186 Experiment 7 Solubility Product Constant of Copper (II) lodate 4. The slightly soluble salt AB2 ionizes as shown. (1) AB2 (s) = A2+ (aq) + 2B (aq) When a solution of CX is titrated into a saturated solution of AB2, the equivalence point is reached when B is completely consumed by the added C2+ ion. (2) C2+ (aq) + 2 В (ад) CB2 (aq) It takes 5.00 mL of 0.10 M CX solution to reach the equivalence point when titrated into a 20.0 mL saturated AB, solution. Refer to the Introduction and Data Sheet to solve the following problems: a) Refer to equation 1 above and write the K expression for AB2 in terms of the ion concentrations and in terms of the molar solubility, s. b) Calculate how many moles of C2+ were titrated to reach the equivalence point. c) Based on your result to part b, calculate the number of moles of B in the saturated AB2 solution. Consider the stoichiometry of equation 2. d) Based on your result to part c, calculate the number of moles of AB, in the saturated solution. Consider the stoichiometry of equation 1. e) Based on your result to part d, calculate the molar solubility, s, of AB,. f) Based on your result to part e, calculate the Ksp value for AB2.
186 Experiment 7 Solubility Product Constant of Copper (II) lodate 4. The slightly soluble salt AB2 ionizes as shown. (1) AB2 (s) = A2+ (aq) + 2B (aq) When a solution of CX is titrated into a saturated solution of AB2, the equivalence point is reached when B is completely consumed by the added C2+ ion. (2) C2+ (aq) + 2 В (ад) CB2 (aq) It takes 5.00 mL of 0.10 M CX solution to reach the equivalence point when titrated into a 20.0 mL saturated AB, solution. Refer to the Introduction and Data Sheet to solve the following problems: a) Refer to equation 1 above and write the K expression for AB2 in terms of the ion concentrations and in terms of the molar solubility, s. b) Calculate how many moles of C2+ were titrated to reach the equivalence point. c) Based on your result to part b, calculate the number of moles of B in the saturated AB2 solution. Consider the stoichiometry of equation 2. d) Based on your result to part c, calculate the number of moles of AB, in the saturated solution. Consider the stoichiometry of equation 1. e) Based on your result to part d, calculate the molar solubility, s, of AB,. f) Based on your result to part e, calculate the Ksp value for AB2.
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Transcribed Image Text:186
Experiment 7 Solubility Product Constant of Copper (II) lodate
4. The slightly soluble salt AB2 ionizes as shown.
(1)
AB2 (s)
= A2+ (aq) + 2B (aq)
When a solution of CX is titrated into a saturated solution of AB2, the equivalence point
is reached when B is completely consumed by the added C2+ ion.
(2)
C2+ (aq) +
2 В (ад)
CB2 (aq)
It takes 5.00 mL of 0.10 M CX solution to reach the equivalence point when titrated into
a 20.0 mL saturated AB, solution. Refer to the Introduction and Data Sheet to solve the
following problems:
a) Refer to equation 1 above and write the K expression for AB2 in terms of the ion
concentrations and in terms of the molar solubility, s.
b) Calculate how many moles of C2+ were titrated to reach the equivalence point.
c) Based on your result to part b, calculate the number of moles of B in the saturated
AB2 solution. Consider the stoichiometry of equation 2.
d) Based on your result to part c, calculate the number of moles of AB, in the saturated
solution. Consider the stoichiometry of equation 1.
e) Based on your result to part d, calculate the molar solubility, s, of AB,.
f) Based on your result to part e, calculate the Ksp value for AB2.
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