STOMACH ANTACID TABLETS 2009, 1996, 1973 by David A. Katz. All rights reserved. Reproduction permitted for education use provided original copyright
More informationLab #10 How much Acetic Acid (%) is in Vinegar?
Lab #10 How much Acetic Acid (%) is in Vinegar? SAMPLE CALCULATIONS NEED TO BE DONE BEFORE LAB MEETS!!!! Purpose: You will determine the amount of acetic acid in white vinegar (sold in grocery stores)
More informationDetermining the Identity of an Unknown Weak Acid
Purpose The purpose of this experiment is to observe and measure a weak acid neutralization and determine the identity of an unknown acid by titration. Introduction The purpose of this exercise is to identify
More informationEXPERIMENT 12 A SOLUBILITY PRODUCT CONSTANT
PURPOSE: 1. To determine experimentally the molar solubility of potassium acid tartrate in water and in a solution of potassium nitrate. 2. To examine the effect of a common ion on the solubility of slightly
More informationStoichiometry Limiting Reagent Laboratory. Chemistry 118 Laboratory University of Massachusetts, Boston
Chemistry 118 Laboratory University of Massachusetts, Boston STOICHIOMETRY - LIMITING REAGENT --------------------------------------------------------------------------------------------------------------------------------------------
More informationCarolina s Solution Preparation Manual
84-1201 Carolina s Solution Preparation Manual Instructions Carolina Biological Supply Company has created this reference manual to enable you to prepare solutions. Although many types of solutions may
More information9. Analysis of an Acid-Base Titration Curve: The Gran Plot
9. Analysis of an Acid-Base Titration Curve: The Gran Plot In this experiment, you will titrate a sample of pure potassium hydrogen phthalate (Table 10-4) with standard NaOH. A Gran plot will be used to
More informationPrecipitation Titration: Determination of Chloride by the Mohr Method by Dr. Deniz Korkmaz
Precipitation Titration: Determination of Chloride by the Mohr Method by Dr. Deniz Korkmaz Introduction Titration is a process by which the concentration of an unknown substance in solution is determined
More informationQ.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 informationExperiment 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 informationEvaluation copy. Titration of a Diprotic Acid: Identifying an Unknown. Computer
Titration of a Diprotic Acid: Identifying an Unknown Computer 25 A diprotic acid is an acid that yields two H + ions per acid molecule. Examples of diprotic acids are sulfuric acid, H 2 SO 4, and carbonic
More informationDetermination of calcium by Standardized EDTA Solution
Determination of calcium by Standardized EDTA Solution Introduction The classic method of determining calcium and other suitable cations is titration with a standardized solution of ethylenediaminetetraacetic
More informationAP 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 informationEXPERIMENT 10: TITRATION AND STANDARDIZATION
EXPERIMENT 10: TITRATION AND STANDARDIZATION PURPOSE To determine the molarity of a NaOH solution by titrating it with a standard HCl solution. To determine the molarity of acetic acid in vinegar using
More informationStandard Methods for the Examination of Water and Wastewater
2320 ALKALINITY*#(1) 2320 A. Introduction 1. Discussion Alkalinity of a water is its acid-neutralizing capacity. It is the sum of all the titratable bases. The measured value may vary significantly with
More informationAnalysis of Vitamin C Using Iodine. Introduction
Analysis of Vitamin C Using Iodine Introduction Vitamin C (ascorbic acid) is oxidized to dehydroascorbic acid using a mild oxidizing agent such as iodine. The oxidation is a two- electron process, following
More information15. Acid-Base Titration. Discover the concentration of an unknown acid solution using acid-base titration.
