# Chemistry

posted by Caroline

1. Imagine you have a saturated solution of Ca(OH)2, at equilibrium, that has some undissolved
Ca(OH)2 precipitated on the bottom of the test tube. If you add an additional scoop of Ca(OH)2 to
the solution will concentration of [OH-] in the solution (increase, decrease, or be unchanged)?
Explain. Assume you let the solution reach equilibrium again.

Unchanged because the solution is already in equilibrium of ions.

2. Imagine you have a saturated solution of Ca(OH)2, at equilibrium, that has some undissolved
Ca(OH)2 precipitated on the bottom of the test tube. If you add pure water to the test tube will
the amount of solid Ca(OH)2 at the bottom (increase, decrease, or be unchanged)? Explain.
Assume you let the solution reach equilibrium again.

Shift to the right because the increased volume of solution with reduce the concentration of the products so the reactant solid with decrease and the product ions will increase until it reaches equilibrium.

3. Imagine you have a saturated solution of Ca(OH)2, at equilibrium, that has some undissolved
Ca(OH)2 precipitated on the bottom of the test tube. If you add pure water will the concentration
of [OH-] in the solution (increase, decrease, or be unchanged)? Explain. Assume you let the
solution reach equilibrium again and the solution remains saturated.

Unchanged because while the mass of [OH-] ions will increase the concentration in the solution will be the same because that is the equilibrium.

So I answered these they way I thought was correct but I wanted to make sure. I have trouble understanding number 2 in particular.

1. DrBob222

I thought you did a super job.

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