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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 $3.09 脳 10^{- 11} M$

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 脳 10^{- 6} M [H_{3} O^{+}] = [H_{3} O^{+}] = [H_{3} O^{+}] = 1.0 脳 10^{- 8} M p H = - \log [H_{3} O^{+}] p H = - \log [1.0 脳 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 脳 10^{- 4} M [O H^{-}] = [O H^{-}] = = 3.09 脳 10^{- 11} M

04

Explanation

(iii)

[H_{3} O^{+}] = 2.8 脳 10^{- 5} M [O H^{-}] = [O H^{-}] = [O H -] = 3.571 脳 10^{- 10} M p H = - \log [H_{3} O^{+}] p H = - \log [2.8 脳 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

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

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

$HClO (a q) + H_{2} O (l) 鈬� H_{3} O^{+} (a q) + {ClO}^{鈭�} (a q)$

a. removing some $HClO (a q)$

b. adding more ${ClO}^{鈭�} (a q)$

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

d. adding more $HClO (a q)$

Identify the Bronsted-Lowry acid-base pairs in each of the following equations:

a. $H_{3} {PO}_{4} (a q) + H_{2} O (l) 鈬� H_{2} {PO}_{4}^{-} (a q) + H_{3} O^{+} (a q)$

b.localid="1652710222540" ${CO}_{3} {}^{2 -}(a q) + H_{2} O (l) 鈬� {HCO}_{3}^{-} (a q) + {OH}^{-} (a q)$

c.localid="1652710226359" $H_{3} {PO}_{4} (a q) + {NH}_{3} (a q) 鈬� H_{2} {PO}_{4}^{-} (a q) + {NH}_{4}^{+} (a q)$

Identify the reactant that is a Br酶nsted-Lowry acid and the reactant that is a Br酶nsted-Lowry base in each of the following:

a. ${CO}_{3} {}^{2 -}(a q) + H_{2} O (l) 鈬� {HCO}_{3} {}^{-}(a q) + {OH}^{-} (a q)$

b. $H_{2} {SO}_{4} (a q) + H_{2} O (l) 鉄� {HSO}_{4}^{-} (a q) + H_{3} O^{+} (a q)$

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

$H_{2} S (a q) + H_{2} O (l) 鈬� H_{3} O^{+} (a q) + {HS}^{鈭�} (a q)$

a. adding more $H_{2} S (a q)$

b. removing some ${HS}^{鈭�} (a q)$

c. adding more $H_{3} O^{+} (a q)$

d. removing some $H_{2} S (a q)$

See all solutions

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