Consider the following aqueous equilibria that take place simultaneously in the same container.
Ca2+(aq) + C2O42-(aq) <---> CaC2O4(s)
and
H+(aq) + C2O42-(aq) <---> HC2O4-(aq)
Indicate if the amount of CaC2O4(s) increases, decreases, or stays the same as a result of the following disturbances.
Explain each prediction. Assume any volume changes are negligible. Consider the solubility rules.
a) Add LiOH(aq)
b) Add HNO3(aq)
c) add Ca(NO3)2(aq)
d) Increase the volume of the container
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Here are my answers:
a) Increase. Because the hydroxides will bond with the H+ to form water, and the 2nd rxn will shift to the left in order to rebalance the loss of H+. Then, the excess C2O4- will shift the 1st rxn to the right to form more Ca(C2O4) (s).
b) Decrease. The HNO3 will cause an increase in H+, so the 2nd rxn will shift to the right (forward) and the decrease in C2O4 2- will cause the 1st rxn to shift to the left in order to return to equilibrium.
c) Increase. The additional Ca will shift the 1st rxn to the right.
d) No change (stays the same). Increase in volume of container does not affect concentration.
I'm relatively confident about c and d. But my (a) and (b) seem a bit out there...help please!