S HIFT INTO NEUTRAL 15. Acid-Base Titration Shift into Neutral Student Instruction Sheet Challenge Discover the concentration of an unknown acid solution using acid-base titration. Equipment and Materials
More informationAcid-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 information3 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 informationAnalyzing the Acid in Vinegar
Analyzing the Acid in Vinegar Purpose: This experiment will analyze the percentage of acetic acid in store bought vinegar using titration. Introduction: Vinegar can be found in almost any home. It can
More informationOXIDATION-REDUCTION TITRATIONS-Permanganometry
Experiment No. Date OXIDATION-REDUCTION TITRATIONS-Permanganometry INTRODUCTION Potassium permanganate, KMnO 4, is probably the most widely used of all volumetric oxidizing agents. It is a powerful oxidant
More informationCalcium Analysis by EDTA Titration
Calcium Analysis by EDTA Titration ne of the factors that establish the quality of a water supply is its degree of hardness. The hardness of water is defined in terms of its content of calcium and magnesium
More information(1) Hydrochloric acid reacts with sodium hypochlorite to form hypochlorous acid: NaOCl(aq) + HCl(aq) HOCl(aq) + NaCl(aq) hypochlorous acid
The Determination of Hypochlorite in Bleach Reading assignment: Chang, Chemistry 10 th edition, pages 156-159. We will study an example of a redox titration in order to determine the concentration of sodium
More informationQ.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 informationTITRATION CURVES, INDICATORS, AND ACID DISSOCIATION CONSTANTS
TITRATION CURVES, INDICATORS, AND ACID DISSOCIATION CONSTANTS Adapted from "Chemistry with Computers" Vernier Software, Portland OR, 1997 INTRODUCTION Titration is the volumetric measurement of a solution
More informationCoordination Compounds with Copper (II) Prelab (Week 2)
Coordination Compounds with Copper (II) Prelab (Week 2) Name Total /10 SHOW ALL WORK NO WORK = NO CREDIT 1. What is the purpose of this experiment? 2. Write the generic chemical formula for the coordination
More informationPART I: PREPARATION OF SOLUTIONS AND STANDARDIZATION OF A BASE
TITRATION: STANDARDIZATION OF A BASE AND ANALYSIS OF STOMACH ANTACID TABLETS 2009, 1996, 1973 by David A. Katz. All rights reserved. Reproduction permitted for education use provided original copyright
More informationJuice Titration. Background. Acid/Base Titration
Juice Titration Background Acids in Juice Juice contains both citric and ascorbic acids. Citric acid is used as a natural preservative and provides a sour taste. Ascorbic acid is a water-soluble vitamin
More informationThe Determination of Acid Content in Vinegar
The Determination of Acid Content in Vinegar Reading assignment: Chang, Chemistry 10 th edition, pages 153-156. Goals We will use a titration to determine the concentration of acetic acid in a sample of
More informationEXPERIMENT 2 THE HYDROLYSIS OF t-butyl CHLORIDE. PURPOSE: To verify a proposed mechanism for the hydrolysis of t-butyl Chloride.
PURPOSE: To verify a proposed mechanism for the hydrolysis of t-butyl Chloride. PRINCIPLES: Once the Rate Law for a reaction has been experimentally established the next step is its explanation in terms
More informationDetermination of Citric Acid in Powdered Drink Mixes
Determination of Citric Acid in Powdered Drink Mixes Citric acid and its salts (sodium citrate and potassium citrate) are found in many foods, drinks, pharmaceuticals, shampoos, and cosmetics. The tartness
More informationStoichiometry Limiting Reagent Laboratory. Chemistry 118 Laboratory University of Massachusetts, Boston
Chemistry 118 Laboratory University of Massachusetts, Boston STOICHIOMETRY - LIMITING REAGENT -----------------------------------------------------------------------------------------------------------------------------
More informationexperiment5 Understanding and applying the concept of limiting reagents. Learning how to perform a vacuum filtration.
