Chapter 6: Q6TY (page 138)

$K_{b}$ for dimethylamine is $5.9 \times 10^{- 4}$ . Find $K_{a}$ for dimethyl ammonium ion.

Short Answer

Expert verified

For the dimethylammonium ion, the value of $K_{a} is 1.7 \times 10^{- 11}$ .

Step by step solution

Step 1: Define the formula for calculation of Kb

The value of $K_{b}$ can be calculated as

$K_{b} = \frac{[{BH}^{+}] [OH]}{[B]}$

where $K_{b}$ is called the base dissociation constant.

The value of $K_{w}$ is calculated by the formula

$K_{w} = K_{a} \times K_{b}$

Calculate the value of Kb

It is given that the value of $K_{b}$ for dimethylamine is $5.9 \times 10^{- 4}$ .

$K_{a}$ for the dimethylammonium ion can be derived from

$K_{w} = K_{a} \times K_{b}$

where

$(K_{b})$ is base dissociation constant

$(K_{w})$ is ionic product of water , and

$(K_{a})$ is acid dissociation constant.

$K_{a} = \frac{K_{w}}{K_{b}}$

$\begin{array}{l} = \frac{10 \times 10^{a}}{5.9 \times 10} \\ = 0.169 \times 10^{- 10} \\ = 1.7 \times 10^{- 11} \end{array}$

Thus, for the dimethylammonium ion, $K_{a} is 1.7 \times 10^{- 11}$ .

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$K_{b}$ for dimethylamine is $5.9 \times 10^{- 4}$ . Find $K_{a}$ for dimethyl ammonium ion.

Short Answer

Step by step solution

Step 1: Define the formula for calculation of Kb

Calculate the value of Kb

One App. One Place for Learning.

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Kbfor dimethylamine is 5.9×10-4. Find Kafor dimethyl ammonium ion.

Short Answer

Step by step solution

Step 1: Define the formula for calculation of Kb

Calculate the value of Kb

One App. One Place for Learning.

Most popular questions from this chapter

Recommended explanations on Chemistry Textbooks

Ionic and Molecular Compounds

Chemical Analysis

Making Measurements

Physical Chemistry

Nuclear Chemistry

Inorganic Chemistry

Study anywhere. Anytime. Across all devices.

$K_{b}$ for dimethylamine is $5.9 \times 10^{- 4}$ . Find $K_{a}$ for dimethyl ammonium ion.