Question

. The Ksp of barium sulfate is 1.1 × 10–10. What is the sulfate-ion concentration of a 1.0-L saturated solution of BaSO4 to which 0.025 mol of Ba(NO3)2 is added? 4.4 × 10–9M 1.0 × 10–5M 6.6 × 10–5M 2.8 × 10–12M

Answer 1

`[SO_4^(2-)]=4.4*10^(-9)M`

Step-by-step explanation:

From the question we are told that:

`Ksp=1.1*10^(-10)`

Volume of
`SO_4^(2-)=1.O`

Moles of
`Ba(NO_3)^2 =0.025`

Generally the equation for Ksp is mathematically given by

`Ksp=[Ba^(2+)][SO_4^(2-)]`

`1.1*10^(-10)=[0.025][SO_4^(2-)]`

Therefore

`[SO_4^(2-)]=4.4*10^(-9)M`