81 experiment5 LECTURE AND LAB SKILLS EMPHASIZED Synthesizing an organic substance. Understanding and applying the concept of limiting reagents. Determining percent yield. Learning how to perform a vacuum
More informationNeutralizing 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 informationAcetic Acid Content of Vinegar: An Acid-Base Titration E10-1
Experiment 10 Acetic Acid Content of Vinegar: An Acid-Base Titration E10-1 E10-2 The task The goal of this experiment is to determine accurately the concentration of acetic acid in vinegar via volumetric
More information1. 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 informationUnit 2: Quantities in Chemistry
Mass, Moles, & Molar Mass Relative quantities of isotopes in a natural occurring element (%) E.g. Carbon has 2 isotopes C-12 and C-13. Of Carbon s two isotopes, there is 98.9% C-12 and 11.1% C-13. Find
More informationWe 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 informationChem101: 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 informationEDTA Titrations 1: Standardization of EDTA and Analysis of Zinc in a Supplement Tablet. by Professor David Cash. September, 2008
CHEMICAL, ENVIRONMENTAL, AND BIOTECHNOLOGY DEPARTMENT EDTA Titrations 1: Standardization of EDTA and Analysis of Zinc in a Supplement Tablet by Professor David Cash September, 2008 Mohawk College is the
More informationNote: (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 informationTitrations. 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 informationRecovery of Elemental Copper from Copper (II) Nitrate
Recovery of Elemental Copper from Copper (II) Nitrate Objectives: Challenge: Students should be able to - recognize evidence(s) of a chemical change - convert word equations into formula equations - perform
More informationHOW TO MAKE STANDARD SOLUTIONS FOR CHEMISTRY
HOW TO MAKE STANDARD SOLUTIONS FOR CHEMISTRY Phillip Bigelow Chemists make two common types of "standard solutions": Molar solutions Normal solutions Both of these solutions are concentrations (or strengths
More informationQUESTION (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 informationEquilibria 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 informationFAJANS DETERMINATION OF CHLORIDE
EXPERIMENT 3 FAJANS DETERMINATION OF CHLORIDE Silver chloride is very insoluble in water. Addition of AgNO 3 to a solution containing chloride ions results in formation of a finely divided white precipitate
More informationFormulas, Equations and Moles
Chapter 3 Formulas, Equations and Moles Interpreting Chemical Equations You can interpret a balanced chemical equation in many ways. On a microscopic level, two molecules of H 2 react with one molecule
More informationChemical 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 informationAcid-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 informationSeparation by Solvent Extraction
Experiment 3 Separation by Solvent Extraction Objectives To separate a mixture consisting of a carboxylic acid and a neutral compound by using solvent extraction techniques. Introduction Frequently, organic
More informationDETERMINING THE ENTHALPY OF FORMATION OF CaCO 3
DETERMINING THE ENTHALPY OF FORMATION OF CaCO 3 Standard Enthalpy Change Standard Enthalpy Change for a reaction, symbolized as H 0 298, is defined as The enthalpy change when the molar quantities of reactants
More informationChapter 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 informationElement of same atomic number, but different atomic mass o Example: Hydrogen
Atomic mass: p + = protons; e - = electrons; n 0 = neutrons p + + n 0 = atomic mass o For carbon-12, 6p + + 6n 0 = atomic mass of 12.0 o For chlorine-35, 17p + + 18n 0 = atomic mass of 35.0 atomic mass
More informationChapter 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 informationChem 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 informationThe introduction of your report should be written on the on the topic of the role of indicators on acid base titrations.
Experiment # 13A TITRATIONS INTRODUCTION: This experiment will be written as a formal report and has several parts: Experiment 13 A: Basic methods (accuracy and precision) (a) To standardize a base (~
More informationDetermination of Aspirin using Back Titration
Determination of Aspirin using Back Titration This experiment is designed to illustrate techniques used in a typical indirect or back titration. You will use the NaH you standardized last week to back
More informationApparatus error for each piece of equipment = 100 x margin of error quantity measured
1) Error Analysis Apparatus Errors (uncertainty) Every time you make a measurement with a piece of apparatus, there is a small margin of error (i.e. uncertainty) in that measurement due to the apparatus
More informationI. 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 informationThe Empirical Formula of a Compound
The Empirical Formula of a Compound Lab #5 Introduction A look at the mass relationships in chemistry reveals little order or sense. The ratio of the masses of the elements in a compound, while constant,
More informationSaturated NaCl solution rubber tubing (2) Glass adaptor (2) thermometer adaptor heating mantle
EXPERIMENT 5 (Organic Chemistry II) Pahlavan/Cherif Dehydration of Alcohols - Dehydration of Cyclohexanol Purpose - The purpose of this lab is to produce cyclohexene through the acid catalyzed elimination
