Answer :
Answer:
Explanation:
The solution contain 0.01 M concentration of Ba²⁺
0.01M concentration of Ca²⁺
Ksp ( solubility constant) for BaSO₄ = 1.07 × 10⁻¹⁰
Ksp for CaSO₄ = 7.10 × 10⁻⁵
(BaSO₄) = (Ba²⁺) (SO₄²⁻)
1.07 × 10⁻¹⁰ = 0.01 M (SO₄²⁻)
1.07 × 10⁻¹⁰ / 0.01 = ( SO₄²⁻)
1.07 × 10⁻⁸ M = ( SO₄²⁻)
so the minimum of concentration of concentration sulfate needed is 1.07 × 10⁻⁸ M
For CaSO₄
CaSO₄ = ( Ca²⁺) ( SO₄²⁻)
7.10 × 10⁻⁵ = 0.01 (SO₄²⁻)
(SO₄²⁻) = 7.10 × 10⁻⁵ / 0.01 = 7.10 × 10⁻³ M
so BaSO₄ will precipitate first since its cation (0.01 M Ba²⁺) required a less concentration of SO₄²⁻ (1.07 × 10⁻⁸ M ) compared to CaSO₄
b) The minimum concentration of SO₄²⁻ that will trigger the precipitation of the cation ( 0.01 M Ba²⁺) that precipitates first is 1.07 × 10⁻⁸ M
The cation which precipitates first is Ba²⁺ and the minimum concentration of SO₄²⁻ that will trigger the precipitation of that cation is 1.07 × 10⁻⁸ M.
What is Ksp?
Ksp is known as the solubility product constant which in equilbrium shows the dissociation of any solid into their constitute ions in an aqueous solution.
Given value of Ksp for BaSO₄ = 1.07 × 10⁻¹⁰
Given value of Ksp for CaSO₄ = 7.10 × 10⁻⁵
- Solubility product constant of BaSO₄ in terms of concentration will be written as:
[BaSO₄] = [Ba²⁺] [SO₄²⁻]
1.07 × 10⁻¹⁰ = 0.01 M [SO₄²⁻]
1.07 × 10⁻¹⁰ / 0.01 = [SO₄²⁻]
[SO₄²⁻] = 1.07 × 10⁻⁸ M
- Solubility product constant of CaSO₄ in terms of concentration will be written as:
[CaSO₄] = [Ca²⁺] [SO₄²⁻]
7.10 × 10⁻⁵ = 0.01 [SO₄²⁻]
[SO₄²⁻] = 7.10 × 10⁻⁵ / 0.01 = 7.10 × 10⁻³ M
From the above calculation it is clear that Ba²⁺ will precipitate first as it requires less amount of sulphate ion and minimum concentration of SO₄²⁻ ion is 1.07 × 10⁻⁸ M.
Hence, Ba²⁺ will precipitate first and required concentration of SO₄²⁻ ion is 1.07 × 10⁻⁸ M.
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