In a 500-mL volumetric flask, 0.050 mole of formic acid (Ka=1.82 x 10-4) and 0.05 mole...

In a 500-mL volumetric flask, 0.050 mole of formic acid (Ka=1.82 x 10^-4) and 0.05 mole of NaOh are placed together and diluted to exactly 500.0 mL. What is the pH of the resulting solution?

Expert Solution

moles of HCOOH = 0.050 mol

volume = 500 mL = 0.500 L

concentration of formic acid = 0.050 / 0.500 = 0.10 M

concentration of NaOH = 0.05 / 0.500 = 0.10 M

HCOOH + NaOH ---------------> HCOONa + H2O

0.10 0.10 0 0

0 0 0.10

concentration of HCOONa = 0.10 M

pH = 7 + 1/2 (pKa + log C)

= 7 + 1/2 (3.74 + log 0.10)

pH = 8.37

queen_honey_blossom answered 2 years ago

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