Chemistry: Principles and Reactions
8th Edition
ISBN: 9781305079373
Author: William L. Masterton, Cecile N. Hurley
Publisher: Cengage Learning
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Chapter 14, Problem 59QAP
A solution of an unknown weak base (nonelectrolyte) at 25°C has an osmotic pressure of 1.287 atm and a pH of 8.94. (Assume that, in the equation for
[Chapter 101,
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Chapter 14 Solutions
Chemistry: Principles and Reactions
Ch. 14 - Write a net ionic equation for the reaction...Ch. 14 - Write a net ionic equation for the reaction...Ch. 14 - Write a balanced net ionic equation for the...Ch. 14 - Write a balanced net ionic equation for the...Ch. 14 - Calculate K for the reactions in Question 1.Ch. 14 - Calculate K for the reactions in Question 2.Ch. 14 - Prob. 7QAPCh. 14 - Calculate K for the reactions in Question 4.Ch. 14 - Calculate [H+] and pH in a solution in which...Ch. 14 - Calculate [OH-] and pH in a solution in which the...
Ch. 14 - A buffer is prepared by dissolving 0.0250 mol of...Ch. 14 - A buffer is prepared by dissolving 0.062 mol of...Ch. 14 - A buffer solution is prepared by adding 15.00 g of...Ch. 14 - A buffer solution is prepared by adding 5.50 g of...Ch. 14 - A solution with a pH of 9.22 is prepared by adding...Ch. 14 - An aqueous solution of 0.057 M weak acid, HX, has...Ch. 14 - Which of the following would form a buffer if...Ch. 14 - Which of the following would form a buffer if...Ch. 14 - Calculate the pH of a solution prepared by mixing...Ch. 14 - Calculate the pH of a solution prepared by mixing...Ch. 14 - Calculate the pH of a solution prepared by mixing...Ch. 14 - Calculate the pH of a solution prepared by mixing...Ch. 14 - Consider the weak acids in Table 13.2. Which...Ch. 14 - Prob. 24QAPCh. 14 - A sodium hydrogen carbonate-sodium carbonate...Ch. 14 - You want to make a buffer with a pH of 10.00 from...Ch. 14 - Prob. 27QAPCh. 14 - The buffer capacity indicates how much OH- or H+...Ch. 14 - A buffer is made up of 0.300 L each of 0.500 M...Ch. 14 - A buffer is made up of 239 mL of 0.187 M potassium...Ch. 14 - Enough water is added to the buffer in Question 29...Ch. 14 - Enough water is added to the buffer in Question 30...Ch. 14 - A buffer is prepared in which the ratio [ H2PO4...Ch. 14 - A buffer is prepared using the butyric...Ch. 14 - Blood is buffered mainly by the HCO3 H2CO3 buffer...Ch. 14 - There is a buffer system in blood H2PO4 HPO42 that...Ch. 14 - Given three acid-base indicators—methyl orange...Ch. 14 - Given the acid-base indicators in Question 37,...Ch. 14 - Metacresol purple is an indicator that changes...Ch. 14 - Thymolphthalein is an indicator that changes from...Ch. 14 - When 25.00 mL of HNO3 are titrated with Sr(OH)2,...Ch. 14 - A solution of KOH has a pH of 13.29. It requires...Ch. 14 - A solution consisting of 25.00 g NH4Cl in 178 mL...Ch. 14 - A 50.0-mL sample of NaHSO3 is titrated with 22.94...Ch. 14 - A sample of 0.220 M triethylamine, (CH3CH2)3 N, is...Ch. 14 - A 35.00-mL sample of 0.487 M KBrO is titrated with...Ch. 14 - A 0.4000 M solution of nitric acid is used to...Ch. 14 - A 0.2481 M solution of KOH is used to titrate...Ch. 14 - Consider the titration of butyric acid (HBut) with...Ch. 14 - Morphine, C17H19O3N, is a weak base (K b =7.4107)....Ch. 14 - Consider a 10.0% (by mass) solution of...Ch. 14 - A solution is prepared by dissolving 0.350 g of...Ch. 14 - Prob. 53QAPCh. 14 - Ammonia gas is bubbled into 275 mL of water to...Ch. 14 - For an aqueous solution of acetic acid to be...Ch. 14 - Prob. 56QAPCh. 14 - Prob. 57QAPCh. 14 - Water is accidentally added to 350.00 mL of a...Ch. 14 - A solution of an unknown weak base...Ch. 14 - Consider an aqueous solution of HF. The molar heat...Ch. 14 - Each symbol in the box below represents a mole of...Ch. 14 - Use the same symbols as in Question 61 ( = anion,...Ch. 14 - The following is the titration curve for the...Ch. 14 - Prob. 64QAPCh. 