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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

01

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.

02

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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Most popular questions from this chapter

Identify the Lewis acids in the following reactions:

${BF}_{3} + {NH}_{3} ⇌ F_{3} B - \overset{+}{N} H_{3}$
$F^{-} + {AsF}_{5} ⇌ {AsF}_{6}^{-}$

The formation of tetrafluoroethylene from its elements is highly exothermic:

$\underset{Fluorine}{2 F_{2}} (g) + \underset{Graphite}{2 C (s)} ⇌ \underset{Tetrafluoroethylene}{F_{2} C = {CF}_{2} (g)}$

(a)If a mixture of $F_{2}$ graphite, and $C_{2} F_{4}$ is at equilibrium in a closed container, will the reaction go to the right or to the left if $F_{2}$ is added?

(b) Rare bacteria from the planet Teflon eat $C_{2} F_{4}$ and make Teflon for their cell walls. Will the reaction go to the right or to the left if these bacteria are added?

(c) Will the reaction go right or left if solid graphite is added? (Neglect any effect of increased pressure due to the decreased volume in the vessel when solid is added.)

(d) Will the reaction go right or left if the container is crushed to one-eighth of its original volume?

(e) Does the equilibrium constant become larger or smaller if the container is heated?

A solution contains $0.0500 {MCa}^{2 +}$ and $0.0300 {MAg}^{+}$ . Can 99%of ${Ca}^{2 +}$ be precipitated by sulphate without precipitating ${Ag}^{+}$ ? What will be the concentration of ${Ca}^{2 +}$ when ${Ag}_{2} {SO}_{4}$ begins to precipitate?

Given the following equilibria, calculate the concentration of

each zinc species in a solution saturated with $Zn {(OH)}_{2} (s)$ and containing $[{OH}^{-}]$

at a fixed concentration of $3.2 \times 10^{27} M$ .

$Zn {(OH)}_{2} (s) Ksp = 3 \times 10^{- 16} Zn {(OH)}^{+} β_{1} = 1 \times 10^{4} Zn {(OH)}_{2} (aq) β_{2} = 2 \times 10^{10} Zn {(OH)}_{3}^{-} β_{3} = 8 \times 10^{13} Zn {(OH)}_{4}^{2 -} β_{3} = 3 \times 10^{15}$

For $H_{2} (g) + B r_{2} (g) ⇌ 2 H B r (g), K = 7.2 \times 10^{- 4}$ at 1362Kand $∆ H^{°}$ is positive. A vessel is charged with $48.0 Pa H Br, 1370 Pa H_{2}$ , and $3310 Pa {Br}_{2}$ at1362K.

(a) Will the reaction proceed to the left or the right to reach equilibrium?

(b) Calculate the pressure (Pa) of each species at equilibrium.

(c) If the mixture at equilibrium is compressed to half of its original volume, will the reaction proceed to the left or the right to re-establish equilibrium?

(d) If the mixture at equilibrium is heated from 1362 to 1407K , will HBr be formed or consumed in order to re-establish equilibrium?

See all solutions

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