Be sure to answer all parts. find the molar solubility of bacro4 (ksp= 2.1 × 10−10) in (a) pure water × 10 m (b) 1.6 × 10−3 m na2cro4 × 10 m

The molar solubility of BaCrO₄ in pure water is 1.4 × 10⁻⁵ M, while the molar solubility in 1.6 × 10⁻³ M Na₂CrO₄ is 1.3 × 10⁻⁷ M.

Let's consider the solution of BaCrO₄.

BaCrO₄(s) ⇄ Ba²⁺(aq) + CrO₄²⁻(aq)

To find the molar solubility (S) in pure water, we need to make an ICE chart.

        BaCrO₄(s) ⇄ Ba²⁺(aq) + CrO₄²⁻(aq)

I                                0                 0

C                              +S               +S

E                               S                  S

The solubility product constant is:

To calculate the molar solubility of BaCrO₄ in 1.6 × 10⁻³ M Na₂CrO₄, we need to consider the Na₂CrO₄ that is a strong electrolyte. Thus, when making the ICE chart, the initial concentration of CrO₄²⁻ will be 1.6 × 10⁻³ M.

   BaCrO₄(s) ⇄ Ba²⁺(aq) + CrO₄²⁻(aq)

I                                0          1.6 × 10⁻³

C                              +S               +S

E                               S        1.6 × 10⁻³ + S

The solubility product constant is:

Since 1.6 × 10⁻³ >>> S, 1.6 × 10⁻³ + S ≅ 1.6 × 10⁻³

The molar solubility of BaCrO₄ in pure water is 1.4 × 10⁻⁵ M, while the molar solubility in 1.6 × 10⁻³ M Na₂CrO₄ is 1.3 × 10⁻⁷ M.

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