Chemistry, 15.01.2020 03:31 holyturnley

Chromium(iii) hydroxide has ksp 1.6 x 10-30. what is the molar solubility of cr(oh)3 in a solution whose ph is maintained at 6.00?

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Answer from: tylerkrobinson7853

Explanation:

Chemical reaction equation for $Cr(OH)_{3}$ is as follows.

$Cr(OH)_{3} \rightarrow Cr^{3+} + 3OH^{-}$

As it is given that pH is 6. So, the concentration of hydrogen ions will be as follows.

pH = $-log [H^{+}]$

antilog (-6) = $[H^{+}]$

$[H^{+}] = 10^{-6}$

and $[OH^{-}] = \frac{10^{-14}}{[H^{+}]}$

= $\frac{10^{-14}}{10^{-6}}$

= $10^{-8}$

Now, let us assume that the solubility is "s". Therefore,

$Cr(OH)_{3} \rightarrow Cr^{3+} + 3OH^{-}$

s $10^{-8}$

Therefore, calculate the value of $K_{sp}$ for this reaction as follows.

$K_{sp} = [Cr^{3+}][10^{-8}]^{3}$

$1.6 \times 10^{-30} = s \times (10^{-8})^{-30}$

s = $1.6 \times 10^{-6} mol/L$

Thus, we can conclude that the molar solubility of $Cr(OH)_{3}$ is $1.6 \times 10^{-6} mol/L$ .

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