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 16QRT
Without doing calculations, determine the pH of a buffer made front equimolar amounts of these acid-base pairs.
- (a) Nitrous acid and sodium nitrite
- (b) Ammonia and ammonium chloride
- (c) Formic acid and potassium formate
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Students have asked these similar questions
You wish to add enough NaOCl (sodium hypochlorite) to a 150 m³ swimming pool to provide
a dose of 5.0 mg/L TOTOCI as Cl2.
(a) How much NaOCI (kg) should you add? (Note: the equivalent weight of NaOCl is
based on the reaction: NaOCl + 2H + 2 e→CI + Na +H₂O.) (10 pts) (atomic
weight: Na 23, O 16, C1 35.5)
(b) The pH in the pool after the NaOCl addition is 8.67. To improve disinfection, you
want at least 90% of the TOTOCI to be in the form of HOCI (pKa 7.53). Assuming
that HOCI/OCI is the only weak acid/base group in solution, what volume (L) of
10 N HCl must be added to achieve the goal? (15 pts)
Note that part a) is a bonus question for undergraduate students. If you decide not to work on
this part of the question, you many assume TOTOCI = 7×10-5 M for part b).
Part A
2K(s)+Cl2(g)+2KCI(s)
Express your answer in grams to three significant figures.
Part B
2K(s)+Br2(1)→2KBr(s)
Express your answer in grams to three significant figures.
Part C
4Cr(s)+302(g)+2Cr2O3(s)
Express your answer in grams to three significant figures.
Part D
2Sr(s)+O2(g) 2SrO(s)
Express your answer in grams to three significant figures.
Thank you!
A solution contains 10-28 M TOTCO3 and is at pH 8.1. How much HCI (moles per liter of
solution) is required to titrate the solution to pH 7.0? (H2CO3: pKa1=6.35, pKa2=10.33)
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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