Question

At 25 °c only 0.0260 mol of the generic salt ab3 is soluble in 1.00 l of water. what is the ksp of the salt at 25 °c?

Answer 1

Given:

At 25 degrees Celcius:

amount of generic salt AB3 = 0.0260 moles
Volume of solvent = 1.0 L water

Set up a balanced chemical equation:

AB3 =========> A3+ + 3B-
0.0260M             0.0260   0.078

Ksp = [A][B]^3
Ksp = 1.23 x 10^-5

Answer 2

We have that for the Question, it can be said that the ksp of the salt at 25 °c is

Ksp=1.23*10^{-5}

From the question we are told

At 25 °c only 0.0260 mol of the generic salt ab3 is soluble in 1.00 l of water. what is the ksp of the salt at 25 °c

Generally the equation for Ksp   is mathematically given as

Ksp=(X)(Y)^3

Where

ab3=0.0260 moles

Vol of solvent =1.0L

Having the equation as

$ab3=a3+3B-\\\\Where\\\\ab3=0.0260\\\\a3+0.0260\\\\3B-=0.078$

Therefore

the ksp of the salt at 25 °c is

Ksp=(0.0260)(0.078)^3

Ksp=1.23*10^{-5}

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