Answered

Join IDNLearn.com and start exploring the answers to your most pressing questions. Our community provides timely and precise responses to help you understand and solve any issue you face.

Calculate the solubility of Ca(OH)2 in a 0.469M CaCl2 solution at 31°C, given that the Ksp of Ca(OH)2 is 4.96 x 10-6 at that temperature. Give your answer in milliMolar units 2.927 mM 1.626 mM 2.764 mM 1.382 mM 1.463 mM 3.252 mM​

Sagot :

Onyebuchinnajiidn

The solubility of Ca(OH)2 in a 0.469M CaCl2 solution at 31°C, at given Ksp of Ca(OH)2 is determined as 1.626 mM.

Dissociation reaction of Ca(OH)2

The dissociation reaction of Ca(OH)2 is given as follows;

Ca(OH)₂  ⇄ Ca²⁺  + 2OH⁻¹

                     x           2x

Concentration of Ca²⁺ = 0.469 M

Ksp = [x][2x]²

ksp = (0.469)(2x²)

ksp = 4(0.469)x²

ksp = 1.876x²

4.96 x 10⁻⁶ = 1.876x²

x² = (4.96 x 10⁻⁶)/(1.876)

x² = 2.643 x 10⁻⁶

x = √(2.643 x 10⁻⁶)

x = 1.626 x 10⁻³ M

x = 1.626 mM

Thus, the solubility of Ca(OH)2 in a 0.469M CaCl2 solution at 31°C, at given Ksp of Ca(OH)2 is determined as 1.626 mM.

Learn more about solubility here: https://brainly.com/question/23946616

#SPJ1

We appreciate your contributions to this forum. Don't forget to check back for the latest answers. Keep asking, answering, and sharing useful information. IDNLearn.com has the solutions you’re looking for. Thanks for visiting, and see you next time for more reliable information.