Look at sample problem 19.10 in the 8th ed Silberberg book. Write the Ksp expression. Find the concentrations of the ions you need (in this case Ca2 and F-). Put those concentrations into the Ksp expression to calculate Q. Compare Q to K A common laboratory method for preparing a precipitate is to mix solutions containing the component ions. Does a precipitate form when 10. ml of 0.0010 M Ca(NO3)2 is mixed with 10. ml of 0.00010 M NaF
Answers: 1
= 0.01 L × 0.0010 mol/L
= 0.01 L × 0.00010 mol/L
![[Ca^{2+}}] = \dfrac{1\times10^{-5} \ mol}{0.02 \ L} \\ \\ \\ \[[Ca^{2+}}] = 0.0005 \ mol/L](/tpl/images/1138/9149/5dc3a.png)
![[F^{-}] = \dfrac{(1\times 10^{-6} \ mol)}{0.02 \ L}](/tpl/images/1138/9149/ecdb2.png)
![[F^{-}] = 5 \times 10^{-5} \ mol/L](/tpl/images/1138/9149/20d72.png)
![Q = [Ca^{2+}][F^-]^2 \\ \\ Q = 0.0005 \times (5\times 10^{-5})^2 \\ \\ Q = 1.25 \times 10^{-12}](/tpl/images/1138/9149/52d7c.png)
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