A 2.50 g sample of KCl is dissolved in 34.0 mL of water. The resulting solution is then added to 59.0 mL of a 0.500 M CaCl2 (aq) solution. Assuming that the volumes are additive, calculate the concentrations of each ion present in final solution. Concentration of K+ ions = M Concentration of Ca+ jons = M Concentration of Cl ions = M
A 2.50 g sample of KCl is dissolved in 34.0 mL of water. The resulting solution is then added to 59.0 mL of a 0.500 M CaCl2 (aq) solution. Assuming that the volumes are additive, calculate the concentrations of each ion present in final solution. Concentration of K+ ions = M Concentration of Ca+ jons = M Concentration of Cl ions = M
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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![A 2.50 g sample of KCl is dissolved in 34.0 mL of water. The resulting solution is then added to 59.0 mL of a 0.500 M CaCl2 (aq) solution. Assuming that the
volumes are additive, calculate the concentrations of each ion present in
final solution.
Concentration of Kt ions =
M
Concentration of Ca?+ ions =
M
Concentration of Cl ions =
|M
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Transcribed Image Text:A 2.50 g sample of KCl is dissolved in 34.0 mL of water. The resulting solution is then added to 59.0 mL of a 0.500 M CaCl2 (aq) solution. Assuming that the
volumes are additive, calculate the concentrations of each ion present in
final solution.
Concentration of Kt ions =
M
Concentration of Ca?+ ions =
M
Concentration of Cl ions =
|M
Submit Answer
Try Another Version
5 item attempts remaining
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