EBK INTRODUCTION TO CHEMISTRY
5th Edition
ISBN: 9781260162165
Author: BAUER
Publisher: MCGRAW HILL BOOK COMPANY
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Chapter 13, Problem 102QP
What would you expect to observe if you ran a titration of a base at a
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Explain how the pH of a mixture of aqueous ammonium chloride and aqueous ammonium remains constant when a small amount of strong base is added.Give suitable equations in your explanation.
Sodium hypochlorite solution is also known as bleach. It contains the hypochlorite ion ClO-.
(a) Write an equation for the reaction between hypochlorite ion and ammonium ion. Label the acids and bases in the forward and reverse reactions. Identify the two conjugate acid-base pairs.
(b) This equilibrium favors the reactants. Which of the acids is stronger and donates protons more readily?
Suppose 50.00 mL of 0.100 M HCl is titrated with 0.200 M NaOH.
Calculate the pH of the resulting mixture after the addition of 13.4 mL (total) of strong base. Enter your answer to 2 decimal places.
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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Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- You have a solution of the weak acid HA and add some of the salt NaA to it. What are the major species in the solution? What do you need to know to calculate the pH of the solution, and how would you use this information? How does the pH of the solution of just the HA compare with that of the final mixture? Explain.arrow_forwardEstimate the pH that results when the following two solutions are mixed. a) 50 mL of 0.3 M CH3COOH and 50 mL of 0.4 M KOH b) 100 mL of 0.3 M CH3COOH and 50 mL of 0.4 M NaOH c) 150 mL of 0.3 M CH3COOH and 100 mL of 0.3 M Ba(OH)2 d) 200 mL of 0.3 M CH3COOH and 100 mL of 0.3 M Ba(OH)2arrow_forwardUsing an acetic acid/sodium acetate buffer solution, what ratio of conjugate base to acid will you need to maintain the pH at 5.00? Describe how you would prepare such a solution.arrow_forward
- What is a salt? List some anions that behave as weak bases in water. List some anions that have no basic properties in water. List some cations that behave as weak acids in water. List some cations that have no acidic properties in water. Using these lists, give some formulas for salts that have only weak base properties in water. What strategy would you use to solve for the pH of these basic salt solutions? Identify some salts that have only weak acid properties in water. What strategy would you use to solve for the pH of these acidic salt solutions? Identify some salts that have no acidic or basic properties in water (produce neutral solutions). When a salt contains both a weak acid ion and a weak base ion, how do you predict whether the solution pH is acidic, basic, or neutral?arrow_forwardWrite two BrnstedLowry acid-base reactions and show how they represent proton-transfer reactions.arrow_forwardUsing the diagrams shown in Problem 10-117, which of the solutions would have the greatest buffer capacity, that is, greatest protection against pH change, when the following occurs? a. A strong acid is added to the solution. b. A strong base is added to the solution.arrow_forward
- Consider all acid-base indicators discussed in this chapter. Which of these indicators would be suitable for the titration of each of these? (a) NaOH with HClO4 (b) acetic acid with KOH (c) NH3 solution with HBr (d) KOH with HNO3 Explain your choices.arrow_forwarda) What is the pH of a solution prepared by adding 11.1 mL of 0.50 M NaOH solution to 200. mL of a solution which is 0.40 M in NH4+ and 0.40 M in NH3? The Kb of NH3 is 1.8 x 10-5. The correct answer should be reported to two places past the decimal. b) Caculate the pH of a solution prepared by mixing 84.7 mL of a 0.25 M aqueous aniline solution (C6H5NH2, Kb = 4.3 x 10-10) with 100. mL of a 0.11 M aqueous nitric acid solution. Your pH should be reported to two places past the decimal point.arrow_forwardA 0.1724-g sample of an unknown monoprotic acid was dissolved in 26.9 mL of water and titrated with 0.0623 M NaOH solution. The volume of base required to bring the solution to the equivalence point was 19.8 mL. (a) Calculate the molar mass of the acid. (b) After 11.5 mL of base had been added during the titration, the pH was determined to be 5.66. What is the Ka of the unknown acid?arrow_forward
- A 0.1276 g sample of an unknown monoprotic acid was dissolved in 25.0 mL of water and titrated with 0.0633 M NaOH solution. The volume of base required to bring the solution to the equivalence point was 18.4 mL. (a) Calculate the molar mass of the acid. (b) After 10.0 mL of base had been added during the titration, the pH was determined to be 5.87. What is the Ka of the unknown acid? *only need help with barrow_forwardSuppose 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 Marrow_forwardCan you distinguish between a strong acid and weak acid (strong base and weak base) by using only the pH indicators like bromothymol blue , litmus paper and pH paper?arrow_forward
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