The acid dissociation constants for sulfurous acid are: Ka1 = 1.2 x 10-2 and Ka2 = 6.6 x 10-8 (a) Calculate the pH of a solution of 0.10 M H2SO3. (b) Calculate the pH of a solution of 0.10 M Na2SO3. (c) Calculate the pH of the solution resulting when equal volumes of the solutions described in parts (a) and (b) are mixed.

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A: Answer: Given data: pH=2.62α=0.02C=0.12M

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A: pH is defined as negative logarithm of hydrogen ion concentration.

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A: Given: The simplest amino acid is glycine, H2NCH2COOH.

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A: PH = -log [H+]

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A: The dissociation reaction taking place is BOH ⇌ B+ + OH-

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A:

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A: Determine the pH of a 0.13 M solution of pyridinium nitrate

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A: We will calculate pH

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A: As the pH of Na2CO3 is 11.0 which means that it is basic in nature.

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A:

Q: you mix 100. mL of 0.11 M HCl with 50.0 mL of 0.22 M NH3, what is the pH of the resulting solution?…

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A: Given data, The pOH of a weak base is calculated as shown below.

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A:

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A:

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A: Given information: 0.10 M NaNO2 Ka of HNO2 is 4.5 x 10-4

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Q: Determine the pH of the solution

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A:

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