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Minchanka [31]
3 years ago
11

A sample of Cd(OH)2 is added to pure water and allowed to come to equilibrium at 25ºC. The concentration of Cd +2 = 1.7 x 10 -5M

at equilibrium. Calculate Ksp.
Chemistry
1 answer:
Archy [21]3 years ago
3 0

Answer:

Ksp=2.0x10^{-14}

Explanation:

Hello there!

In this case, given the solubilization of cadmium (II) hydroxide:

Cd(OH)_2(s)\rightleftharpoons Cd^{2+}(aq)+2OH^-(aq)

The solubility product can be set up as follows:

Ksp=[Cd^{2+}][OH^-]^2

Now, since we know the concentration of cadmium (II) ions at equilibrium and the mole ratio of these ions to the hydroxide ions is 1:2, we infer that the concentration of the latter at equilibrium is 3.5x10⁻⁵ M. In such a way, the resulting Ksp turns out to be:

Ksp=(1.7x10^{-5})(3.4x10^{-5})^2\\\\Ksp=2.0x10^{-14}

Regards!

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<h3>Answer:</h3>

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<h3>Explanation:</h3>

Step 1: Calculate mass of Fe;

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Or,

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Putting values,

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Step 2: Calculate amount of FeCl₂;

The balance chemical equation is as follow,

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       55.85 g (1 mol) Fe produced  =  110.98 g (1 mol) of FeCl₂

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               81.744 g Fe will produce  =  X g of FeCl₂

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