Equilibrium Question: CuSO4 * 5 H2O, Temp, & Concentration

• elasticities

Homework Statement

Crystals of CuSO4 * 5 H2O are blue. If you place a few small crystals in a beaker of water, water molecules break apart the ions and they enter into the solution. A few ions in the solution may re-attach to the crystals. Because more ions enter the solution than reattach to the crystals, however, all the solid eventually dissolves. If you keep adding crystals of copper (II) sulfate pentahydrate, the solution eventually becomes saturated. Crystals remain at the bottom of the beaker.

a) There are two closed containers one with a darker blue liquid, one with lighter blue liquid. Which system is at equilibrium?

b) Will changing the temp affect the concentration of the solution at equilibrium system?

Homework Equations

None that I can think of.

The Attempt at a Solution

a) I think the lighter blue one without the precipitate at the bottom is the one that's at equilibrium because the solution isn't saturated and some of the ions are reforming into crystals, and some crystals are becoming ions.

b) Yes, because the equilibrium constant is dependent on temperature.

Here's another similar question.

Homework Statement

A supersaturated solution of sodium acetate was prepared by adding sodium acetate to a saturated solution and heated to dissolve added crystals. Finally the solution was left to return slowly to room temperature. A single crystal of sodium acetate was added to the supersaturated solution. Solute ions rapidly left the solution, and solid formed.

Which is at equilibrium:
a) Supersaturated solution of sodium acetate.
b) Supersaturated solution of sodium acetate with a crystal added to it.
c) Neither.

Homework Equations

None that I can think of.

The Attempt at a Solution

Supersaturated solution of sodium acetate? No crystals present, so it's at eq?