Introduction To Chemistry
5th Edition
ISBN: 9781259911149
Author: BAUER, Richard C., Birk, James P., Marks, Pamela
Publisher: Mcgraw-hill Education,
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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,…
Suppose 85 mL of a buffer solution that was 0.15 M
HCHO2 and 0.25 M NaCHO₂ had 7.5 mL of 0.10 M
hydrochloric acid added to it. Afterwards, 35 mL of
this mixture was measured out, placed inside an
Erlenmeyer flask, and diluted to 75 mL. What was
the concentration of the hydroxide ion in the
resulting solution in the flask? Ka for HCHO2, formic
acid, is 1.7 x 10-4.
a. 9.80 x 10-11 M
Ob. 2.81 x 10-7 M
c. 2.55 x 10-9 M
d.
8.94 x 10-11 M
e. 2.10 x 10-10 M
9.77 x 10-11 M
g. 1.12 x 10-4 M Incorrect
Of.
Oh. 1.91 x 10-10 M
Chapter 13 Solutions
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
- Write an introduction for the titration of acetic acid with NaOH and for the titration of Polyprotic acids with NaOH.arrow_forwardPetanoic (or valeric) acid is a weak organic acid with an unpleasant odour. Like other small carboxylic acids, it is used to make pleasant smelling esters that are used in perfumes, cosmetics, and food additives. Completed Part D In Part B, a 20.00 mL aliquot of a 0.195 mol L-1 pentanoic acid solution was titrated to its equivalence point with 19.7 mL of 0.198 mol L- 1 NaOH solution. At the equivalence point, all of the weak acid, pentanoic acid, is converted to its weak conjugate base, pentanoate. In part A, the Ka for pentanoic acid was determined to be 1.48×10-5. What is the pH at this equivalence point? 5.089 6.997 pentanoic acid 9.170 4.830 The pka of pentanoic acid is 4.830. 8.911arrow_forwardSuppose you are given solutions of 1.00 M acetic acid and 1.00 M sodium acetate and are asked to make 100.00 mL of buffer at pH 5.00 using only these two solutions. What volume, in milliliters, of acid would you need? The pKa of acetic acid is 4.75.arrow_forward
- Be sure to answer all parts. Which indicators that would be su ble for each of the following titrations: (a) CH;NH, with HBr thymol blue bromophenol blue methyl orange methyl red chlorophenol blue bromothymol blue O cresol red O phenolphthalein (b) HNO, with NaOH thymol blue bromophenol blue methyl orange methyl red chlorophenol blue bromothymol blue cresol red phenolphthalein (c) HNO, with KOH thymol blue O bromopbenol blue methyl orange methyl red chlorophenel bluearrow_forwardYou 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_forward
- What is the purpose of titration? What is the purpose of phenolphthalein? Why is phenolphthalein traditionally used in titrations?arrow_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_forwardCalculate 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_forward
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Acid-Base Equilibrium; Author: Bozeman Science;https://www.youtube.com/watch?v=l5fk7HPmo5g;License: Standard YouTube License, CC-BY
Introduction to Titrimetric analysis; Author: Vidya-mitra;https://www.youtube.com/watch?v=uykGVfn9q24;License: Standard Youtube License