Chapter 10: QBE (page 229)

(c) How many milliliters of $0.320 {MNHO}_{3}$ should be added to $4.00 g$ of to give a pH of $10.00$ in $250 mL$ ?

Short Answer

Expert verified

The volume of nitric acid is = 61.6mL

Step by step solution

Define the Henderson-Hasselbalch equation.

The relationship between pH and pKa(acid dissociation constant)of acids in aqueous solutions is described by the Henderson-Hasselbalch equation. This equation can be used to forecast the pH of a buffer solution when the concentrations of such acid as well as its conjugate base, or the base and the related conjugate acid, are determined.

$pH = {pKK}_{1} + \log \frac{|{HA}^{-}|}{|H_{2} A|}$

Step 2:Calculate the volume of nitric acid

The of the given solution (after acid is added) is $10.31$ .

$\to_{{HCO}_{3}^{-}} {CO}_{3}^{2 -} + H^{+}$

Initial molecules: $0 . 0289_{4} x$

Final molecules: $0 . 0289_{4} - x x$

$10 = 10.329 + \log \frac{0.0289}{0.320} = 61.6 mL$

Thus, the volume of nitric acid is $61.6 mL$

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(c) How many milliliters of $0.320 {MNHO}_{3}$ should be added to $4.00 g$ of to give a pH of $10.00$ in $250 mL$ ?

Short Answer

Step by step solution

Define the Henderson-Hasselbalch equation.

Step 2:Calculate the volume of nitric acid

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(c) How many milliliters of 0.320MNHO3should be added to 4.00gof to give a pH of10.00 in 250mL?

Short Answer

Step by step solution

Define the Henderson-Hasselbalch equation.

Step 2:Calculate the volume of nitric acid

One App. One Place for Learning.

Most popular questions from this chapter

Recommended explanations on Chemistry Textbooks

Ionic and Molecular Compounds

Nuclear Chemistry

Kinetics

Organic Chemistry

Chemistry Branches

Chemical Analysis

Study anywhere. Anytime. Across all devices.

(c) How many milliliters of $0.320 {MNHO}_{3}$ should be added to $4.00 g$ of to give a pH of $10.00$ in $250 mL$ ?