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 47QAP
A 0.4000 M solution of nitric acid is used to titrate 50.00 mL of 0.237 M barium hydroxide. (Assume that volumes are additive.)
(a) Write a balanced net ionic equation for the reaction that takes place during titration.
(b) What are the species present at the equivalence point?
(c) What volume of nitric acid is required to reach the equivalence point?
(d) What is the pH of the solution before any HNO3 is added?
(e) What is the pH of the solution halfway to the equivalence point?
(f) What is the pH of the solution at the equivalence point?
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3) 2.0 g of NaOH is dissolved in distilled water to prepare 100 mL solution. 20.0 mL of this solution
reaches to the equivalence point when 25 mL of an acid solution containing 1.22 g unknown
monoprotic weak acid is added.
(a) Calculate the molar mass of the unknown acid.
(b) After 15.0 mL of NaOH solution had been added during the titration, the pH was determined
to be 4.7. What is the Ka of the unknown acid?
(NaOH
= 40.0 g/mol)
(4) A solution is made of a mixture of 0.500 M Calcium chloride and 0.0100 M iron (II) nitrate.
The two metals are to be separated by precipitation by increasing the pH.
(a) At what pH will the first metal begin to precipitate?
(b) At what pH will 99.9% of the first metal be precipitated?
(c) At what pH will the second metal begin to precipitate?
(d) Can the metals be separated successfully?
Consider the titration of 36.0 mL of 0.117 M ammonia with 0.0752 M HCl. (See the Acid-Base Table.)
(a) How many mL of HCl are required to reach the equivalence point?5.60 mL(b) What is the pH at the equivalence point? 5.30(c) What is the pH of the solution after the addition of 15.7 mL of acid? (d) What is the pH of the solution after the addition of 82.9 mL of acid?
only need part c and d please
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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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
- 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_forwardWrite the net ionic equation in which the slightly soluble salt barium fluoride, BaF2, dissolves in dilute hydrochloric acid.arrow_forwardA 5.145 g sample of a solid, weak, monoprotic acid is used to make a 100.0 mL solution. 27.00 mL of the resulting acid solution is then titrated with 0.09636 M NaOH. The pH after the addition of 16.00 mL of the base is 5.75, and the endpoint is reached after the addition of 45.85 mL of the base. (a) How many moles of acid were present in the 27.00 mL sample?4.42e-3 mol(b) What is the molar mass of the acid?314 g/mol(c) What is the pKa of the acid? (only confused on part c, answers for a and b are given)arrow_forward
- A buffer is prepared by adding 5.0 g of ammonia, NH3, and 20.0 g of ammonium chloride, NH4Cl, to enough water to form 2.50 L of solution. (a) What is the pH of the buffer? (b) Write the complete ionic equation for the reaction that occurs when a few drops of nitric acid are added to the buffer. (c) Write the complete ionic equation for the reaction that occurs when a few drops of potassium hydroxide solution are added to the buffer.arrow_forwardA 5.296 g sample of a solid, weak, monoprotic acid is used to make a 100.0 mL solution. 30.00 mL of the resulting acid solution is then titrated with 0.09755 M NaOH. The pH after the addition of 21.00 mL of the base is 5.02, and the endpoint is reached after the addition of 46.38 mL of the base. (a) How many moles of acid were present in the 30.00 mL sample? 0.004524 mol(b) What is the molar mass of the acid?351.1 g/mol(c) What is the pKa of the acid? just need help with part Carrow_forward1. 50.00ml of 2.000M ammonium nitrate is titrated with 0.800M NaOH. (a) What is the pH at the equivalence point? (b) What is the pH of the solution at the initial point? (c) What is the volume of NaOH required to react with all of the acid? (d) What is the pH of the solution after the addition of 175.00ml of the base? (e) What is the pH of the solution halfway to the equivalence point?arrow_forward
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