PRINCIPLES+REACTIONS
8th Edition
ISBN: 9781337759632
Author: Masterton
Publisher: CENGAGE L
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Chapter 14, Problem 38QAP
Given the acid-base indicators in Question 37, select a suitable indicator for the following titrations.
(a) sodium formate (NaCHO2) with HNO3
(b) hypochlorous acid with barium hydroxide
(c) nitric acid with HI
(d) hydrochloric acid with ammonia
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A buffer is prepared by adding 20.0 g of sodium acetate(CH3COONa) to 500 mL of a 0.150 M acetic acid(CH3COOH) solution. (a) Determine the pH of the buffer.(b) Write the complete ionic equation for the reaction thatoccurs when a few drops of hydrochloric acid are added tothe buffer. (c) Write the complete ionic equation for the reactionthat occurs when a few drops of sodium hydroxidesolution are added to the buffer.
An acid–base titration is performed: 250.0 mL of an unknownconcentration of HCl (aq) is titrated to the equivalence pointwith 36.7 mL of a 0.1000 M aqueous solution of NaOH. Whichof the following statements is not true of this titration?
(a) The HCl solution is less concentrated than the NaOH solution.(b) The pH is less than 7 after adding 25 mL of NaOHsolution. (c) The pH at the equivalence point is 7.00. (d) If anadditional 1.00 mL of NaOH solution is added beyond theequivalence point, the pH of the solution is more than 7.00.(e) At the equivalence point, the OH- concentration in thesolution is 3.67 x 10-3 M.
Calculate the pH change that results when 12 mL of 5.3 M NaOH is added to 768 mL of each the following solutions. (See the Acid-Base Table attached.)
(a) pure water (b) 0.10 M NH4Cl (c) 0.10 M NH3(d) a solution that is 0.10 M in each NH4+ and NH3
Chapter 14 Solutions
PRINCIPLES+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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Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- When might a pH meter be better than an indicator to determine the end point of an acid-base titration?arrow_forwardUsing the diagrams shown in Problem 10-117, which of the solutions would have the greatest buffer capacity, that is, greatest protection against pH change, when the following occurs? a. A strong acid is added to the solution. b. A strong base is added to the solution.arrow_forwardEqual molar quantities of ammonia and sodium dihydrogen phosphate (NaH2PO4) are mixed. (a) Write a balanced, net ionic equation for the acid-base reaction that can, in principle, occur. (b) Does the equilibrium lie to the right or left?arrow_forward
- Calculate the pH change that results when 11 mL of 5.1 M NaOH is added to 796 mL of each the following solutions. (See the Acid-Base Table.) (a) pure water (b) 0.10 M NH4Cl (c) 0.10 M NH3 (d) a solution that is 0.10 M in each NH4+ and NH3arrow_forwardCalculate the pH change that results when 15 mL of 2.7 M HCI is added to 600. mL of each of the following solutions. Use the Acid-Base Table. (a) pure water 4.0 -5.82 (b) 0.10 M CH3COO- 4.0 4.43 (c) 0.10 M CH3COOH 4.0 X (d) a solution that is 0.10 M in each CH3COO and CH3COOH. 4.0arrow_forwardConsider the titration of formic acid, HCHO2, with barium hydroxide. (a) Write a balanced net ionic equation for the reaction. (b) Calculate K for the reaction. (c) Is the solution at the equivalence point acidic, basic, or neutral? (d) What would be an appropriate indicator for the titration?arrow_forward
- (a) Calculate the pH in a solution prepared by dissolving 0.050 mol of acetic acid and 0.020 mol of sodium acetate in water and adjusting the volume to 500 mL.(b) Suppose 0.010 mol of NaOH is added to the buffer from part (a).Calculate the pH of the solution that results.arrow_forwardCalculate the pH at the following points in a titration of 40.0 mL of 0.100 M barbituric acid(Ka = 9.8 × 10−5) with 0.100 M KOH. (a) no KOH added (b) 20.0 mL of KOH solution added (c)39.0 mL of KOH solution added (d) 40.0 mL of KOH solution added (e) 41.0 mL of KOHSketch an appropriate pH titration curve indicating the buffer region, equivalence point,and excess base region. Why is the pH at the equivalence point not 7.00?arrow_forwardA 0.1724-g sample of an unknown monoprotic acid was dissolved in 26.9 mL of water and titrated with 0.0623 M NaOH solution. The volume of base required to bring the solution to the equivalence point was 19.8 mL. (a) Calculate the molar mass of the acid. (b) After 11.5 mL of base had been added during the titration, the pH was determined to be 5.66. What is the Ka of the unknown acid?arrow_forward
- Calculate the pH change that results when 15 mL of 2.0 M HCI is added to 580. mL of each of the following solutions (a) pure water 4.0-5.70 (b) 0.10 M CH3COO 4.04.28 (c) 0.10 M CH3COOH 4.0 (d) a solution that is 0.10 M in each CH3COO and CH3COOH. 4.0arrow_forwardNitesharrow_forward13. A 60.00 mL sample of 0.075 M sodium benzoate (NaC7H5O2) was titrated with 0.050 M HCl. What is the pH of the solutionafter 10.00 ml of HCl is added?(a) 4.19(b) 5.09(c) 5.74(d) 6.2414. What is the ratio of moles of benzoate (C7H5O2‒) to benzoic acid (HC7H5O2) in the solution that results from thecombination of the NaC7H5O2 and HCl in the problem above?(a) 8(b) 0.125(c) 0.0040(d) 0.00050arrow_forward
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Acid-Base Titration | Acids, Bases & Alkalis | Chemistry | FuseSchool; Author: FuseSchool - Global Education;https://www.youtube.com/watch?v=yFqx6_Y6c2M;License: Standard YouTube License, CC-BY