186 Experiment 7 Solubility Product Constant of Copper (II) lodate 4. The slightly soluble salt AB, 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 B (aq) • 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 Km 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 result to part c, calculate the number of moles of AB, in the saturated solution. Consider the stoichiometry of equation 1. your 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 K value for AB.
186 Experiment 7 Solubility Product Constant of Copper (II) lodate 4. The slightly soluble salt AB, 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 B (aq) • 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 Km 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 result to part c, calculate the number of moles of AB, in the saturated solution. Consider the stoichiometry of equation 1. your 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 K value for AB.
Chemistry by OpenStax (2015-05-04)
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Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter15: Equilibria Of Other Reaction Classes
Section: Chapter Questions
Problem 16E: Assuming that no equilibria other than dissolution are involved, calculate the concentration of all...
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Transcribed Image Text:186
Experiment 7 Solubility Product Constant of Copper (II) lodate
4. The slightly soluble salt AB, 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 B (aq)
• 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 Km 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 result to part c, calculate the number of moles of AB, in the saturated
solution. Consider the stoichiometry of equation 1.
your
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 K value for AB.
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