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Hi. I'm not sure if my strategy for this problem is correct:

How many grams of CaCO3 will dissolve in 3.0x10^-2 mL of 0.050M Ca(NO3)2?

I think I'm supposed to convert molarity of Ca(NO3)2 into moles, but then i don't know how to get from mols of that to mols of it a 1 to 1 ratio? from then on do i just convert to grams?


  • chemistry -

    This is a solubility product problem with CaCO3 in which there is a common ion (the Ca in Ca(NO3)2)
    CaCO3 ==> Ca^+2 + CO3^=

    Ksp = (Ca^+2)(CO3^=) = ??
    Look up the Ksp for CaCO3.

    Ca(NO3)2 ==> Ca^+2 + 2NO3^- (100% ionized)
    [Ca(NO3)2] = 0.05 M
    Let y = solubility of CaCO3, then y = concn of Ca^+2 from CaCO3 and y is concn of CO3^=. Total (Ca^+2) = y+0.05 (that's Ca from CaCO3 and Ca from Ca(NO3)2).
    Solve for y, the units will be mols/L CaCO3, then convert from mols/L to mols/3.0 x 10^-2 mL, and from there to grams.
    0.05 M = (Ca^+2) from Ca(NO3)2

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