which one of the following solutions will contain the greatest strontium ion concentration: strontium carbonate solution (Ksp=5.6*106-10) or strontium fluoride solution (Ksp= 4.3*106-9)

Write down the equations:

SrCO_3 _{(s)} \rightarrow Sr^{2+}\ _{(aq)} + CO_3 \ ^{2-}\ _{(aq)}

SrF_2\ _{(s)} \rightarrow Sr^{2+}\ _{(aq)} +2F \ ^- \ _{(aq)}

Write down the formula for each reaction and equate it to the corresponding Ksp value.

Post what you did! :)

SrCO3(s) goes to equilibrium then Sr+2+ CO3-2
Ksp= conc of Sr+2 multiply by conc of CO3-25.6 *10^-5=X^2 then that equals to 2.5*10^-5=x

then For the second equation you do the same thing except different values of Ksp

Ksp=conc of Sr+2 multiplied by F-2 ^2
then, 4.3*10^-3=4X^3
equals to 1.0*10^-3=X

so the final answer is SrF2 has more concentration Sr+2 concentrations.

Well, while your final answer is good, I can't see where you got the numbers:
25.6*10^-5

I got \sqrt{5.6\times10^{-10}} = 2.4 \times 10^{-5}

Check your calculation well.

I made a mistake sorry, its suppose to be CO3-2 5.6 *10^-5=X^2 I forgot to be put space between Co3-2 so the final answer is 2.5*10 ^-5.

Oh, now I see it. The numbers just got messed up.

It's good, you got the correct answer :)