Consider the following reaction at equilibrium: CaSO_4(s) <----->Ca2+(aq)+SO_42-

Question

Consider the following reaction at equilibrium:

CaSO_4(s) <----->Ca2+(aq)+SO_42-(aq) Keq= 9.1*10^6

If 60.0mL of 0.10 M Ca2+(aq) and 200.0 mL of 0.05 M SO_42-(aq) and 2.0 grams of CaSO_4(s) are mixed together, which direction does the reaction go?

(Show all calculations)

I know I have to calculate Qc which is products over reactants. I took 2.0 grams and multiply it by the molar mass to get my number of moles and then divide by the sum of the volume to get my concentration. After this, I realize I didnt have to to this because my reactant is a solid. Now, the professor told me I have to use M1V1=M2V2 but how?? and why?? I really dont see how can this equation can be apply to this problem.

Explanation / Answer

Related Questions

Navigate

• Browse (All)
• Browse C
• Subjects