Chapter 6: Q38P (page 143)

The equilibrium constant for the reaction $H_{2} O ⇌ H^{+} + O H^{-}$ is $1.0 \times 10^{- 14}$ at $25 ° C$ . What is the value of K for the reaction $4 H_{2} O ⇌ 4 H^{+} + 4 O H^{-}$ ?

Short Answer

Expert verified

The value of the equilibrium constant is $1.0 \times 10^{- 56}$

Step by step solution

Definition of Equilibrium constant

In the equilibrium reaction, the equilibrium constant is given as the ratio of the concentration of the products to the concentration of the reactant.

The formula of the ionic product of water is:

$K_{W} = [H^{+}] [O H]$

Calculate the value of equilibrium constant

For the given reaction:

$4 H_{2} O ⇌ 4 H^{+} + 4 O H^{-}$

The equilibrium concentration is given by:

$K = \frac{[H^{+}] {[O H^{-}]}^{4}}{{[H_{2} O]}^{4}}$

Since undissociated water molecules are present in large concentrations, we can write:

role="math" localid="1663326848932" $K = {[H^{+}]}^{4} {[O H^{-}]}^{4} = {([H^{+}] [O H^{-}])}^{4} = {(K_{W})}^{4} = 1.0 \times 10^{- 56}$

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The equilibrium constant for the reaction $H_{2} O ⇌ H^{+} + O H^{-}$ is $1.0 \times 10^{- 14}$ at $25 ° C$ . What is the value of K for the reaction $4 H_{2} O ⇌ 4 H^{+} + 4 O H^{-}$ ?

Short Answer

Step by step solution

Definition of Equilibrium constant

Calculate the value of equilibrium constant

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The equilibrium constant for the reactionH2O⇌H++OH-is1.0×10-14 at25°C . What is the value of K for the reaction 4H2O⇌4H++4OH-?

Short Answer

Step by step solution

Definition of Equilibrium constant

Calculate the value of equilibrium constant

One App. One Place for Learning.

Most popular questions from this chapter

Recommended explanations on Chemistry Textbooks

Nuclear Chemistry

Chemical Reactions

The Earths Atmosphere

Kinetics

Chemistry Branches

Organic Chemistry

Study anywhere. Anytime. Across all devices.

The equilibrium constant for the reaction $H_{2} O ⇌ H^{+} + O H^{-}$ is $1.0 \times 10^{- 14}$ at $25 ° C$ . What is the value of K for the reaction $4 H_{2} O ⇌ 4 H^{+} + 4 O H^{-}$ ?