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Chapter 15: Problem 55

If a solution has a hydronium ion concentration of \(6.7 \times 10^{-1} \mathrm{M},\) what is its pH?

Short Answer

Expert verified
The pH of the solution is 0.17.

Step by step solution

01

Understanding pH

pH is a measure of the acidity or alkalinity of a solution. It's calculated as the negative logarithm (base 10) of the hydronium ion concentration, expressed in moles per liter. The formula is \( pH = -\log[H_3O^+]\) where \(H_3O^+\) is the concentration of hydronium ions.
02

Inserting given values into the formula

Given that the hydronium ion concentration in the exercise is \(6.7 \times 10^{-1} M\), insert it into the formula: \(pH = -\log(6.7 \times 10^{-1})\).
03

Calculating pH

Using a calculator, figure out the logarithm of \(6.7 \times 10^{-1}\) which comes out to be around -0.17. But because of the negative sign in the formula, the pH equals positive 0.17.

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Most popular questions from this chapter

Find \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) in a solution of \(\mathrm{pH} 4\).

What volume of 0.100 \(\mathrm{M} \mathrm{NaOH}\) is required to neutralize 25.00 \(\mathrm{mL}\) of 0.150 \(\mathrm{M} \mathrm{HCl}\) ?

Describe two precautions that should be taken to ensure an accurate titration.

The pH of a solution is \(9.5 .\) What is \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) ? What is \(\left[\mathrm{OH}^{-}\right] ?\)

If a solution has a pH of 13.3, what is its hydronium ion concentration?
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