Chapter 19: Q19.15P (page 873)

Find the pH of a buffer that consists of 0.45M HCOOH and 0.63M HCOONa ( ${pK}_{a}$ of HCOOH=3.74)?

Short Answer

Expert verified

The pH is obtained is 3.89 .

Step by step solution

Define Ionic Equilibrium

AN ionic equilibrium refers to an equilibrium that exists in the solution of weak electrolytes between unionized molecules and ions.

The pH of the buffer solution

Write the 0.45 M HCOOH dissociation equation first.

${HCOOH +H}_{2} O ⇄ {HCOO}^{-} {+H}_{3} O^{+} .$

Then, write the 0.63 M HCOONa dissociation equation.

$HCOONa \to {HCOO}^{-} {+ Na}^{+} .$

We now have the initial formic acid and formate concentrations.

$HCOOH = 0.45 M {HCOO}^{-} = 0.63 M$

To find the pH, we may utilize the Henderson-Hasselbalch equation.

$pH = pKa + log \frac{[{HCOO}^{-}]}{[HCOOH]} = 3.74 + log \frac{0.63 M}{0.45 M} = 3.89.$

Therefore, the pH value is3.89.

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Find the pH of a buffer that consists of 0.45M HCOOH and 0.63M HCOONa ( ${pK}_{a}$ of HCOOH=3.74)?

Short Answer

Step by step solution

Define Ionic Equilibrium

The pH of the buffer solution

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Find the pH of a buffer that consists of 0.45M HCOOH and 0.63M HCOONa ( pKaof HCOOH=3.74)?

Short Answer

Step by step solution

Define Ionic Equilibrium

The pH of the buffer solution

One App. One Place for Learning.

Most popular questions from this chapter

Recommended explanations on Chemistry Textbooks

Chemical Reactions

Ionic and Molecular Compounds

Nuclear Chemistry

Organic Chemistry

Kinetics

Chemistry Branches

Study anywhere. Anytime. Across all devices.

Find the pH of a buffer that consists of 0.45M HCOOH and 0.63M HCOONa ( ${pK}_{a}$ of HCOOH=3.74)?