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 15QAP
A solution with a pH of 9.22 is prepared by adding water to 0.413 mol of KX to make 2.00 L of solution. What is the pH of the solution after 0.368 mol of HX is added?
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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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- A buffer solution is prepared by adding 5.50 g of ammonium chloride and 0.0188 mol of ammonia to enough water to make 155 mL of solution. (a) What is the pH of the buffer? (b) If enough water is added to double the volume, what is the pH of the solution?arrow_forwardA buffer solution is prepared by adding 5.50 g of ammonium chloride and 0.0188 mol of ammonia to enough water to make 155 mL of solution. (a) What is the pH of the buffer? (b) If enough water is added to double the volume, what is the pH of the solution?arrow_forwardAn aqueous solution of 0.057 M weak acid, HX, has a pH of 4.65. What is the pH of the solution if 0.018 mol of KX is dissolved in one liter of the weak acid?arrow_forward
- Consider the titration of HF (K a=6.7104) with NaOH. What is the pH when a third of the acid has been neutralized?arrow_forwardA buffer is prepared by dissolving 0.0250 mol of sodium nitrite, NaNO2, in 250.0 mL of 0.0410 M nitrous acid, HNO2. Assume no volume change after HNO2 is dissolved. Calculate the pH of this buffer.arrow_forwardWhen 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.arrow_forward
- A monoprotic organic acid that has a molar mass of 176.1 g/mol is synthesized. Unfortunately, the acid produced is not completely pure. In addition, it is not soluble in water. A chemist weighs a 1.8451-g sample of the impure acid and adds it to 100.0 mL of 0.1050 M NaOH. The acid is soluble in the NaOH solution and reacts to consume most of the NaOH. The amount of excess NaOH is determined by titration: It takes 3.28 mL of 0.0970 M HCl to neutralize the excess NaOH. What is the purity of the original acid, in percent?arrow_forwardA buffer solution is composed of 1.360 g of KH2PO4 and 5.677 g of Na2HPO4. (a) What is the pH of the buffer solution? (b) What mass of KH2PO4 must be added to decrease the buffer solution pH by 0.50 unit from the value calculated in part (a)?arrow_forwardA buffer is prepared by dissolving 0.062 mol of sodium fluoride in 127 mL of 0.0399 M hydrofluoric acid. Assume no volume change after NaF is added. Calculate the pH of this buffer.arrow_forward
- A 0.400-g sample of propionic acid was dissolved in water to give 50.0 mL of solution. This solution was titrated with 0.150 M NaOH. What was the pH of the solution when the equivalence point was reached?arrow_forwardA buffer solution is prepared from 5.15 g NH4NO3 and 0.10 L of 0.15-M NH3; calculate the pH of the solution.arrow_forwardA 1.0-L solution that is 4.2 M in ammonia is mixed with 26.7 g of ammonium chloride. a What is the hydroxide-ion concentration of this solution? b 0.075 mol of MgCl2 is added to the above solution. Assume that there is no volume change. After Mg(OH)2 has precipitated, what is the molar concentration of magnesium ion? What percent of the Mg2+ is removed from solution?arrow_forward
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