Chemistry: The Central Science (14th Edition)
14th Edition
ISBN: 9780134414232
Author: Theodore E. Brown, H. Eugene LeMay, Bruce E. Bursten, Catherine Murphy, Patrick Woodward, Matthew E. Stoltzfus
Publisher: PEARSON
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Textbook Question
Chapter 17, Problem 24E
A buffer is prepared by adding 10.0 g of ammonium chloride (NH4CI) to 250 mL of 1.00 M NH3 solution.
- What is the pH of this buffer?
- Write the complete ionic equation for the reaction that occurs when a few drops of nitric acid are added to the buffer.
- Write the complete ionic equation for the reaction that occurs when a few drops of potassium hydroxide solution are added to the buffer.
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1) A buffer solution contains 0.350 M ammonium bromide and 0.400 M ammonia.If 0.0452 moles of perchloric acid are added to 225 mL of this buffer, what is the pH of the resulting solution ?(Assume that the volume change does not change upon adding perchloric acid)pH =
2) A buffer solution contains 0.320 M hypochlorous acid and 0.383 M potassium hypochlorite.If 0.0405 moles of hydrochloric acid are added to 225 mL of this buffer, what is the pH of the resulting solution ?(Assume that the volume change does not change upon adding hydrochloric acid)pH
A buffer solution is formed by adding 0.180 moles of solid potassium nitrite, KNO₂, to 200.0 ml of 0.600 M Nitrous acid, HNO₂ solution. You may assume that the change in volume is negligible upon addition of the solid.
Calculate the pH of the buffer solution.pH = AnswerCalculate the pH of the buffer solution after the addition of 8.00 ml of 1.50 M HCl.pH = Answer
A buffer solution is prepared by dissolving 1.000 g of sodium acetate (CH3COONa) into 100.00 mL of a 0.100 M solution of acetic acid. Then 2.00 mL of a 2.00 M solution of hydrochloric acid is added to the acetic acid/sodium acetate buffer solution. The Ka of acetic acid is 1.8 ×10−5.
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Chapter 17 Solutions
Chemistry: The Central Science (14th Edition)
Ch. 17.1 - For the generic equilibrium HA(aq)H+(aq)+A(aq) ,...Ch. 17.1 - Practice Exercise 2 Calculate the pH of a solution...Ch. 17.1 - Calculate the concentration of the lactate ion in...Ch. 17.1 - Practice Exercise 2 Calculate the format ion...Ch. 17.2 - Practice Exercise 1 If the pH of a buffer solution...Ch. 17.2 - Prob. 17.3.2PECh. 17.2 - Prob. 17.4.1PECh. 17.2 - Prob. 17.4.2PECh. 17.2 - Calculate the number of grams of ammonium chloride...Ch. 17.2 - Prob. 17.5.2PE
Ch. 17.2 - Prob. 17.6.1PECh. 17.2 - Determine The pH of the original buffer described...Ch. 17.3 - An acid-base titration is performed: 250.0 mL of...Ch. 17.3 - Prob. 17.7.2PECh. 17.3 - Prob. 17.8.1PECh. 17.3 - Calculate the pH in the solution formed by adding...Ch. 17.3 - Prob. 17.9.1PECh. 17.3 - Prob. 17.9.2PECh. 17.4 - Which of these expressions correctly expresses the...Ch. 17.4 - Prob. 17.10.2PECh. 17.4 - You add 10.0 grams of solid copper(II) phosphate,...Ch. 17.4 - Prob. 17.11.2PECh. 17.4 - Prob. 17.12.1PECh. 17.4 - Prob. 17.12.2PECh. 17.5 - Consider a saturated solution of the salt MA3, in...Ch. 17.5 - Prob. 17.13.2PECh. 17.5 - Prob. 17.14.1PECh. 17.5 - Prob. 17.14.2PECh. 17.5 - Prob. 17.15.1PECh. 17.5 - Prob. 17.15.2PECh. 17.6 - An insoluble salt MA has a Kap of 1.0 × 10-10. Two...Ch. 17.6 - Does a precipitate form when 0.050 L of 2.0 × 10-2...Ch. 17.6 - Under what conditions does an ionic compound...Ch. 17.6 - Prob. 17.17.2PECh. 17 - Prob. 1DECh. 17 - The following boxes represent aqueos solutions...Ch. 17 - Prob. 2ECh. 17 - Prob. 3ECh. 17 - Prob. 4ECh. 17 - Prob. 5ECh. 17 - Prob. 6ECh. 17 - Prob. 7ECh. 17 - Prob. 8ECh. 17 - 17.9 The following graphs represent the behavior...Ch. 17 - Prob. 10ECh. 17 - 17.11 The graph below shows the solubility of a...Ch. 17 - 