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Chapter 10: Q. 10.25 (page 340)

10.25 Why are the concentrations of $H_{3} O^{+}$ and ${OH}^{-}$ equal in pure water?

Short Answer

Expert verified

In pure water, $[H_{3} O^{+}] = [{OH}^{-}]$ because in pure water, the transfer of a proton between two water molecules produces equal numbers of $H_{3} O^{+}$ and ${OH}^{-}$

Step by step solution

01

Introduction

The given are the two equations $H_{3} O^{-}$ and $O H^{-}$ . To find how both are equal in pure water?

02

Explanation

In pure water, $[H_{3} O^{+}] = [{OH}^{-}]$ because in pure water, the transfer of a proton between two water molecules produces equal numbers of $H_{3} O^{+}$ and $O H^{-}$

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Most popular questions from this chapter

Identify each of the solutions in problem 10.87 as acidic, basic, or neutral.

Calculate the $pH$ of each solution given the following:

a. localid="1654581866672" $[H_{3} O^{+}] = 1 \times 10^{- 8} M$

b. localid="1654581885926" $|H_{3} O^{+}| = 5 \times 10^{- 6} M$

c. localid="1654581933543" $[{OH}^{-}] = 1 \times 10^{- 2} M$

d. localid="1654581908454" $[{OH}^{-}] = 8.0 \times 10^{- 1} M$

e.localid="1654581942428" $[H_{3} O^{+}] = 4.7 \times 10^{- 2} M$

f. localid="1654581956589" $[{OH}^{-}] = 3.9 \times 10^{- 6} M$

Calculate the $[H_{3} O^{+}] and [{OH}^{-}]$ for a solution with the following pH values:

a. 3.40

b. 6.00

c. 8.0

d. 11.0

e. 9.20

Name each of the following acids or bases:

a. $Hcl$

b. $Ca {(OH)}_{2}$

c. ${HclO}_{4}$

d. ${HNO}_{3}$

e. $H_{2} {SO}_{3}$

f. ${HBrO}_{2}$

A buffer solution is made by dissolving $H_{3} {PO}_{4} and {NaH}_{2} {PO}_{4}$ in water.

a. Write an equation that shows how this buffer neutralizes added acid.

b. Write an equation that shows how this buffer neutralizes added base.

See all solutions

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