Q19.19P Find the pH of a buffer that con... [FREE SOLUTION]

Chapter 19: Q19.19P (page 873)

Find the pH of a buffer that consists of 0.25M ${NH}_{3}$ and 0.15M ${NH}_{4} Cl$ ( ${pK}_{b}$ of ${NH}_{3} = 4.75$ )?

Short Answer

Expert verified

The pH value is 9.47.

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 given solution

Write the 0.25 M ${NH}_{3}$ dissociation equation first.

${NH}_{3} {+H}_{2} O 鈬� N {H_{3}}^{+} {+ OH}^{-} .$

Then write the 0.15 M ${NH}_{4} Cl$ dissociation equation.

${NH}_{4} Cl 鈫� N {H_{4}}^{+} {+ Cl}^{-} .$

We now have the initial ammonia and ammonium concentrations.

${NH}_{3} = 0.25 M. N {H_{4}}^{+} = 0.15 M.$

To find the pH, we may utilize the Henderson-Hasselbalch equation. First, solve for the value of ${pK}_{a}$ as:

role="math" localid="1663396782915" ${pK}_{w} {= pK}_{a} {+ pK}_{b} {pK}_{a} {= pK}_{w} {+ pK}_{b} = 14 - 4.75 = 9.25. pH = pKa + log \frac{[base]}{[acid]} = pKa + log \frac{[{NH}_{3}]}{[N {H_{4}}^{+}]} = 9.25 + log \frac{0.25 M}{0.15 M} = 9.47.$

Therefore, the pH value is 9.47.

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91影视

Find the pH of a buffer that consists of 0.25M ${NH}_{3}$ and 0.15M ${NH}_{4} Cl$ ( ${pK}_{b}$ of ${NH}_{3} = 4.75$ )?

Short Answer

Step by step solution

Define Ionic Equilibrium

The pH of the given solution

One App. One Place for Learning.

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91影视

Find the pH of a buffer that consists of 0.25MNH3and 0.15MNH4Cl(pKbofNH3= 4.75)?

Short Answer

Step by step solution

Define Ionic Equilibrium

The pH of the given solution

One App. One Place for Learning.

Most popular questions from this chapter

Recommended explanations on Chemistry Textbooks

Making Measurements

The Earths Atmosphere

Organic Chemistry

Physical Chemistry

Inorganic Chemistry

Chemical Analysis

Study anywhere. Anytime. Across all devices.

Find the pH of a buffer that consists of 0.25M ${NH}_{3}$ and 0.15M ${NH}_{4} Cl$ ( ${pK}_{b}$ of ${NH}_{3} = 4.75$ )?