
Chemistry: Principles and Reactions
8th Edition
ISBN: 9781305079373
Author: William L. Masterton, Cecile N. Hurley
Publisher: Cengage Learning
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Calculate the pOH of a solution that is 0.165 M morphine C17H19O3N and 0.386 M morphine hydrochloride C17H20O3NCl. Kb of C17H19O3N is 1.6 x 10^-6
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Estimate the pH that results when the following two solutions are mixed. a) 50 mL of 0.3 M CH3COOH and 50 mL of 0.4 M KOH b) 100 mL of 0.3 M CH3COOH and 50 mL of 0.4 M NaOH c) 150 mL of 0.3 M CH3COOH and 100 mL of 0.3 M Ba(OH)2 d) 200 mL of 0.3 M CH3COOH and 100 mL of 0.3 M Ba(OH)2
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What is the freezing point of 0.92 M aqueous acetic acid? The density of this solution is 1.008 g/cm3.
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Calculate the pH of each of the following solutions. (a) 10.0 mL of 0.300 M hydrofluoric acid plus 30.0 mL of 0.100 M sodium hydroxide (b) 100.0 mL of 0.250 M ammonia plus 50.0 mL of 0.100 M hydrochloric acid (c) 25.0 mL of 0.200 M sulfuric acid plus 50.0 mL of 0.400 M sodium hydroxide
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Using 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.
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Which of the diagrams in Problem 10-135 represents the substance that is the weakest electrolyte?
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Classify each of the following acids as monoprotic, diprotic, or triprotic. a. HClO3 (chloric acid) b. HC3H5O4 (glyceric acid) c. H3C6H5O7 (citric acid) d. H3PO4 (phosphoric acid)
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Consider the following six beakers. All have 100 mL of aqueous 0.1 M solutions of the following compounds: beaker A has HI beaker B has HNO2 beaker C has NaOH beaker D has Ba(OH)2 beaker E has NH4Cl beaker F has C2H5NH2 Answer the questions below, using LT (for is less than), GT (for is greater than), EQ (for is equal to), or MI (for more Information required). (a) The pH in beaker A the pH in beaker B. (b) The pH in beaker C the pH in beaker D. (c) The % ionization in beaker A the % ionization in beaker C. (d) The pH in beaker B the pH in beaker E. (e) The pH in beaker E the pH in beaker F. (f) The pH in beaker C the pH in beaker F.
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What is the freezing point of vinegar, which is an aqueous solution of 5.00% acetic acid, HC2H3O2, by mass (d=1.006g/cm3)?
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Classify each of the following acids as monoprotic, diprotic, or triprotic. a. H2SO4 (sulfuric acid) b. HC2H3O2 (acetic acid) c. H2C5H6O4 (glutaric acid) d. HCN (cyanic acid)
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Calculate [H+] and pH in a solution in which lactic acid, HC3H5O3, is 0.250 M and the lactate ion, C3H5O3-, is (a) 0.250 M (b) 0.125 M (c) 0.0800 M (d) 0.0500 M
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Classify each of the following compounds as a strong electrolyte or a weak electrolyte. a. H3PO4 b. HNO3 c. KNO3 d. NaOH
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Write chemical equations showing the individual proton-transfer steps that occur in aqueous solution for each of the following acids. a. H2C2O4 (oxalic acid) b. H2C4H4O6 (tartaric acid)
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