Chemistry: The Molecular Science
5th Edition
ISBN: 9781285199047
Author: John W. Moore, Conrad L. Stanitski
Publisher: Cengage Learning
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Textbook Question
Chapter 15, Problem 17QRT
Without doing calculations, determine the pH of a buffer made front equimolar amounts of these acid-base pairs.
- (a) Phosphoric acid and sodium dihydrogen phosphate
- (b) Sodium monohydrogen phosphate and sodium dihydrogen phosphate
- (c) Sodium phosphate and sodium monohydrogen phosphate
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Without detailed calculation and RICE table, determine whether the following solutions are acidic or basic, buffer or not buffer. Explain your answers by identifying the major species and the dominate chemical reaction.
(a) 1M NaCl + 1M HCl in equal amounts
(b) 1M NH4Cl + 1M NH3 in equal amounts
(c) 1M Na2C2O4 + 1M HCl in equal amounts
(d) 2M H3PO4 + 3M NaOH in equal amounts
In each of the following questions, assume that there is no volume change when HCl is added to water in part (a) or the phosphate buffer in part (c).
(a) Calculate the pH when 0.049 moles of HCl are added to 1.000 liter of water.
(b) What is the difference between the pH of pure water (pH 7.00) and the pH of the solution after HCl was added?
(c) Calculate the pH when 0.049 moles of HCl are added to 1.000 liters of a buffer containing 0.277 M KH2PO4 and 0.208 M K2HPO4 .
(d) The pH before the HCl was added is equal to 7.083. What is the difference between the pH before adding the HCl and after adding the HCl?
Calculate the pH of the following buffer solutions:
(a) a solution made by dissolving 2.668 g KH2PO4 and 2.095 g K2HPO4 in water to give 200. mL of solution. Stepwise acid dissociation constants for phosphoric acid may be found in your textbook.
(b) a solution made by mixing 35.00 mL 0.33 M NH2OH with 15.00 mL 0.27 M NH3OHCl. The base dissociation constant Kb is 6.60 x 10-9 for NH2OH. Assume that the final volume is the sum of the volunes of the two solutions that are mixed.
Chapter 15 Solutions
Chemistry: The Molecular Science
Ch. 15.1 - Predict whether 1.0 L of each solution is a...Ch. 15.1 - Calculate the pH of blood containing 0.0020-M...Ch. 15.1 - Prob. 15.2ECh. 15.1 -
Calculate the ratio of [] to [] in blood at a...Ch. 15.1 - Use the data in Table 15.1 to select a conjugate...Ch. 15.1 -
Calculate the mole ratio of sodium acetate and...Ch. 15.1 - Calculate the pH of these buffers.
Ch. 15.1 - If an abnormally high CO2 concentration is present...Ch. 15.1 - Calculate the minimum mass (g) of KOH that would...Ch. 15.2 - For the titration of 50.0 mL of 0.100-M HCl with...
Ch. 15.2 - Draw the titration curve for the titration of 50.0...Ch. 15.2 - Use the Ka expression and value for acetic acid to...Ch. 15.2 - Explain why the curve for the titration of acetic...Ch. 15.4 - Write the Ksp expression for each of these...Ch. 15.4 - The Ksp of AgBr at 100 C is 5 1010. Calculate the...Ch. 15.4 - A saturated solution of silver oxalate. Ag2C2O4....Ch. 15.4 - Prob. 15.9CECh. 15.5 - Consider 0.0010-M solutions of these sparingly...Ch. 15.5 - Prob. 15.11PSPCh. 15.5 - Calculate the solubility of PbCl2 in (a) pure...Ch. 15.5 - Prob. 15.13PSPCh. 15.6 - (a) Determine whether AgCl precipitates from a...Ch. 15.6 - Prob. 15.15PSPCh. 15 - Prob. 1SPCh. 15 - Choose a weak-acid/weak-base conjugate pair from...Ch. 15 - Prob. 4SPCh. 15 - Define the term buffer capacity.Ch. 15 - What is the difference between the end point and...Ch. 15 - What are the characteristics of a good acid-base...Ch. 15 - A strong acid is titrated with a strong base, such...Ch. 15 - Repeat the description for Question 4, but use a...Ch. 15 - Use Le Chatelier’s principle to explain why PbCl2...Ch. 15 - Describe what a complex ion is and give an...Ch. 15 - Define the term “amphoteric”.
