A buffer was prepared containing 0.50 M formic acid (HCOOH) and 0.50 M sodium formate (NaCOOH). The Ka of formic acid is 1.7 x 1

Question

2 years ago

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0-4. What will be the pH after 0.010 mol of NaOH(s) is added to 100.0 mL of the buffer

1 answer:

olga_2 [115] · Answer 1 · 2023-05-01T22:57:30+03:00

For a buffer that was prepared contain 0.50 M formic acid (HCOOH) and 0.50 M sodium formate (NaCOOH). the pH is mathematically given as

pH=3.95

<h3>What is the pH after 0.010 mol of NaOH(s) is added to 100.0 mL of the buffer?</h3>

Generally, the equation for the Hendersons equation is mathematically given as

pH=pKa+log(SALT)/(ACID)

Where

moles of (NaCOOH)=100*0.05/1000

moles of (NaCOOH)=0.05moles

and formic acid

moles of formic acid=100*0.05/1000

moles of formic acid=0.05moles

Therefore

pKa=-logka

pKa=1.4*10*3.77

pH=3.77+log{0.06/0.04}

pH=3.95

In conclusion, the pH is

pH=3.95