b. Write out the equilibrium expressions for each reaction in a.and CN- (aq) ions in a 0.050 M KCN solution.Write out the reactions that need to be considered.2. Given that the solubility product of AgCN (s) is a ax10 16, calculate the concentration of Ag* (aq)а.c. Calculate the ionic strength of this systemd. Calculate the activity coefficients for each species in the equilibrium expressions b.where aAg+= 250 and aCN- = 300 pm.Write the charge balance equatione.f. Write the mass balance equation (s)g. Setup Excel spreadsheet to solve this problem

Given that the solubility product of AgCN (s) is 2.2x10-1º, calculate the concentration of Ag* (aq) and CN- (aq) ions in a 0.050 M KCN solution. b. Write out the equilibrium expressions for each reaction in a. Write out the reactions that need to be considered. a.

Given that the solubility product of AgCN (s) is 2.2x10-1º, calculate the concentration of Ag* (aq) and CN- (aq) ions in a 0.050 M KCN solution. b. Write out the equilibrium expressions for each reaction in a. Write out the reactions that need to be considered. a.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

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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Question

b. Write out the equilibrium expressions for each reaction in a.
and CN- (aq) ions in a 0.050 M KCN solution.
Write out the reactions that need to be considered.
2. Given that the solubility product of AgCN (s) is a ax10 16, calculate the concentration of Ag* (aq)
а.
c. Calculate the ionic strength of this system
d. Calculate the activity coefficients for each species in the equilibrium expressions b.
where aAg+
= 250 and aCN- = 300 pm.
Write the charge balance equation
e.
f. Write the mass balance equation (s)
g. Setup Excel spreadsheet to solve this problem

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