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Chapter 15: Problem 65

A solution has a pH of \(10.1 .\) Calculate the hydronium ion concentration and the hydroxide ion concentration.

Short Answer

Expert verified
[H+] is approximately \( 7.94 \times 10^{-11} \) M and [OH-] is approximately \( 1.26 \times 10^{-4} \) M.

Step by step solution

01

Calculate the Hydronium Ion Concentration

The formula to find the hydronium ion concentration [H+] from the pH is: \[ [H+] = 10^{-pH} \] By plugging the given pH of 10.1 in this formula, the hydronium ion concentration can be calculated.
02

Calculate the Hydroxide Ion Concentration

After determining the hydronium ion concentration, the hydroxide ion concentration [OH-] can be calculated using the dissociation constant of water (Kw). The formula is: \[ [OH-] = \frac{Kw}{[H+]} \] where \( Kw = 1.0 \times 10^{-14} \) at 25 degrees Celsius.
03

Perform the Calculations

First, calculate the hydronium ion concentration: \[ [H+] = 10^{-10.1} \] Then calculate the hydroxide ion concentration using the obtained [H+]: \[ [OH-] = \frac{1.0 \times 10^{-14}}{[H+]} \] Each of these calculations should provide the concentrations required.

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Most popular questions from this chapter

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

A 50 \(\mathrm{mL}\) sample of apple juice has a pH of \(3.2 .\) What amount, in moles, of \(\mathrm{H}_{3} \mathrm{O}^{+}\) is present?

What is a neutralization reaction?

An HNO \(_{3}\) solution has a pH of \(3.06 .\) What volume of 0.015 \(\mathrm{M}\) LiOH will be required to titrate 65.0 \(\mathrm{mL}\) of the HNO \(_{3}\) solution to reach the equivalence point?

If 50.00 \(\mathrm{mL}\) of 1.000 \(\mathrm{M} \mathrm{HI}\) is neutralized by 35.41 \(\mathrm{mL}\) of \(\mathrm{KOH}\) , what is the molarity of the \(\mathrm{KOH}\) solution?
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