Question
The $K_{\text {sp }}$ value for radium sulfate, $\mathrm{RaSO}_4$, is $4.2 \times 10^{-11}$. If $25 \mathrm{mg}$ of radium sulfate is placed in $1.00 \times 10^2 \mathrm{~mL}$ of water, does all of it dissolve? If not, how much dissolves?
Step 1
- The molar mass of radium (Ra) is approximately 226.03 g/mol. - The molar mass of sulfur (S) is approximately 32.07 g/mol. - The molar mass of oxygen (O) is approximately 16.00 g/mol. - Therefore, the molar mass of $\mathrm{RaSO}_4$ is: \[ 226.03 \, Show more…
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The $K_{\mathrm{sp}}$ value for radium sulfate, $\mathrm{RaSO}_{4}$, is $4.2 \times 10^{-11} .$ If $25 \mathrm{mg}$ of radium sulfate is placed in $1.00 \times 10^{2} \mathrm{mL}$ of water, does all of it dissolve? If not, how much dissolves?
The $K_{s p}$ value for radium sulfate, $\operatorname{RaSO}_{4},$ is $4.2 \times 10^{-11}$ If 25 mg of radium sulfate is placed in $1.00 \times 10^{2} \mathrm{mL}$ of water, does all of it dissolve? If not, how much dissolves?
Using the $K_{\mathrm{sp}}$ data in Table $22.1$, calculate the value of the equilibrium constant at $25^{\circ} \mathrm{C}$ for the reaction described by $$ \mathrm{Ag}_{2} \mathrm{SO}_{4}(s)+\mathrm{Ca}^{2+}(a q) \leftrightharpoons \mathrm{CaSO}_{4}(s)+2 \mathrm{Ag}^{+}(a q) $$ Calculate $\left[\mathrm{Ag}^{+}\right]$ and $\left[\mathrm{Ca}^{2+}\right]$ when excess $\mathrm{CaSO}_{4}(s)$ is equilibrated with $0.100 \mathrm{M} \mathrm{AgNO}_{3}(a q)$ at $25^{\circ} \mathrm{C}$.
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