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Anna35 [415]
3 years ago
13

The ksp of yttrium fluoride, yf3, is 8.62 × 10-21. calculate the molar solubility of this compound.

Chemistry
1 answer:
motikmotik3 years ago
6 0

Answer:

The molar solubility of YF₃ is 4.23 × 10⁻⁶ M.

Explanation:

In order to calculate the molar solubility of YF₃ we will use an ICE chart. We identify 3 stages: Initial, Change and Equilibrium and we complete each row with the concentration of change of concentration. Let's consider the solubilization of YF₃.

       YF₃(s) ⇄ Y³⁺(aq) + 3 F⁻(aq)

I                       0               0

C                     +S            +3S

E                       S              3S

The solubility product (Ksp) is:

Ksp = [Y³⁺].[F⁻]³= S . (3S)³ = 27 S⁴

S=\sqrt[4]{Ksp/27} =\sqrt[4]{8.62 \times 10^{-21}  /27}=4.23 \times 10^{-6}M

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<em />

To solve this question we need to convert each mass of reactant to moles using its respectives molar masses in order to find limitng reactant. Moles of limiting reactant = Moles of iron produced:

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