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Effects of Adding Common Ion at Equilibrium

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Consider the equilibrium of AgCl(s) in water. What is the effect of adding KCl?
a. The KCl has no effect
b. The reaction goes to the right
c. The reaction goes to the left
d. Silver chloride solubility increases
e. Silver dichloride precipitates

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Solution Summary

Solution provides chemical formula and explanation based on Le Chatelier's Principle.

See Also This Related BrainMass Solution

Chromate-dichromate equilibrium.

See attached file for full problem description.

1. How does the (H+) of the solution affect the CrO42-/Cr2O72- eqiuilibrium?

2. What poof was shown that CrO42- ions exist in a solution of K2Cr2O7.

3. In what way does OH- affect the equilibrium? Give two methods by which this ion upsets the equilibrium?

4. Write the equations for the equilibrium, showing

a) the reaction between H+ and CrO42- to produce Cr2O72- and H2O

b) the reaction between OH- and Cr2O72- to produce CrO42- and H2O

c) a summation equation showing both H+ and OH - in the equilibrium reaction between CrO42- and Cr2O72- ions.

5. Explain fully what happens when H+ is added to a mixture containing BaCrO4(s) and CrO42-(aq).

6. In effect what was occurring in steps 7 and 8?

7. Explain the general effect of the acids and bases added in part III.

8. If all the bases have OH- (aq) in common, then explain why NH3(aq) acts like a base.

9. Explain why Ca(OH)2 has little effect on the equilibrium.

Is it because it is moderately soluble?

10. Why does C2H5OH not affect the equilibrium?

11. List the conclusions for this experiment, based on le Chatelier's principle.

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