Calculate the molar solubility of magnesium fluoride (MgF2) in a solution that is 0.250 M in NaF. For magnesium fluoride, Ksp = 5.16 * 10 - 11.

Question

contestada

Respuesta :

PiaDeveau PiaDeveau · Answer 1 · 2020-08-15T04:25:17+02:00

Answer:

Molar solubility of magnesium fluoride (MgF2) = 8.26 × 10⁻¹⁰ M

Explanation:

Given:

Ksp = 5.16 × 10⁻¹¹

NaF = 0.250

Find:

Molar solubility of magnesium fluoride (MgF2)

Computation:

Molar solubility of magnesium fluoride (MgF2) = Ksp / NaF²

Molar solubility of magnesium fluoride (MgF2) = 5.16 × 10⁻¹¹ / (0.250)²

Molar solubility of magnesium fluoride (MgF2) = 8.26 × 10⁻¹⁰ M

Answer Link

andromache andromache · Answer 2 · 2022-03-29T19:48:31+02:00

The molar solubility of magnesium fluoride (MgF2) is 8.26 × 10⁻¹⁰ M.

Since

Ksp = 5.16 × 10⁻¹¹

NaF = 0.250

Now we know that

Molar solubility of magnesium fluoride (MgF2) = Ksp / NaF²

= 5.16 × 10⁻¹¹ / (0.250)²

= 8.26 × 10⁻¹⁰ M

hence, The molar solubility of magnesium fluoride (MgF2) is 8.26 × 10⁻¹⁰ M.

Learn more about molar here: https://brainly.com/question/14776534