Consider the equilibrium shown. SrF, (s) = Sr² +(aq) + 2 F¯(aq) Ksp = 2.60 × 10-9 Determine the concentrations of Sr² + and F¯ in a saturated solution of SrF, in pure water (assume u = 0 M). -3 [Sr? +] = 8.66239 x10¬4 [F¯] = 1.73246 ×10' M M Determine the concentrations of Sr² + and F¯ in a saturated solution of SrF, in a solution with an ionic strength of 0.010 M.
Consider the equilibrium shown. SrF, (s) = Sr² +(aq) + 2 F¯(aq) Ksp = 2.60 × 10-9 Determine the concentrations of Sr² + and F¯ in a saturated solution of SrF, in pure water (assume u = 0 M). -3 [Sr? +] = 8.66239 x10¬4 [F¯] = 1.73246 ×10' M M Determine the concentrations of Sr² + and F¯ in a saturated solution of SrF, in a solution with an ionic strength of 0.010 M.
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter15: Complex Ion And Precipitation Equilibria
Section: Chapter Questions
Problem 38QAP: To a beaker with 500 mL of water are added 95 mg of Ba(NO3)2, 95 mg of Ca(NO3)2, and 100.0 mg of...
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![Consider the equilibrium shown.
SrF, (s) = Sr²+(aq) + 2 F¯(aq)
Ksp
= 2.60 x 10-9
Determine the concentrations of Sr² + and F¯ in a saturated solution of SrF, in pure water (assume µ = 0 M).
-4
-3
[Sr? +] = 8.66239 ×10°
M
[F] =
1.73246 x10
M
%3|
Determine the concentrations of Sr?+ and F- in a saturated solution of SrF, in a solution with an ionic strength of
0.010 M.
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Transcribed Image Text:Consider the equilibrium shown.
SrF, (s) = Sr²+(aq) + 2 F¯(aq)
Ksp
= 2.60 x 10-9
Determine the concentrations of Sr² + and F¯ in a saturated solution of SrF, in pure water (assume µ = 0 M).
-4
-3
[Sr? +] = 8.66239 ×10°
M
[F] =
1.73246 x10
M
%3|
Determine the concentrations of Sr?+ and F- in a saturated solution of SrF, in a solution with an ionic strength of
0.010 M.
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