Consider formic acid, HCHO2 (Ka = 1.9x10-4) and its conjugate base, CHO2-. a) A buffer is prepared...

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Consider formic acid, HCHO2 (Ka = 1.9x10-4) and its conjugatebase, CHO2-.
a) A buffer is prepared by dissolving 25.0 grams of sodiumformate in 1.30 L of a solution of 0.660 M formic acid. Assume thevolume remains constant after dissolving the sodium formate.
Â Â i) Calculate the pH of this buffer.
Â Â ii) Calculate the pH after 0.100 mole of nitricacid is added to this buffer.
Â Â iii) Calculate the pH after 10.0 grams of potassiumhydroxide is added to this buffer.
Â Â iv) What is the buffer capacity of this buffer?
b) 35.0 mL of 0.739 M formic acid is titrated with 0.431 Mpotassium hydroxide.
Â Â i) What is the pH of the formic acid solutionbefore titration begins?
Â Â ii) How many milliliters of KOH is required forthis titration to reach its equivalence point?
Â Â iii) What is the pH of the solution after 10.0 mLof KOH has been added?
Â Â iv) What is the pH of the solution halfway toequivalence?
Â Â v) What is the pH of the solution at theequivalence point?

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b HCOOH Ka value 19 x 104 pKa 372 i What is the pH of the formic acid solution before titration begins pH 12 pKa logC pH 12 372 log 0739 pH 193 ii How many See Answer

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