Question

QUESTION 12 Consider the following partially soluble compound in water. Sc(OH)$_3$(s) $\rightleftharpoons$ Sc$^{3+}$(aq) + 3OH$^{-}$(aq) K$_{sp}$ = 8.0 $\times$ 10$^{-31}$ S = 1.3 $\times$ 10$^{-8}$ in pure water. However, what is the solubility of Sc(OH)$_3$ in a pH=10 solution? Hint: The high pH means OH$^{-}$ from a second source $\rightarrow$ common ion effect. S = 8.0 $\times$ 10$^{-19}$ S = 8.0 $\times$ 10$^{-27}$ S = 8.0 $\times$ 10$^{-15}$ S = 3.0 $\times$ 10$^{-8}$

          QUESTION 12
Consider the following partially soluble compound in water.
Sc(OH)$_3$(s) \(\rightleftharpoons\) Sc$^{3+}$(aq) + 3OH$^{-}$(aq)  K$_{sp}$ = 8.0 \(\times\) 10$^{-31}$
S = 1.3 \(\times\) 10$^{-8}$ in pure water.
However, what is the solubility of Sc(OH)$_3$ in a pH=10 solution?
Hint: The high pH means OH$^{-}$ from a second source \(\rightarrow\) common ion effect.
S = 8.0 \(\times\) 10$^{-19}$
S = 8.0 \(\times\) 10$^{-27}$
S = 8.0 \(\times\) 10$^{-15}$
S = 3.0 \(\times\) 10$^{-8}$

QUESTION 12
Consider the following partially soluble compound in water.
Sc(OH)3(s) ⇌ Sc^3+(aq) + 3OH^-(aq) Ksp = 8.0 × 10^-31
S = 1.3 × 10^-8 in pure water.
However, what is the solubility of Sc(OH)3 in a pH=10 solution?
Hint: The high pH means OH^- from a second source → common ion effect.
S = 8.0 × 10^-19
S = 8.0 × 10^-27
S = 8.0 × 10^-15
S = 3.0 × 10^-8

Added by Samantha J.

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