Question

The solubility of eu(oh) 2 in a solution of 0.0151 m koh is 1.20 10 -5 m . calculate k sp for eu(oh) 2 .

Answer 1

To calculate
`Ksp for Eu(OH)2` lity information
`(1.20 x 10^-5 M) in a 0.0151` he values into the solubility product expression Ksp
`= [Eu^2+][OH-]^2 to find Ksp = 6.91 x 10^-16.`

Step-by-step explanation:

To calculate Ksp for Eu(OH)2, we need to use the solubility information provided. The solubility of Eu(OH)2 in a 0.0151 M KOH solution is given as
`1.20 x 10^-5 M`for the dissolution of
`Eu(OH)2 is Eu(OH)2 (s) ⇌ Eu^2+ (aq) + 2OH- (aq)`

From the solubility information, we can determine that
`[Eu^2+] = 1.20 x 10^-5 M and [OH-] = 2 x 1.20 x 10^-5 M = 2.40 x`

Using the solubility product expression,
`Ksp = [Eu^2+][OH-]^2`the values to calculate Ksp = (1.20 x
`10^-5)(2.40 x 10^-5)^2 = 6.91 x 10^-16.`

Answer 2

The
`\(K_{\text{sp}}\)`for
`\(Eu(OH)_2\)`is approximately
`\(4.32 * 10^(-16)\)`.

The solubility product constant
`(\(K_{\text{sp}}\))` for a sparingly soluble salt, like
`\(Eu(OH)_2\)`, is the product of the concentrations of its ions raised to the power of their coefficients in the balanced chemical equation.

The balanced chemical equation for the dissociation of
`\(Eu(OH)_2\)` is:

`\[ Eu(OH)_2 \rightleftharpoons Eu^(2+) + 2OH^- \]`

The dissociation's equilibrium expression is provided by:

`\[ K_{\text{sp}} = [Eu^(2+)][OH^-]^2 \]`
`\(1.20 * 10^(-5) \, \text{M}\),`

Given that the solubility of
`\(Eu(OH)_2\)` in a solution of
`\(0.0151 \, \text{M} \, KOH\)` is
`\(1.20 * 10^(-5) \, \text{M}\)`, we can use this information to set up the equilibrium concentrations:

`\[ [Eu^(2+)] = 1.20 * 10^(-5) \, \text{M} \]`

`\[ [OH^-] = 2 * [Eu^(2+)] = 2 * 1.20 * 10^(-5) \, \text{M} \]`

Now, substitute these values into the
`\(K_{\text{sp}}\)`expression:

`\[ K_{\text{sp}} = (1.20 * 10^(-5)) * (2 * 1.20 * 10^(-5))^2 \]`

`\[ K_{\text{sp}} = 1.20 * 10^(-5) * 4 * (1.20 * 10^(-5))^2 \]`

`\[ K_{\text{sp}} = 4.32 * 10^(-16) \]`

Therefore, the
`\(K_{\text{sp}}\)`for
`\(Eu(OH)_2\)`is approximately
`\(4.32 * 10^(-16)\)`.