Answered

The Ksp of barium sulfate (BaSO4) is 1.1 × 10–10. What is the solubility concentration of sulfate ions in a saturated solution at 25°C?

a.1.0 x 10^-5m

B1.5 x10^-5m
C5.5 x 10^-11m

d.7.4 x 10^-6m

Verified Answer :

Given:

Ksp of BaSO4 = 1.1 10⁻¹⁰

To determine:

The solubility concentration of SO4²⁻ ions

Explanation:

BaSO4 ↔ Ba²⁺(aq) + SO4²⁻(aq)

Ksp = [Ba²⁺][SO4²⁻]

if 's' is the solubility of the ions then we have

Ksp = s²

s = √ksp = √1.110⁻¹⁰ = 1.0510⁻⁵M

Ans: solubility of sulfate ions is 1.0510⁻⁵ M

The solubility concentration of sulfate ions in the given saturated solution of BaSO₄ at 25°C is 1.05 × 10⁻⁵M.

What is Ksp?

Ksp is known as the solubility product sonstant which is equal to the product of the concentration of their constituent ions.

Given chemical reaction is:

BaSO₄ ⇄ Ba²⁺(aq) + SO₄²⁻(aq)

Let the solubility of the Ba²⁺ & SO₄²⁻ ions be x, and Ksp equation will be written as:

Ksp = [Ba²⁺][SO₄²⁻]

1.1 × 10⁻¹⁰ = x²

x = √1.1 × 10⁻¹⁰ = 1.05 × 10⁻⁵M

Hence option (a) is correct.

To know more about Ksp, visit the below link:

https://brainly.com/question/25134328

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