Calculate the molar solubility of SrF2 in: (a) 0.010 M Sr(NO3)2 (b) 0.010 M NaF.

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1. Step 1: Write the dissolution equation for SrF2: SrF2(s) ⇌ Sr²⁺(aq) + 2F⁻(aq).
2. Step 2: Write the expression for the solubility product constant (Ksp) of SrF2: Ksp = [Sr²⁺][F⁻]².
3. Step 3: For part (a), consider the common ion effect from Sr(NO3)2. The concentration of Sr²⁺ from Sr(NO3)2 is 0.010 M. Let the molar solubility of SrF2 be 's'. The total [Sr²⁺] = 0.010 + s and [F⁻] = 2s.
4. Step 4: Substitute the concentrations into the Ksp expression for part (a): Ksp = (0.010 + s)(2s)². Since s is small compared to 0.010, approximate [Sr²⁺] ≈ 0.010.
5. Step 5: For part (b), consider the common ion effect from NaF. The concentration of F⁻ from NaF is 0.010 M. Let the molar solubility of SrF2 be 's'. The total [F⁻] = 0.010 + 2s and [Sr²⁺] = s. Substitute these into the Ksp expression: Ksp = s(0.010 + 2s)². Since s is small compared to 0.010, approximate [F⁻] ≈ 0.010.