More informationTITRATION OF VITAMIN C
TITRATION OF VITAMIN C Introduction: In this lab, we will be performing two different types of titrations on ascorbic acid, more commonly known as Vitamin C. The first will be an acid-base titration in
More informationExperiment 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 informationProperties 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 informationChemistry 119: Experiment 7. Potentiometric Titration of Ascorbic Acid in Vitamin C Tablets
Chemistry 119: Experiment 7 Potentiometric Titration of Ascorbic Acid in Vitamin C Tablets Vitamin C is another name for ascorbic acid (C 6 H 8 O 6, see below ), a weak acid that can be determined by titration
More informationCHM1 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 informationSOLUBILITY, IONIC STRENGTH AND ACTIVITY COEFFICIENTS
SOLUBILITY, IONIC STRENGTH AND ACTIVITY COEFFICIENTS References: 1. See `References to Experiments' for text references.. W. C. Wise and C. W. Davies, J. Chem. Soc., 73 (1938), "The Conductivity of Calcium
More informationChemistry 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 informationExperiment 8 - Double Displacement Reactions
Experiment 8 - Double Displacement Reactions A double displacement reaction involves two ionic compounds that are dissolved in water. In a double displacement reaction, it appears as though the ions are
More informationCHM220 Nucleophilic Substitution Lab. Studying S N 1 and S N 2 Reactions: Nucloephilic Substitution at Saturated Carbon*
CHM220 Nucleophilic Substitution Lab Studying S N 1 and S N 2 Reactions: Nucloephilic Substitution at Saturated Carbon* Purpose: To convert a primary alcohol to an alkyl bromide using an S N 2 reaction
More informationAcid/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 informationANALYSIS OF VITAMIN C
Purpose To learn how to analyze food for vitamin C content and to examine various sources for vitamin C content. Caution Handle the glassware with caution to prevent breakage. When using a burner in the
More informationIB Chemistry. DP Chemistry Review
DP Chemistry Review Topic 1: Quantitative chemistry 1.1 The mole concept and Avogadro s constant Assessment statement Apply the mole concept to substances. Determine the number of particles and the amount
More informationColorimetric Determination of Iron in Vitamin Tablets
Cautions: 6 M hydrochloric acid is corrosive. Purpose: To colorimetrically determine the mass of iron present in commercial vitamin tablets using a prepared calibration curve. Introduction: Iron is considered
More informationA Volumetric Analysis (Redox Titration) of Hypochlorite in Bleach
CHEM 311L Quantitative Analysis Laboratory Revision 2.3 A Volumetric Analysis (Redox Titration) of Hypochlorite in Bleach In this laboratory exercise, we will determine the concentration of the active
More informationAqueous Solutions. Water is the dissolving medium, or solvent. Some Properties of Water. A Solute. Types of Chemical Reactions.
Aqueous Solutions and Solution Stoichiometry Water is the dissolving medium, or solvent. Some Properties of Water Water is bent or V-shaped. The O-H bonds are covalent. Water is a polar molecule. Hydration
More informationThis 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 informationChem 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 informationWhere the exp subscripts refer to the experimental temperature and pressure acquired in the laboratory.
Molar Volume of Carbon Dioxide Reading assignment: Julia Burdge, Chemistry 3rd edition, Chapter 10. Goals To determine the molar volume of carbon dioxide gas and the amount of sodium carbonate in a sample.
More informationDetermination of Ascorbic Acid in Vitamin C Tablets by Redox and Acid/Base Titrations
hemistry 211 Spring 2011 Purpose: Determination of Ascorbic Acid in Vitamin Tablets by Redox and Acid/Base Titrations To determine the quantity of Vitamin (ascorbic acid) found in commercially available
More informationName 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 informationLab 25. Acid-Base Titration and Neutralization Reactions: What Is the Concentration of Acetic Acid in Each Sample of Vinegar?
Lab 25. Acid-Base Titration and Neutralization Reactions: What Is the Concentration of Acetic Acid in Each Sample of Vinegar? Introduction Vinegar is basically a solution of acetic acid (CH3COOH). It is
More informationTopic 4 National Chemistry Summary Notes. Formulae, Equations, Balancing Equations and The Mole
Topic 4 National Chemistry Summary Notes Formulae, Equations, Balancing Equations and The Mole LI 1 The chemical formula of a covalent molecular compound tells us the number of atoms of each element present
More informationExperiment 4 (Future - Lab needs an unknown)
Experiment 4 (Future - Lab needs an unknown) USING A ph TITRATION TO DETERMINE THE ACID CONTENT OF SOFT DRINKS 2 lab periods Reading: Chapter 9, 185-197; Chapter 10, pg 212-218; Chapter 14 pg 317-323,
More informationEXPERIMENT 7 Reaction Stoichiometry and Percent Yield
EXPERIMENT 7 Reaction Stoichiometry and Percent Yield INTRODUCTION Stoichiometry calculations are about calculating the amounts of substances that react and form in a chemical reaction. The word stoichiometry
More informationChapter 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