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Chapter 15: Problem 150

What is the \(\mathrm{pH}\) of a solution whose \(\mathrm{OH}^{-}\) concentration is \(10^{-14} \mathrm{M} ?\) Is the solution acidic or basic?

Short Answer

Expert verified
The pH of the solution with an OH⁻ concentration of \(10^{-14}\) M is 0. The solution is acidic.

Step by step solution

01

Given concentration of OH⁻ ions

The given concentration of OH⁻ ions in the solution is \(10^{-14}\) M (Molar).
02

Use the ionic product of water

The ionic product of water, \(K_w\), relates the concentration of both H₃O⁺ and OH⁻ ions in the solution. According to the ionic product of water: \[K_w = [\mathrm{H}^+] [\mathrm{OH}^-]\] Where \(K_w\) is the ionic product of water (equals to \(1 \times 10^{-14}\)), \([\mathrm{H}^{+}]\) is the concentration of H⁺ ions and \([\mathrm{OH}^{-}]\) is the concentration of OH⁻ ions.
03

Calculate the concentration of H⁺ ions

Since we know the concentration of OH⁻ ions and the value of \(K_w\), we can now calculate the concentration of H⁺ ions using the ionic product equation: \[1 \times 10^{-14} = [\mathrm{H}^+] (10^{-14})\] \[[\mathrm{H}^+] = \frac{1 \times 10^{-14}}{10^{-14}}\]
04

Find the concentration of H⁺ ions

By solving for the concentration of H⁺ ions, we get: \[[\mathrm{H}^+] = \frac{1 \times 10^{-14}}{10^{-14}} = 1\]
05

Calculate the pH value

Now, we can calculate the pH value of the solution: \[\mathrm{pH} = -\log_{10}[\mathrm{H}^+]\] \[\mathrm{pH} = -\log_{10}(1)\]
06

Find the pH value

By solving for the pH value, we get: \[\mathrm{pH} = -\log_{10}(1) = 0\]
07

Determine if the solution is acidic or basic

A solution with a pH value less than 7 is acidic, pH equal to 7 is neutral, and pH greater than 7 is basic. Since the pH value found is 0, the solution is acidic. To summarize, the pH of the solution is 0, and the solution is acidic.

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Most popular questions from this chapter

Acrylic acid, \(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{COOH}\), is a weak monoprotic acid. Write a balanced equation for the reaction that occurs when \(25.0 \mathrm{~mL}\) of \(0.200 \mathrm{M} \mathrm{KOH}\) is added to \(50.0 \mathrm{~mL}\) of \(0.200 \mathrm{M} \mathrm{C}_{2} \mathrm{H}_{3} \mathrm{COOH}\). Besides water, what species are present in the solution? Is this solution a buffer? Why or why not?

It is possible to make two completely different buffers using the dihydrogen phosphate ion, \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}\) (a) In one buffer, \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}\) serves as the weak acid. What is the conjugate weak base? (b) Write the equations that show how the buffer in part (a) works when either \(\mathrm{H}_{3} \mathrm{O}^{+}\) or \(\mathrm{OH}^{-}\) is added. (c) In the other buffer, \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}\) serves as the weak base. What is the conjugate weak acid? (d) Write the equations that show how the buffer in part (c) works when either \(\mathrm{H}_{3} \mathrm{O}^{+}\) or \(\mathrm{OH}^{-}\) is added.

Without using a calculator, what is the base-10 logarithm of \(10^{13}\) ?

What is the molar hydroxide ion concentration in a solution that is 1000 times more acidic than a solution that has a pH of \(9.20\) ?

Acetic acid is a weak acid. Upon losing a proton, acetic acid yields the acetate anion. (a) Draw a dot diagram for the acetate anion. (b) Hydrogen atoms that are bound to carbon atoms are not acidic. Knowing this, is it possible for the acetate anion to serve as an acid? Explain. (c) In fact, acetate ion is a weak base. Write a chemical equilibrium with unequal-length arrows showing how acetate in water produces a weakly basic solution. (d) Is water acting as an acid or a base? Explain.
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