Will a precipitate form when 50.0 mL of 2.0 x 10-2 M NaF is mixed with 10.0 mL of 1.0 × 10-2 M Ca(NO3)2? Ksp = 3.9 ×10-11

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Chapter1: Chemical Foundations
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Can you explain this problem in detail? And where does the 2+ From Ca came from and how do you find it.

Will a precipitate form when 50.0 mL of 2.0 x 10-2 M NaF is mixed with 10.0 mL of
1.0 × 10 2 M Ca(NO3)2? Ksp = 3.9 ×10-11
Solution
We must get the Molarities of the principal ions that will lead to the precipitation.
Neither Na+ nor NO3 will precipitate, so we're left with Ca2+ and F as the ions that will form
the precipitate.
moles Ca2+ = 0.010 L x 0.010 M = 1.0 × 10-4 moles Ca2+
moles F= 0.050 L x 0.020 M = 1.0 x 10-3 moles F-
total volume = 50.0 mL + 10.0 mL = 60.0 mL
1.0 × 10-4 mol
[Ca2+] =
1.0 x 10-3 mol
= 1.67 x 103 M
[F] =
= 1.67 x 10-2
0.060 L
0.060 L
CaF2 (s) -
Ca2+ (aq)
+
2F- (aq)
4.6 x 10-7
Qsp = [Ca2+] [F]² = (1.67 x 10-3) (1.67 x 10-2)²
Thus: Qsp > Ksp, and a precipitate WILL form!!
Transcribed Image Text:Will a precipitate form when 50.0 mL of 2.0 x 10-2 M NaF is mixed with 10.0 mL of 1.0 × 10 2 M Ca(NO3)2? Ksp = 3.9 ×10-11 Solution We must get the Molarities of the principal ions that will lead to the precipitation. Neither Na+ nor NO3 will precipitate, so we're left with Ca2+ and F as the ions that will form the precipitate. moles Ca2+ = 0.010 L x 0.010 M = 1.0 × 10-4 moles Ca2+ moles F= 0.050 L x 0.020 M = 1.0 x 10-3 moles F- total volume = 50.0 mL + 10.0 mL = 60.0 mL 1.0 × 10-4 mol [Ca2+] = 1.0 x 10-3 mol = 1.67 x 103 M [F] = = 1.67 x 10-2 0.060 L 0.060 L CaF2 (s) - Ca2+ (aq) + 2F- (aq) 4.6 x 10-7 Qsp = [Ca2+] [F]² = (1.67 x 10-3) (1.67 x 10-2)² Thus: Qsp > Ksp, and a precipitate WILL form!!
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