CHEMISTRY:PRIN.+REACTIONS-OWLV2 ACCESS
8th Edition
ISBN: 9781305079298
Author: Masterton
Publisher: Cengage Learning
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Chapter 15, Problem 14QAP
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?
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a) What is the pH of a buffer solution that is made by dissolving 125.5 g of sodium benzoate and 166.9g of benzoic acid in 500 mL of water?
(b) What is the pH if you added 26.7 mL of 2.22 M NaOH to 254 mL of the buffer solution from above?
(c) What is the pH if you added 32.8 mL of 3.36 M HCl to 354 mL of the buffer solution from above?
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A 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.
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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.
Chapter 15 Solutions
CHEMISTRY:PRIN.+REACTIONS-OWLV2 ACCESS
Ch. 15 - Write a net ionic equation for the reaction...Ch. 15 - Write a net ionic equation for the reaction...Ch. 15 - Write a balanced net ionic equation for the...Ch. 15 - Write a balanced net ionic equation for the...Ch. 15 - Calculate K for the reactions in Question 1.Ch. 15 - Calculate K for the reactions in Question 2.Ch. 15 - Calculate K for the reactions in Question 3.Ch. 15 - Calculate K for the reactions in Question 4.Ch. 15 - Calculate [H+] and pH in a solution in which...Ch. 15 - Calculate [OH-] and pH in a solution in which the...
Ch. 15 - A buffer is prepared by dissolving 0.0250 mol of...Ch. 15 - Prob. 12QAPCh. 15 - A buffer solution is prepared by adding 15.00 g of...Ch. 15 - A buffer solution is prepared by adding 5.50 g of...Ch. 15 - A solution with a pH of 9.22 is prepared by adding...Ch. 15 - An aqueous solution of 0.057 M weak acid, HX, has...Ch. 15 - Which of the following would form a buffer if...Ch. 15 - Which of the following would form a buffer if...Ch. 15 - Calculate the solubility (in grams per liter) of...Ch. 15 - Calculate the solubility (in grams per liter) of...Ch. 15 - Copper(l) chloride, CuCl, is the starting material...Ch. 15 - Prob. 22QAPCh. 15 - Prob. 23QAPCh. 15 - Ksp for CaSO4 at 100C is estimated to be1.6105. At...Ch. 15 - Prob. 25QAPCh. 15 - At 25C, 10.24 mg of Cr(OH)2 are dissolved in...Ch. 15 - Calcium nitrate is added to a sodium sulfate...Ch. 15 - Cadmium(ll) chloride is added to a solution of...Ch. 15 - Water from a well is found to contain 3.0 mg of...Ch. 15 - Silver(I) sulfate (Ksp=1.2105) is used in the...Ch. 15 - A solution is prepared by mixing 13.00 mL of...Ch. 15 - A solution is prepared by mixing 45.00 mL of 0.022...Ch. 15 - A solution is 0.047 M in both NaF and Na2CO3....Ch. 15 - Solid lead nitrate is added to a solution that is...Ch. 15 - A solution is made up by adding 0.632 g of barium...Ch. 15 - A solution is made up by adding 0.839 g of...Ch. 15 - Prob. 37QAPCh. 15 - To a beaker with 500 mL of water are added 95 mg...Ch. 15 - Write net ionic equations for the reaction of H+...Ch. 15 - Prob. 40QAPCh. 15 - Prob. 41QAPCh. 15 - Write a net ionic equation for the reaction with...Ch. 15 - Prob. 43QAPCh. 15 - Write a net ionic equation for the reaction with...Ch. 15 - Prob. 45QAPCh. 15 - Write an overall net ionic equation and calculate...Ch. 15 - Consider the reaction...Ch. 15 - Consider the reaction BaF2(s)+SO42(aq)BaSO4(s)+2...Ch. 15 - Aluminum hydroxide reacts with an excess of...Ch. 15 - Prob. 50QAPCh. 15 - Calculate the molar solubility of gold(I) chloride...Ch. 15 - Calculate the molar solubility of PbCl2 in 0.2 M...Ch. 15 - For the reaction...Ch. 15 - For the reaction Zn(OH)2(s)+2OH(aq)Zn(OH)42(aq)...Ch. 15 - What are the concentrations of Cu2+, NH3, and...Ch. 15 - Prob. 56QAPCh. 15 - Calcium ions in blood trigger clotting. To prevent...Ch. 15 - Prob. 58QAPCh. 15 - A town adds 2.0 ppm of F- ion to fluoridate its...Ch. 15 - Consider the following hypothetical dissociation:...Ch. 15 - Prob. 61QAPCh. 15 - Consider a 2.0-L aqueous solution of 4.17 M NH3,...Ch. 15 - Marble is almost pure CaCO3. Acid rain has a...Ch. 15 - Prob. 64QAPCh. 15 - Prob. 65QAPCh. 15 - The box below represents one liter of a saturated...Ch. 15 - Consider a saturated solution of BaCO3 at 7.5C....Ch. 15 - Prob. 68QAPCh. 15 - Consider the insoluble salts JQ, K2R, L2S3, MT2,...Ch. 15 - Prob. 70QAPCh. 15 - Consider the equilibrium curve for AgCl shown...Ch. 15 - Dissolving CaCO3 is an endothermic reaction. The...Ch. 15 - Challenge Problems Insoluble hydroxides such as...Ch. 15 - What is the solubility of CaF2 in a buffer...Ch. 15 - What is [Br-] just as AgCl begins to precipitate...Ch. 15 - Prob. 76QAPCh. 15 - Prob. 77QAPCh. 15 - Prob. 78QAP
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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_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_forwardThe weak base, CIO (hypochlorite ion), is used in the form of NaCIO as a disinfectant in swimming pools and water treatment plants. What are the concentrations of HCIO and OH and the pH of a 0.015 M solution of NaCIO?arrow_forward
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- Calculate the pH change that results when 11 mL of 5.1 M NaOH is added to 790. mL of each the following solutions. Use the Acid-Base Table. (a) pure water 4.0 5.84 (b) 0.10 M NH4CI 4.0 5.43 (c) 0.10 M NH3 4.0✔ X (d) a solution that is 0.10 M in each NH4+ and NH3 4.0✔arrow_forwardA buffer solution is prepared from equal volumes of 0.200 M acetic acid and 0.600 M sodium acetate. Use 1.80 × 10−5 as Ka for acetic acid.(a) What is the pH of the solution?(b) Is the solution acidic or basic?(c) What is the pH of a solution that results when 3.00 mL of 0.034 M HCl is added to 0.200 L of the original buffer?arrow_forwardNitesharrow_forward
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