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Chapter 15: Problem 156

The pH of a solution is \(-1\). What are the \(\mathrm{H}_{3} \mathrm{O}^{+}\) and OH concentrations? Is the solution acidic or basic?

Short Answer

Expert verified
Given the pH of -1, the concentration of H₃O⁺ ions can be calculated as \( [H_{3}O^+] = 10^{-(-1)} = 10 \) moles/L. Using the ion product of water, the concentration of OH⁻ ions is found to be \( [OH^-] = \frac{1 \times 10^{-14}}{10} = 1 \times 10^{-15} \) moles/L. Since the H₃O⁺ concentration is greater than the OH⁻ concentration, the solution is acidic.

Step by step solution

01

Recall the definition of pH

The pH of a solution is defined as the negative logarithm of the H₃O⁺ concentration: \( pH = -\log{[H_{3}O^+]} \) where [H₃O⁺] represents the concentration of hydronium ions in the solution,
02

Calculate the H₃O⁺ concentration

Given the pH value of -1, we can rearrange the formula to find the H₃O⁺ concentration: \[ [H_{3}O^+] = 10^{-pH} \] Substitute pH value and compute the concentration: \[ [H_{3}O^+] = 10^{-(-1)} = 10 \] So, the concentration of H₃O⁺ in the solution is 10 moles/L.
03

Recall the relationship between H₃O⁺ and OH⁻ concentrations

The relationship between H₃O⁺ and OH⁻ concentrations can be described using the ion product of water (Kw): \[ K_w = [H_{3}O^+][OH^-] \] For pure water at 25°C, Kw value is 1 x 10⁻¹⁴.
04

Calculate the OH⁻ concentration

Using the Kw value and the calculated H₃O⁺ concentration, find the concentration of OH⁻ ions: \[ [OH^-] = \frac{K_w}{[H_{3}O^+]} \] Substitute the values and compute the concentration: \[ [OH^-] = \frac{1 \times 10^{-14}}{10} = 1 \times 10^{-15} \] So, the concentration of OH⁻ ions in the solution is 1 x 10⁻¹⁵ moles/L.
05

Determine if the solution is acidic or basic

A solution is considered acidic if the H₃O⁺ concentration is greater than the OH⁻ concentration, and it's considered basic if the OH⁻ concentration is greater than the H₃O⁺ concentration. Since the H₃O⁺ concentration (10 moles/L) is greater than the OH⁻ concentration (1 x 10⁻¹⁵ moles/L), the solution is acidic.

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Most popular questions from this chapter

Without using a calculator, what is the base- 10 logarithm of \(10^{0}\) ? Of 1?

Is it possible to obtain water at \(25{ }^{\circ} \mathrm{C}\) that contains absolutely no ions of any sort? Explain.

When a strong acid is added to a buffer, the \(\mathrm{pH}\) changes a little bit. (a) Does the pH increase or decrease? (b) Why does the \(\mathrm{pH}\) change at all? Why doesn't the buffer hold the \(\mathrm{pH}\) constant?

Citric acid, \(\mathrm{H}_{3} \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{O}_{7}\), is a weak triprotic acid. Write equations for the three equilibrium reactions that occur during the stepwise dissociation of citric acid in water.

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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