Question

The ksp for silver sulfate (ag2so4) is 1. 2 ✕ 10-5. Calculate the solubility of silver sulfate in each of the following

Answer 1

For ksp of silver sulfate (ag2so4) at 1. 2 ✕ 10-5, the solubility of silver sulfate is mathematically given as

x = 5.26*10^{-4}

What is the solubility of silver sulfate in 0.15 M AgNO3?

Generally, the equation for the  Chemical reaction is mathematically given as

Ag2SO4 ⇄ 2Ag+  + SO4 2-

Therefore

Ksp = [Ag+ ]2 *[SO4 2-]

1.2*10-5 = ( 0.15 +2x)2*(x)

x = 5.26*10^{-4}

In conclusion, the solubility of silver sulfate is

x = 5.26*10^{-4}

Read more about Chemical reaction

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Answer 2

If the ksp of silver sulfate (ag2so4) at 1.2 × 10⁻⁵, the solubility of silver sulfate is  5.26 × 10⁽⁻⁴⁾.

What is the ksp value?

ksp value determines the equilibrium between the solids and its respective ions in a solution.

The reaction is $\rm Ag_2SO_4 \leftrightharpoons 2Ag+ + SO_4^2-$

The ksp pf silver sulfate is  1.2 × 10⁻⁵

Tho calculate the solubility?

Putting the values in the equation

$\rm Ksp = [Ag^+ ]^2 \times [SO_4^ 2^-]\\\\1.2\times 10^-^5 = ( 0.15 +2x)2\times (x)\\x = 5.26\times 10^{-4}$

Thus, the solubility of silver sulfate is  5.26 × 10⁽⁻⁴⁾.

Learn more about silver sulfate

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