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Chapter 10: Q. 10.41 (page 346)

Complete the following table:

Short Answer

Expert verified

i) The pH value is greater than $7.0$ and is basic

ii) The ion value $[O H^{-}]$ is determined as $3.09 \times 10^{- 11} M$

iii) The pH value is lesser than $7$ and is acidic

Step by step solution

01

Introduction

The given is the table with components

The objective is to complete the table

02

Explanation

(i)

[O H -] = 1.0 \times 10^{- 6} M [H_{3} O^{+}] = [H_{3} O^{+}] = [H_{3} O^{+}] = 1.0 \times 10^{- 8} M p H = - \log [H_{3} O^{+}] p H = - \log [1.0 \times 10^{- 8}] = 8 p H > 7.0 s o, b a s i c

03

Explanation

(ii)

p H = 3.49 < 7.0 s o, A c i d i c [H_{3} O^{+}] = 10^{- p H} [H_{3} O^{+}] = 10^{- 3.49} = 3.236 \times 10^{- 4} M [O H^{-}] = [O H^{-}] = = 3.09 \times 10^{- 11} M

04

Explanation

(iii)

[H_{3} O^{+}] = 2.8 \times 10^{- 5} M [O H^{-}] = [O H^{-}] = [O H -] = 3.571 \times 10^{- 10} M p H = - \log [H_{3} O^{+}] p H = - \log [2.8 \times 10^{- 5}] = 4.55 p H < 7.0 s o, A c i d i c

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Most popular questions from this chapter

At rest, the $[H_{3} O^{+}]$ of the stomach fluid is $2.0 \times 10^{- 4} M$ . What is the $pH$ of the stomach fluid?

Which of the following are not at equilibrium?

a. The rates of the forward and reverse reactions are equal.

b. The rate of the forward reaction does not change.

c. The concentrations of reactants and the products are not constant.

Use Le Châtelier's principle to predict if each of the following changes causes the system to shift in the direction of products or reactants:

$HClO (a q) + H_{2} O (l) ⇄ H_{3} O^{+} (a q) + {ClO}^{-} (a q)$

a. removing some $HClO (a q)$

b. adding more ${ClO}^{-} (a q)$

c. removing some $H_{3} O^{+} (a q)$

d. adding more $HClO (a q)$

When food enters the stomach, $HCl$ is released and the $[H_{3} O^{+}]$ of the stomach fluid rises to $4 \times 10^{- 2} M$ . What is the $pH$ of the stomach fluid?

Why would the pH of your blood plasma increase if you breathe fast?

See all solutions

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