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Chapter 15: Problem 69

The pH of a solution is \(3.0 .\) What is \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right] ?\)

Short Answer

Expert verified
The hydronium ion concentration [\(\mathrm{H}_{3}\mathrm{O}^{+}\)] in a solution with a pH of 3.0 is 0.001 M or 1 x 10-3 moles per liter.

Step by step solution

01

Understand the formula

The formula used for these conversions is pH = -log([\(\mathrm{H}_{3}\mathrm{O}^{+}\)]). The pH stands for 'potential hydrogen' and refers to the acid concentration in a solution, represented by [\(\mathrm{H}_{3}\mathrm{O}^{+}\)]. The formula shows that as the pH value decreases, the concentration of the acid increases. It is important to remember that the pH value given is on a logarithmic scale, not linear.
02

Rearrange the formula

To find [\(\mathrm{H}_{3}\mathrm{O}^{+}\)], the formula should be rearranged as follows: [\(\mathrm{H}_{3}\mathrm{O}^{+}\)] = 10^{-pH}
03

Substitute pH value into the formula

Substitute the pH value into the rearranged formula to calculate the hydronium ion concentration. For this exercise, the solution's pH value is 3.0. Therefore, the calculation would be [\(\mathrm{H}_{3}\mathrm{O}^{+}\)] = 10^{-3.0}
04

Calculation and Result

When 10 is raised to the power of -3.0, the result is 0.001. Therefore, the concentration of hydronium ions [\(\mathrm{H}_{3}\mathrm{O}^{+}\)] in a solution with a pH of 3.0 is 0.001 M, or it can be stated as 1 x 10-3 moles per liter

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Most popular questions from this chapter

How does Bronsted and Lowry's definition of an acid differ from Arrhenius's definition of an acid? Explain which definition is broader.

The hydronium ion concentration in a 0.100 M solution of formic acid is 0.0043 \(\mathrm{M}\) . Calculate \(K_{a}\) for formic acid.

Write the equilibrium equation and the equilibrium constant expression for an ammonia-ammonium ion buffer solution.

What volume of 0.100 \(\mathrm{M} \mathrm{NaOH}\) is required to neutralize 25.00 \(\mathrm{mL}\) of 0.110 \(\mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4} ?\)

If 0.150 mol of \(\mathrm{KOH}\) is dissolved in 500 \(\mathrm{mL}\) of water, what are \(\left[\mathrm{OH}^{-}\right]\) and \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) ?
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