Chapter 10: Q. 10.87 (page 359)

Determine the pH for the follow ing solutions: $(10, 6)$
a. $[OH] = 1.0 \times 10^{- 7} M$
b. $[H_{2} O^{'}] = 4.2 \times 10^{- 3} M$
c. $[H_{2} O^{+}] = 0.0001 M$
d. $[OH] = 8.5 \times 10^{- 9} M$

Short Answer

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Step by step solution

Step 1 Introduction

The $pH$ scale relates to the logarithmic scale. $[H_{3} O^{+}]$ of aqueous solutions.

Mathematically expression of $pH$ is the negative logarithmic of the $[H_{3} O^{+}]$

$K w = [H_{3} O^{+}] [{OH}^{-}]$

$pH = - \log [H_{3} O^{+}]$

$pOH = - \log [{OH}^{-}]$

Acidic solution $= pH < 7.0 [H_{3} O^{+}] > 1.0 \times 10^{- 7} M$

Neutral solution $= pH = 7.0 [H_{3} O^{+}] = 1.0 \times 10^{- 7} M$

Basic solution $= pH > 7.0 [H_{3} O^{+}] < 1.0 \times 10^{- 7} M$

Step 2 Explantion part (a)

Given acid concentration of the solution is $1.0 \times 10^{- 11} M$ . Calculate the $pH$ of the solution by using the following formula:

$p H = - \log [H_{3} O^{+}]$

$= - \log [1.0 \times 10^{- 11}]$

$= 11 - \log (1.0)$

$= 11$

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Determine the pH for the follow ing solutions: $(10, 6)$
a. $[OH] = 1.0 \times 10^{- 7} M$
b. $[H_{2} O^{'}] = 4.2 \times 10^{- 3} M$
c. $[H_{2} O^{+}] = 0.0001 M$
d. $[OH] = 8.5 \times 10^{- 9} M$

Short Answer

Step by step solution

Step 1 Introduction

Step 2 Explantion part (a)

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Determine the pH for the follow ing solutions:(10,6)a.[OH]=1.0×10-7Mb.H2O'=4.2×10-3Mc.H2O+=0.0001Md.[OH]=8.5×10-9M

Short Answer

Step by step solution

Step 1 Introduction

Step 2 Explantion part (a)

One App. One Place for Learning.

Most popular questions from this chapter

Recommended explanations on Chemistry Textbooks

Inorganic Chemistry

Nuclear Chemistry

Chemistry Branches

Chemical Analysis

Ionic and Molecular Compounds

Organic Chemistry

Study anywhere. Anytime. Across all devices.

Determine the pH for the follow ing solutions: $(10, 6)$
a. $[OH] = 1.0 \times 10^{- 7} M$
b. $[H_{2} O^{'}] = 4.2 \times 10^{- 3} M$
c. $[H_{2} O^{+}] = 0.0001 M$
d. $[OH] = 8.5 \times 10^{- 9} M$