EBK INTRODUCTION TO CHEMISTRY
5th Edition
ISBN: 9781260162165
Author: BAUER
Publisher: MCGRAW HILL BOOK COMPANY
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Chapter 13, Problem 101QP
Interpretation Introduction
Interpretation:
The change on titrating an acid of
Concept Introduction:
Indicators are brightly coloured organic dyes and are weak acids and bases. They give different colours in different
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1. (a) Calculate the pH after addition of 0.0, 5.0, 15.0, 25.0
40.0, 45.0, 49.00, 50.00, 51.00 55.00 and 60.00 mL of 0.1M NAOH in the titration of 50.00
mL of 0.1M HCl. (b) Construct a titration curve by plotting the pH (y-axis) against volume
of NaOH ( x-axis).
In the experiment, we used titration to determine the total acid content ofsamples, which we reported in terms of molarity. Reporting acidity through pHmeasurements is quite different, in that we can only measure the amount of theacid in its ionized form. You were tasked to investigate a clear aqueous solutionof an unknown monoprotic acid. You decided to use two methods togather data.Method 1 – TITRATION: A 10. mL aliquot of the sample was diluted with 25 mLdistilled water. Two drops of phenolphthalein were added and then it was titrated3.54 mL of 0.048 M standardized NaOH to the endpoint.Method 2 – pH STRIP: You took 1 mL of the sample and used a pH strip toestimate the pH, which turned out to be around 3.3. Another 1 mL of the samplewas diluted with 9 mL of water. The pH was taken again and is now around 3.8.a) Calculate the molarity of the acid using the titration data.b) If we assume that the titrated unknown is a strong acid, predict thepH of the sample.c) Using pH strip results,…
Consider the titration of 60.0 mL of 0.200 M pyridine with 0.400 M HCl. What is the pH at 0.00 mL, 15.00 mL, and 31.00 mL of the added acid?
Chapter 13 Solutions
EBK INTRODUCTION TO CHEMISTRY
Ch. 13 - How do acids and bases differ from other...Ch. 13 - Prob. 2QCCh. 13 - Prob. 3QCCh. 13 - Prob. 4QCCh. 13 - Prob. 5QCCh. 13 - Prob. 6QCCh. 13 - Prob. 1PPCh. 13 - Prob. 2PPCh. 13 - Prob. 3PPCh. 13 - Prob. 4PP
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- For conjugate acidbase pairs, how are Ka and Kb related? Consider the reaction of acetic acid in water CH3CO2H(aq)+H2O(l)CH3CO2(aq)+H3O+(aq) where Ka = 1.8 105 a. Which two bases are competing for the proton? b. Which is the stronger base? c. In light of your answer to part b. why do we classify the acetate ion (CH3CO2) as a weak base? Use an appropriate reaction to justify your answer. In general, as base strength increases, conjugate acid strength decreases. Explain why the conjugate acid of the weak base NH3 is a weak acid. To summarize, the conjugate base of a weak acid is a weak base and the conjugate acid of a weak base is a weak acid (weak gives you weak). Assuming Ka for a monoprotic strong acid is 1 106, calculate Kb for the conjugate base of this strong acid. Why do conjugate bases of strong acids have no basic properties in water? List the conjugate bases of the six common strong acids. To tie it all together, some instructors have students think of Li+, K+, Rb+, Cs+, Ca2+, Sr2+, and Ba2+ as the conjugate acids of the strong bases LiOH, KOH. RbOH, CsOH, Ca(OH)2, Sr(OH)2, and Ba(OH)2. Although not technically correct, the conjugate acid strength of these cations is similar to the conjugate base strength of the strong acids. That is, these cations have no acidic properties in water; similarly, the conjugate bases of strong acids have no basic properties (strong gives you worthless). Fill in the blanks with the correct response. The conjugate base of a weak acid is a_____base. The conjugate acid of a weak base is a_____acid. The conjugate base of a strong acid is a_____base. The conjugate acid of a strong base is a_____ acid. (Hint: Weak gives you weak and strong gives you worthless.)arrow_forwardWhich of the acid-base indicators discussed in this chapter would be suitable for the titration of (a) HNO3 with KOH. (b) KOH with acetic acid. (c) HCl with NH3. (d) KOH with HNO2. Explain your answers.arrow_forward8-58 What is the connection between buffer action and Le Chatelier's principle?arrow_forward
- You were asked to estimate the pH of a 15mL of 0.09N of HCl when 16.9mL of 0.085N NaOH is added to a solution. Your supervisor informed you that she added 100 mL of diluent. With your computed pH and Phenolphthalein as the indicator [pH range: 8.00 – 10.00], would you expect a color change? Yes or No?arrow_forwardIn the titration of 40.00 mL of 0.600 M KOH with 0.200M HCI, what is the pH at 120.00 mL of titrant added? Enter your answer in scientific notation (such as (3.08x10^-1)) with 3 sig figs. Do not include any units in your answer. Do not round any intermediate calculations. Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: x10 Answerarrow_forwardA solution has a pH of 4.5. What would be the color of the solution if each of the following indicators were added? (See the figure below.) pH 10 11 12 13 Bromphenol Blue Methyl Orange Bromcresol Green Methyl Red Alizarin Bromthymol Blue Phenol Red o-Cresolphthalein Phenolphthalein The pH ranges shown are approximate. Specific transition ranges depend on the indicator solvent chosen. a. bromphenol blue Oyellow green blue O red O colorless b. bromthymol blue Oyellow O green O blue O red O olorless c. bromcresol green Oyellow O green blue Ored O colorless d. o-cresolphthaleinarrow_forward
- Calculate the pH of a mixture of 0.12 M acetic acid and 0.25 M sodium acetate. The pKa of acetic acid is 4.76.arrow_forwardIn Part A, a 15.00 mL aliquot of a 0.155 mol L-1 3-methylbutanoic acid solution was titrated to its equivalence point with 11.7 mL of 0.198 molL-1 NaOH solution. At the equivalence point, all of the weak acid, 3-methylbutanoic acid, is converted to its weak conjugate base, 3-methylbutanoate. What is the pH at this equivalence point? 6.957 4.770 8.855 5.145 O 9.230arrow_forwardHow do I determine the concentration of hydrochloric acid through acid-base titration? I mean what experiment could be done to do it. Like what materials or methods to usearrow_forward
- a) Calculate the molar ratio of formic acid/sodium formate to prepare a pH-4.00 buffer solution. b) If you have 1.000 g of formic acid dissolved in 1 L of water, how many grams of sodium formate do you need to add to this solution to prepare the pH-4.00 buffer?arrow_forwardWhich one of the buffer solutions (pH 4.20 or pH 4.90) demonstrated the least change in pH, and hence the best buffering ability, upon the addition of the 2 ml NaOH? Explain why.arrow_forwarda) Why can you not prepare a solution of pH = 8 by diluting sufficiently a 0.01 M solution of HCl with water? b) You could determine Ka for benzoic acid by measuring the pH of a 0.010 M solution of benzoic acid. Why is the graphical method used in this experiment a better way of determining Ka? c) List the measurements along with their uncertainties made in the determination of the molar mass of benzoic acid. Calculate the uncertainty in the mola r mass of benzoic acid determined by the titration.arrow_forward
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Introduction to Titrimetric analysis; Author: Vidya-mitra;https://www.youtube.com/watch?v=uykGVfn9q24;License: Standard Youtube License