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ikadub [295]
2 years ago
13

An unknown weak acid with a concentration of 0.530 M has a pH of 5.600. What is the Ka of the weak acid

Chemistry
1 answer:
Aleks [24]2 years ago
6 0

Answer:

Ka = 3.45x10⁻⁶

Explanation:

First we <u>calculate [H⁺]</u>, using <em>the given pH</em>:

  • pH = -log[H⁺]
  • [H⁺] = 10^{-pH}=10^{-5.6}
  • [H⁺] = 2.51x10⁻⁶ M

To solve this problem we can use the following formula describing a monoprotic weak acid:

  • [H⁺] = \sqrt{C*Ka}

We <u>input the data that we already know</u>:

  • 2.51x10⁻⁶ = \sqrt{0.530*Ka}

And <u>solve for Ka</u>:

  • Ka = 3.45x10⁻⁶
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Explanation:

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<em>∴ m = (mass/molar mass of solute)/(mass of water (kg)).</em>

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∵ m = (mass/molar mass of CaCl₂·6H₂O)/(mass of water (kg)).

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∴ 0.125 m = (mass of CaCl₂·6H₂O / 219.0757 g/mol)/(0.5 kg).

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<u><em>(b) What mass of NiSO₄·6H₂O must be dissolved in 500. g of water to produce 0.22 m NiSO₄(aq)?</em></u>

∵ m = (mass/molar mass of NiSO₄·6H₂O)/(mass of water (kg)).

m = 0.22 m, molar mass of NiSO₄·6H₂O = 262.84 g/mol, mass of water = 500.0 g = 0.5 kg.

∴ 0.125 m = (mass of NiSO₄·6H₂O / 262.84 g/mol)/(0.5 kg).

∴ mass of NiSO₄·6H₂O = (0.22 m)(262.84 g/mol)(0.5 kg) = 28.91 g.

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