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Chapter 16: Problem 74

Calculate the \(\mathrm{pH}\) of a \(0.42 \mathrm{M} \mathrm{NH}_{4} \mathrm{Cl}\) solution.

Short Answer

Expert verified
The \(\mathrm{pH}\) of the \(0.42 \mathrm{M} \mathrm{NH}_{4} \mathrm{Cl}\) solution is approximately 0.38

Step by step solution

01

Determine the dissociation of \(\mathrm{NH}_{4} \mathrm{Cl}\)

When \(\mathrm{NH}_{4} \mathrm{Cl}\) dissolves in water, it dissociates into \(\mathrm{NH}_{4}^{+}\) and \(\mathrm{Cl}^{-}\). The \(\mathrm{NH}_{4}^{+}\) ions will behave as an acid and react with water to form \(\mathrm{NH}_{3}\) and \( H_{3}O^{+}\). Write the equation for this reaction as: \(\mathrm{NH}_{4}^{+} + H_{2}O \rightarrow \mathrm{NH}_{3} + H_{3}O^{+}\)
02

Calculate the concentration of \(\mathrm{NH}_{4}^{+}\) and \( H_{3}O^{+}\)

The concentration of \(\mathrm{NH}_{4}^{+}\) is equal to the initial molarity of the \(\mathrm{NH}_{4} \mathrm{Cl}\), 0.42 M. In the reaction, one mole of \(\mathrm{NH}_{4}^{+}\) produces one mole of \( H_{3}O^{+}\), so the concentration of \( H_{3}O^{+}\) is also 0.42 M.
03

Calculate the \(\mathrm{pH}\)

The \(\mathrm{pH}\) of the solution can be calculated using the \(\mathrm{pH}\) formula: \(\mathrm{pH} = -\log[H^{+}]\). Substitute the concentration of \( H_{3}O^{+}\) into the \(\mathrm{pH}\) formula to calculate the \(\mathrm{pH}\) of the solution: \(\mathrm{pH} = -\log(0.42)\).

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Most popular questions from this chapter

Explain the action of smelling salt, which is ammonium carbonate \(\left[\left(\mathrm{NH}_{4}\right)_{2} \mathrm{CO}_{3}\right]\). (Hint: The thin film of aqueous solution that lines the nasal passage is slightly basic.)

The pH of a \(0.30 M\) solution of a weak base is 10.66 . What is the \(K_{\mathrm{b}}\) of the base?

Write all the species (except water) that are present in a phosphoric acid solution. Indicate which species can act as a Bronsted acid, which as a Bronsted base, and which as both a Bronsted acid and a Bronsted base.

Calculate the hydrogen ion concentration in moles per liter for each of these solutions: (a) a solution whose \(\mathrm{pH}\) is \(5.20,\) (b) a solution whose \(\mathrm{pH}\) is 16.00 ; (c) a solution whose hydroxide concentration is \(3.7 \times 10^{-9} M\).

How many milliliters of a strong monoprotic acid solution at \(\mathrm{pH}=4.12\) must be added to \(528 \mathrm{~mL}\) of the same acid solution at \(\mathrm{pH}=5.76\) to change its \(\mathrm{pH}\) to \(5.34 ?\) Assume that the volumes are additive.
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