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1 year ago

what is the solubility of ca(oh)2 (s) in water, given that the ksp is 6.5 x 10-6. molar mass of ca(oh)2 is 74.09 g/mol. g

Chemistry

1 answer:

Pani-rosa [81]1 year ago

8 0

8.7M Is the solubility of Ca(oh)2 in water at a given Ksp of 6.5 .10-6 and molar mass of 74.09g/mol.

Solubility is defined as the amount of the substance dissolved in a given amount of solvent at a certain temperature.

Ca(OH)2 à Ca2+ + 2OH-

Ksp = 6.5 .10-6

Molar mass= 74.09 g/mol

Ksp is solubility product constant which describes the equilibrium between a solid and its ion in solution.

Ksp=[Ca2+] [OH2-]

6.5 .10-6 = S. (74.09g/mol +S)

6.5 .10-6 = S .( 74.09M)

S = 6.5 .10-6 /74.09 M

= 8.7 M

So, the solubility of Ca(OH)2 is 8.7M.

To learn more about solubility product constant please visit:

brainly.com/question/1419865

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