Ch. 15 - Distinguish between the ion product (Q) expression...Ch. 15 - Describe at least two ways that the solubility of...Ch. 15 - Briefly describe how a buffer solution can control...Ch. 15 - Identify each pair that could form a buffer. (a)...Ch. 15 - Identify each pair that could form a buffer. (a)...Ch. 15 - Many natural processes can be studied in the...Ch. 15 - Which of these combinations is the best to buffer...Ch. 15 - Without doing calculations, determine the pH of a...Ch. 15 - Without doing calculations, determine the pH of a...Ch. 15 - Select from Table 15.1 a conjugate acid-base pair...Ch. 15 - Select from Table 15.1 a conjugate acid-base pair...Ch. 15 - Calculate the mass of sodium acetate, NaCH3COO,...Ch. 15 - Calculate the mass in grams of ammonium chloride,...Ch. 15 - A buffer solution can be made from benzoic acid,...Ch. 15 - A buffer solution is prepared from 5.15 g NH4NO3...Ch. 15 - You dissolve 0.425 g NaOH in 2.00 L of a solution...Ch. 15 - A buffer solution is prepared by adding 0.125 mol...Ch. 15 - If added to 1 L of 0.20-M acetic acid, CH3COOH,...Ch. 15 - If added to 1 L of 0.20-M NaOH, which of these...Ch. 15 - Calculate the pH change when 10.0 mL of 0.100-M...Ch. 15 - Prob. 29QRTCh. 15 - Prob. 30QRTCh. 15 - Prob. 31QRTCh. 15 - The titration curves for two acids with the same...Ch. 15 - Explain why it is that the weaker the acid being...Ch. 15 - Prob. 34QRTCh. 15 - Consider all acid-base indicators discussed in...Ch. 15 - Which of the acid-base indicators discussed in...Ch. 15 - It required 22.6 mL of 0.0140-M Ba(OH)2 solution...Ch. 15 - It took 12.4 mL of 0.205-M H2SO4 solution to...Ch. 15 - Vitamin C is a monoprotic acid. To analyze a...Ch. 15 - An acid-base titration was used to find the...Ch. 15 - Calculate the volume of 0.150-M HCl required to...Ch. 15 - Calculate the volume of 0.225-M NaOH required to...Ch. 15 - Prob. 43QRTCh. 15 - Prob. 44QRTCh. 15 - Prob. 45QRTCh. 15 - Explain why rain with a pH of 6.7 is not...Ch. 15 - Identify two oxides that are key producers of acid...Ch. 15 - Prob. 48QRTCh. 15 - Prob. 49QRTCh. 15 - Prob. 50QRTCh. 15 - Prob. 51QRTCh. 15 - A saturated solution of silver arsenate, Ag3AsO4,...Ch. 15 - Prob. 53QRTCh. 15 - Prob. 54QRTCh. 15 - Prob. 55QRTCh. 15 - Prob. 56QRTCh. 15 - Prob. 57QRTCh. 15 - Prob. 58QRTCh. 15 - Prob. 59QRTCh. 15 - Prob. 60QRTCh. 15 - Prob. 61QRTCh. 15 - Prob. 62QRTCh. 15 - Prob. 63QRTCh. 15 - Prob. 64QRTCh. 15 - Predict what effect each would have on this...Ch. 15 - Prob. 66QRTCh. 15 - Prob. 67QRTCh. 15 - The solubility of Mg(OH)2 in water is...Ch. 15 - Prob. 69QRTCh. 15 - Prob. 70QRTCh. 15 - Prob. 71QRTCh. 15 - Prob. 72QRTCh. 15 - Write the chemical equation for the formation of...Ch. 15 - Prob. 74QRTCh. 15 - Prob. 75QRTCh. 15 - Prob. 76QRTCh. 15 - Prob. 77QRTCh. 15 - Prob. 78QRTCh. 15 - Prob. 79QRTCh. 15 - Prob. 80QRTCh. 15 - Prob. 81QRTCh. 15 - Solid sodium fluoride is slowly added to an...Ch. 15 - Prob. 83QRTCh. 15 - Prob. 84QRTCh. 15 - A buffer solution was prepared by adding 4.95 g...Ch. 15 - Prob. 86QRTCh. 15 - Prob. 87QRTCh. 15 - Prob. 88QRTCh. 15 - Prob. 89QRTCh. 15 - Which of these buffers involving a weak acid HA...Ch. 15 - Prob. 91QRTCh. 15 - Prob. 92QRTCh. 15 - When 40.00 mL of a weak monoprotic acid solution...Ch. 15 - Each of the solutions in the table has the same...Ch. 15 - Prob. 95QRTCh. 15 - Prob. 97QRTCh. 15 - The average normal concentration of Ca2+ in urine...Ch. 15 - Explain why even though an aqueous acetic acid...Ch. 15 - Prob. 100QRTCh. 15 - Prob. 101QRTCh. 15 - Prob. 102QRTCh. 15 - Prob. 103QRTCh. 15 - Prob. 104QRTCh. 15 - Apatite, Ca5(PO4)3OH, is the mineral in teeth.
On...Ch. 15 - Calculate the maximum concentration of Mg2+...Ch. 15 - Prob. 107QRTCh. 15 - Prob. 108QRTCh. 15 - The grid has six lettered boxes, each of which...Ch. 15 - Consider the nanoscale-level representations for...Ch. 15 - Consider the nanoscale-level representations for...Ch. 15 - Prob. 112QRTCh. 15 - Prob. 113QRTCh. 15 - Prob. 114QRTCh. 15 - Prob. 115QRTCh. 15 - You want to prepare a pH 4.50 buffer using sodium...Ch. 15 - Prob. 117QRTCh. 15 - Prob. 118QRTCh. 15 - Prob. 119QRTCh. 15 - Prob. 120QRTCh. 15 - Prob. 121QRTCh. 15 - Prob. 122QRTCh. 15 - You are given four different aqueous solutions and...Ch. 15 - Prob. 124QRTCh. 15 - Prob. 126QRTCh. 15 - Prob. 15.ACPCh. 15 - Prob. 15.BCP
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