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Sunny_sXe [5.5K]

3 years ago

9

G the ksp of calcium hydroxide, ca(oh)2, is 5.02 × 10-6. calculate the molar solubility of this compound.

1 answer:

g100num [7]3 years ago

7 0

<span>When calcium hydroxide dissolves, it dissociates into Ca(OH)2 = Ca2+ and 2OH- Let's assign the variable X for the solubility of Ca2+ and OH I.e Ca2+ = X and 2OH- = 2X Then Ksp = [Ca2+][OH-]^2 So we have (X) (2X)^2 = 5.02 * 10^(-6) 4X^3 = 5.02 * 10 ^(-6) X^3 = 5.02 * 10^(-6) / 4 X^3 = 0.003110 X = 0.1459</span>

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Explanation:

$2HI(g)\rightarrow H_2(g)+I_2(g)
$

Rate Law: $k[HI]^2
$

Rate constant of the reaction = k = $6.4\times 10^{-9} L/mol s$

Order of the reaction = 2

Initial rate of reaction = $R=1.6\times 10^{-7} Mol/L s$

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$1.6\times 10^{-7} mol/L s=(6.4\times 10^{-9} L/mol s)[HI]^2$

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