14 - Follow the directions of Question 64. Consider two...Ch. 14 - Prob. 66QAPCh. 14 - Indicate whether each of the following statements...Ch. 14 - Prob. 68QAPCh. 14 - Consider the following titration curves. The...Ch. 14 - Consider the titration of HF (K a=6.7104) with...Ch. 14 - The species called glacial acetic acid is 98%...Ch. 14 - Four grams of a monoprotic weak acid are dissolved...Ch. 14 - Prob. 73QAPCh. 14 - Fifty cm3 of 1.000 M nitrous acid is titrated with...Ch. 14 - A diprotic acid, H2B(MM=126g/moL), is determined...Ch. 14 - Prob. 76QAPCh. 14 - Two students were asked to determine the Kb of an...Ch. 14 - How many grams of NaOH must be added to 1.00 L of...Ch. 14 - How many grams of NaF must be added to 70.00 mL of...Ch. 14 - Prob. 80QAP
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- Consider a weak organic base (nonelectrolyte) with molar mass 281 g/mol. An aqueous solution of the base has a pH of 8.73 and an osmotic pressure of SS mm Hg at 25C. What is Kb for the weak base?arrow_forwardA student is asked to bubble enough ammonia gas through water to make 4.00 L of an aqueous ammonia solution with a pH of 11.55. What volume of ammonia gas at 25C and 1.00 atm pressure is necessary?arrow_forwardLeucine is an amino acid with this Lewis structure: Write the Lewis structure for the zwitterion form of leucine.arrow_forward
- In general, are proteins acids, bases, or both (amphoteric)?arrow_forwardWhat is the Kw of pure water at 50.0 degrees Celsius, if the pH is 6.630?arrow_forwardAcetic acid (CH3COOH) and trifluoroacetic acid (CF3COOH) are shown by these particulate models. The Ka for trifluoroacetic acid is 104 times greater than acetic acid. Use the models to account for the differences in magnitude for the Ka constant. The yellow atoms are fluorine, the red atoms are oxygen, the black atoms are carbon, and the white atoms are hydrogen. Write the formulas for the conjugate bases for the two structures.The conjugate base of acetic acid The conjugate base of trifluoroacetic acidarrow_forward
- The pKw of seawater at 25°C is 13.776. This differs fromthe usual pKw of 14.00 at this temperature because dissolved salts make seawater a nonideal solution. If the pH in seawater is 8.00, what are the concentrations of H3O+ and OH- in seawater at 25°C?arrow_forwardAbbreviating malonic acid, CH2(CO2H)2, as H2M, find the pH and concentrations of H2M, HM, and M2 in each of the following solutions: (a) 0.100 M H2M; (b) 0.100 M NaHM; (c) 0.100 M Na2M. For (b), use the approximation 3HM24 < 0.100 M.arrow_forward1. The hydroxide ion concentration, [OH-], of an aqueous solution of 0.429 M methylamine (a weak base with the formula CH3NH2) , Kb = 4.2×10-4, is: [OH-] = _________ M 2. The pH of an aqueous solution of 0.429 M aniline (a weak base with the formula C6H5NH2) is _______ 3.The hydronium ion concentration of an aqueous solution of 0.429 M diethylamine (a weak base with the formula (C2H5)2NH) is [H3O+] = __________ M.arrow_forward
- A 0.785M solution of the weak acid, hypoiodous acid, HOI, has a Ka of 2.32x10-11. What is the equilibrium concentration of the conjugate base of HOI?arrow_forwardThe hydroxide ion concentration, [OH-], of an aqueous solution of 0.429 M methylamine (a weak base with the formula CH3NH2) is _____ M. The pH of an aqueous solution of 0.429 M aniline (a weak base with the formula C6H5NH2) is ________ . The hydronium ion concentration of an aqueous solution of 0.429 M diethylamine (a weak base with the formula (C2H5)2NH) is [H3O+] = ________ M.arrow_forwardWrite a net ionic equation to show why solid sodium hydroxide, NaOH (s), forms a basic solution when it dissolves in water. The substance morphine is a weak nitrogenous base like ammonia.Write a net ionic equation to show how morphine, C17H19O3N, behaves as a base in water.arrow_forward
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