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pishuonlain [190]
3 years ago
9

There are some data that suggest that zinc lozenges can significantly shorten the duration of a cold. If the solubility of zinc

acetate, Zn(CH3COO)2, is 43.0 g/L, what is the solubility product Ksp of this compound?
Chemistry
1 answer:
zhuklara [117]3 years ago
8 0

Answer:

K_{sp} of Zn(CH_{3}COO)_{2} is 0.0513

Explanation:

Solubility equilibrium of Zn(CH_{3}COO)_{2}:

Zn(CH_{3}COO)_{2}\rightleftharpoons Zn^{2+}+2CH_{3}COO^{-}

Solubility product of Zn(CH_{3}COO)_{2} (K_{sp}) is written as-            K_{sp}=[Zn^{2+}][CH_{3}COO^{-}]^{2}

Where [Zn^{2+}] and [CH_{3}COO^{-}] represents equilibrium concentration (in molarity) of Zn^{2+} and CH_{3}COO^{-} respectively.

Molar mass of Zn(CH_{3}COO)_{2} = 183.48 g/mol

So, solubility of Zn(CH_{3}COO)_{2} = \frac{43.0}{183.48}M = 0.234M

1 mol of Zn(CH_{3}COO)_{2} gives 1 mol of Zn^{2+} and 2 moles of CH_{3}COO^{-} upon dissociation.

so,   [Zn^{2+}] = 0.234 M and [CH_{3}COO^{-}] = (2\times 0.234)M=0.468M

so, K_{sp}=(0.234)\times (0.468)^{2}=0.0513          

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Answer:

Explanation:

The trick here is to realize that if you know the volume of a gas at STP, you can use the fact that

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Under STP conditions:

1 mole of an ideal gas = 22.7 L

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In your case, you know that your sample of gas occupies

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

1 mole gas

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=

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1

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