17.12 Three cations, Ni+2, Cu+2, and Ag+, are...Ch. 17 - Prob. 13ECh. 17 - Prob. 14ECh. 17 - Prob. 15ECh. 17 - Use information from Appendix D to calculate the...Ch. 17 - Prob. 17ECh. 17 - a. calculate the percent ionization of 0.125 M...Ch. 17 - Prob. 19ECh. 17 - 17.20 Which of the following solutions is a...Ch. 17 - Prob. 21ECh. 17 - Calculate the pH of a buffer that is 0.105n M in...Ch. 17 - Prob. 23ECh. 17 - A buffer is prepared by adding 10.0 g of ammonium...Ch. 17 - You are asked to prepare a pH = 3.00 buffer...Ch. 17 - You are asked to prepare an pH = 4.00 buffer...Ch. 17 - Prob. 27ECh. 17 - Prob. 28ECh. 17 - Prob. 29ECh. 17 - Prob. 30ECh. 17 - Prob. 31ECh. 17 - Prob. 32ECh. 17 - The accompanying graph shows the titration curves...Ch. 17 - Prob. 34ECh. 17 - 17.35 The samples of nitric and acetic acids shows...Ch. 17 - 17.36 Determine whether each of the following...Ch. 17 - Prob. 37ECh. 17 - Prob. 38ECh. 17 - Prob. 39ECh. 17 - Assume that 30.0 mL of a M solution of a week base...Ch. 17 - Prob. 41ECh. 17 - Prob. 42ECh. 17 - Prob. 43ECh. 17 - Prob. 44ECh. 17 - Prob. 45ECh. 17 - Consider the titration of 30.0 mL of 0.050 M NH3...Ch. 17 - Prob. 47ECh. 17 - Prob. 48ECh. 17 - 17.49 for each statement, incate whether it is...Ch. 17 - The solubility of two slighty soluble salts of...Ch. 17 - Prob. 51ECh. 17 - 17.52
a. true or false: solubility and...Ch. 17 - If the molar solubility CaF2 at 35 C is 1.24 *10-3...Ch. 17 - Prob. 54ECh. 17 - Prob. 55ECh. 17 - Prob. 56ECh. 17 - using calculate the molar solubility of AgBr in a....Ch. 17 - calculate the solubility of LaF3 in grams per...Ch. 17 - Prob. 59ECh. 17 - Consider a beaker containing a saturated solution...Ch. 17 - Calculate the solubility of Mn (OH) 2 in grams per...Ch. 17 - Calculate the molar solubility of Ni (OH) 2 when...Ch. 17 - 17.63 Which of the following salts will be...Ch. 17 - For each of the following slightly soluble salts,...Ch. 17 - Prob. 65ECh. 17 - Prob. 66ECh. 17 - Use values of Kap for Agl and Kf for Ag (CN) 2- to...Ch. 17 - Prob. 68ECh. 17 - Prob. 69ECh. 17 - Prob. 70ECh. 17 - Calculate the minimum pH needed to precipitate Mn...Ch. 17 - Prob. 72ECh. 17 - Prob. 73ECh. 17 - Prob. 74ECh. 17 - Prob. 75ECh. 17 - Prob. 76ECh. 17 - A solution containing several metal ions is...Ch. 17 - An unknown solid is entirely soluble in water. On...Ch. 17 - Prob. 79ECh. 17 - Prob. 80ECh. 17 - 17.81
Precipitation of the group 4 cautions of...Ch. 17 - Prob. 82ECh. 17 - Prob. 83AECh. 17 - Prob. 84AECh. 17 - Furoic acid (HC5H3O3) has a K value of 6.76 x 10-4...Ch. 17 - Prob. 86AECh. 17 - Equal quantities of 0.010 M solution of an acid HA...Ch. 17 - Prob. 88AECh. 17 - 17.89 A biochemist needs 750 ml of an acetic...Ch. 17 - A sample of 0.2140 g of an unknown monophonic acid...Ch. 17 - A sample of 0.1687 g of an unknown monoprotic acid...Ch. 17 - Prob. 92AECh. 17 - Prob. 93AECh. 17 - What is the pH of a solution made by mixing 0.30...Ch. 17 - Suppose you want to do a physiological experiment...Ch. 17 - Prob. 96AECh. 17 - Prob. 97AECh. 17 - For each pair of compounds, use Kap values to...Ch. 17 - Prob. 99AECh. 17 - Tooth enamel is composed of hydroxyapatite, whose...Ch. 17 - Salts containing the phosphate ion are added to...Ch. 17 - Prob. 102AECh. 17 - 17.103 The solubility –product constant for barium...Ch. 17 - Prob. 104AECh. 17 - Prob. 105AECh. 17 - A buffer of what pH is needed to give a Mg2+...Ch. 17 - The value of Kap for Mg3(AsO4)2 is 2.1 10-20 ....Ch. 17 - Prob. 108AECh. 17 - Prob. 109AECh. 17 - Prob. 110IECh. 17 - Prob. 111IECh. 17 - Prob. 112IECh. 17 - Prob. 113IECh. 17 - Prob. 114IECh. 17 - Prob. 115IECh. 17 - Prob. 116IECh. 17 - A concentration of 10-100 parts per billion (by...Ch. 17 - Prob. 118IECh. 17 - Prob. 119IECh. 17 - In nonaqueous solvents, it is possible to react HF...
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