An aqueous solution contains a mixture of .175 M HF (Ka = 7.2 x 10-4) and...

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An aqueous solution contains a mixture of .175 M HF(K_a = 7.2 x 10^-4) and .250 M HNO₂(K_a = 4.0 x 10^-4). Calculate the pH of thissolution (express your pH to the hundredth position).

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4.4 Ratings (751 Votes)

-log K_a = pK_a

For HF, pK_a = - log (7.2 x 10^-4) = 3.142

For HNO₂, pK_a = - log (4 x 10^-4) = 3.397

HF is the deciding reagent for pH.

Â Â Â Â Â Â Â Â Â Â Â Â HFÂ Â Â Â Â Â ---->Â Â Â Â Â H⁺Â Â Â Â + Â Â F^-

InitialÂ Â Â Â Â Â Â 0.175 MÂ Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â 0Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â 0

ChangeÂ Â Â Â Â -xÂ Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â +xÂ Â Â Â Â Â Â Â Â Â Â Â Â Â +x

EquilibriumÂ Â Â Â Â Â Â 0.175 - xÂ Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â xÂ Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â x

K_a = [H⁺][F^-] / [HF]

7.2 x 10^-4 = x² / (0.175 - x)

0.00072 (0.175 - x) = x²

x = 0.0112 M

[H⁺] = 0.0112 M

pH = -log [H⁺] = 1.95

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An aqueous solution contains a mixture of .175 M HF (Ka = 7.2 x 10-4) and...

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60.1K

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Chemistry

An aqueous solution contains a mixture of .175 M HF(K_a = 7.2 x 10^-4) and .250 M HNO₂(K_a = 4.0 x 10^-4). Calculate the pH of thissolution (express your pH to the hundredth position).

Answer & Explanation Solved by verified expert

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An aqueous solution contains a mixture of .175 M HF (Ka = 7.2 x 10-4) and...

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Chemistry

An aqueous solution contains a mixture of .175 M HF(Ka = 7.2 x 10-4) and .250 M HNO2(Ka = 4.0 x 10-4). Calculate the pH of thissolution (express your pH to the hundredth position).

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An aqueous solution contains a mixture of .175 M HF(K_a = 7.2 x 10^-4) and .250 M HNO₂(K_a = 4.0 x 10^-4). Calculate the pH of thissolution (express your pH to the hundredth position).