Chapter 10: Q.10.87 (page 359)

Determine the pH for the following solutions:
a. $[H_{3} O^{+}] = 1.0 \times 10^{- 11} M$
b. $[H_{3} O^{+}] = 5.0 \times 10^{- 2} M$
c. $[{OH}^{-}] = 3.5 \times 10^{- 4} M$
d. $[{OH}^{-}] = 0.005 M$

Short Answer

Expert verified

Part a. $11$

Part b. $1.3$

Part c. $10.5$

Part d. $11.7$

Step by step solution

Given Information (Part a)

The representation of a chemical reaction in the type of substance is known as a chemical equation. The equation in which the quantity of particles of the multitude of atoms is equivalent on the two sides of the equation is known as a fair chemical equation.

Explanation Part (a)

We know,

$[H_{3} O^{+}] = 1.0 \times 10^{- 11} M$

Using,

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

$pH = - \log (1.0 \times 10^{- 11}) = 11$

Explanation Part (b)

We know,

$[H_{3} O^{+}] = 5.0 \times 10^{- 2} M$

Using,

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

$pH = - \log (5.0 \times 10^{- 2}) = 1.30$

Explanation Part (c)

We know,

$[{OH}^{-}] = 3.5 \times 10^{- 4} M$

Calculating $H_{3} O^{+}$ ,

role="math" localid="1653141748429" $[H_{3} O^{+}] = \frac{1 \times 10^{- 14}}{[{OH}^{-}]} = \frac{1 \times 10^{- 14}}{3.5 \times 10^{- 4}} = 2.85 \times 10^{- 11}$

Using,

$pH = - \log [H_{3} O^{+}] p H = - \log (2.85 \times 10^{- 11}) p H = 10.5$

Explanation Part (d)

We know,

$[{OH}^{-}] = 0.005 M$

Calculating $H_{3} O^{+}$

$[H_{3} O^{+}] = \frac{1 \times 10^{- 14}}{[{OH}^{-}]} = \frac{1 \times 10^{- 14}}{0.005} = 2 \times 10^{- 12}$

Using,

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

$pH = - \log (2.0 \times 10^{- 12}) p H = 11.7$

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Determine the pH for the following solutions:
a. $[H_{3} O^{+}] = 1.0 \times 10^{- 11} M$
b. $[H_{3} O^{+}] = 5.0 \times 10^{- 2} M$
c. $[{OH}^{-}] = 3.5 \times 10^{- 4} M$
d. $[{OH}^{-}] = 0.005 M$

Short Answer

Step by step solution

Given Information (Part a)

Explanation Part (a)

Explanation Part (b)

Explanation Part (c)

Explanation Part (d)

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Determine the pH for the following solutions:a. H3O+=1.0×10−11Mb. H3O+=5.0×10−2Mc. OH−=3.5×10−4Md.OH−=0.005M

Short Answer

Step by step solution

Given Information (Part a)

Explanation Part (a)

Explanation Part (b)

Explanation Part (c)

Explanation Part (d)

One App. One Place for Learning.

Most popular questions from this chapter

Recommended explanations on Chemistry Textbooks

Nuclear Chemistry

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The Earths Atmosphere

Study anywhere. Anytime. Across all devices.

Determine the pH for the following solutions:
a. $[H_{3} O^{+}] = 1.0 \times 10^{- 11} M$
b. $[H_{3} O^{+}] = 5.0 \times 10^{- 2} M$
c. $[{OH}^{-}] = 3.5 \times 10^{- 4} M$
d. $[{OH}^{-}] = 0.005 M$