Chapter 6: Q4TY (page 132)

Find $[{OH}^{-}]$ iflocalid="1663407699090" $[H^{+}] = 1.0 \times 10^{- 4} M [H^{+}] = 1.0 \times 10^{- 4} M$

Short Answer

Expert verified

Thus, the value for $[{OH}^{-}]$ was calculated as $1.0 \times 10^{- 10} M$ .

Step by step solution

Define The formula for finding .

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

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

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

Step 2: Calculate the value for [OH-]

Given:

$[H^{+}] = 1.0 \times 10^{- 4} M$

Concentration of $[O H^{-}]$

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

Where,

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

$(K_{w})$ is the ionic product of water $(1.00 \times 10^{- 14})$

$(K_{w})$ is the acid dissociation constant.

$K_{w} = [H^{+}] \times [O H^{-}]$

$1.0 \times 10^{- 14} = 1.0 \times 10^{- 4} M \times [{OH}^{-}]$

$[O H^{-}] = 1.0 \times 10^{- 10} M$

Thus the value for was calculated as $1.0 \times 10^{- 10} M$

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Find $[{OH}^{-}]$ iflocalid="1663407699090" $[H^{+}] = 1.0 \times 10^{- 4} M [H^{+}] = 1.0 \times 10^{- 4} M$

Short Answer

Step by step solution

Define The formula for finding .

Step 2: Calculate the value for [OH-]

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Find [OH-]iflocalid="1663407699090" [H+]=1.0×10-4M[H+]=1.0×10-4M

Short Answer

Step by step solution

Define The formula for finding .

Step 2: Calculate the value for [OH-]

One App. One Place for Learning.

Most popular questions from this chapter

Recommended explanations on Chemistry Textbooks

Chemistry Branches

Chemical Reactions

Nuclear Chemistry

Physical Chemistry

Chemical Analysis

Inorganic Chemistry

Study anywhere. Anytime. Across all devices.

Find $[{OH}^{-}]$ iflocalid="1663407699090" $[H^{+}] = 1.0 \times 10^{- 4} M [H^{+}] = 1.0 \times 10^{- 4} M$