EBK INTRODUCTION TO CHEMISTRY
5th Edition
ISBN: 9781260162165
Author: BAUER
Publisher: MCGRAW HILL BOOK COMPANY
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Chapter 13, Problem 109QP
(a)
Interpretation Introduction
Interpretation:
A balanced equation showing the acid and its conjugate base in equilibrium is to be written.
(b)
Interpretation Introduction
Interpretation:
The way in which the given buffer system prevents large
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The major component of vinegar is acetic acid, CH3COOH. Its Ka is 1.8 × 10-5 . One student used 1.000 M NaOH to titrate 25.00 mL vinegar. At the end point, 21.82 mL NaOH was used.
(a) What is the concentration of CH3COOH in vinegar?
(b) What is the pH of the solution at the end point?
(c) What indicator(s) the student should use in this titration? Explain
A buffer is prepared by adding 20.0 g of sodium acetate(CH3COONa) to 500 mL of a 0.150 M acetic acid(CH3COOH) solution. (a) Determine the pH of the buffer.(b) Write the complete ionic equation for the reaction thatoccurs when a few drops of hydrochloric acid are added tothe buffer. (c) Write the complete ionic equation for the reactionthat occurs when a few drops of sodium hydroxidesolution are added to the buffer.
Propionic acid, HC3H5O2, has Ka= 1.34 x 10–5.
(a) What is the molar concentration of H3O+ in 0.15 M HC3H5O2 and the pH of the solution?
(b) What is the Kb value for the propionate ion, C3H5O2–?
(c) Calculate the pH of 0.15 M solution of sodium propionate, NaC3H5O2.
(d) Calculate the pH of solution that contains 0.12 M HC3H5O2 and 0.25 M NaC3H5O2.
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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