A formic acid buffer containing 0.50 M HCOOH and 0.50 M HCOONa hasa pH of 3.77....

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Question

A formic acid buffer containing 0.50 M HCOOH and 0.50 M HCOONa hasa pH of 3.77....

A formic acid buffer containing 0.50 M HCOOH and 0.50 M HCOONa hasa pH of 3.77. What will the pH be after 0.010 mol of NaOH has beenadded to 100.0 mL of the buffer?

correct answer: 3.95

please show me step by step how to solve this problem, i couldn'tget the right answer above. Thanks in advance!

science chemistry

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Answer 1

Answer #1

Number of moles of formic acid = 0.5 M * 0.1L

=0.05 mol

Number of moles of sodium formate = 0.5 M * 0.1L

= 0.05 mol

When NaOH is added the number of moles of the aciddecreases and the moles of sodium formate increases .

HCOOH + NaOH

HCOONa + H2O

0.01mol 0.01mol 0.01 mol

pH = PKa + log [HCOONa] /[HCOOH]

= - log 1.7 x 10^-4 + log [0.05 +0.01 ] /[0.05-0.01]

= 3.76 + 0.176

= 3.936

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Answer 2

Answer #2

TheICE tablefor dissociation of formic acidis, I:0.5 C:-0.1 0.4 0.1 0.1 0 0.5 0.1 0.6 pKa of formicacidis3.77 From Henderson-

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Answer 3

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