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Chapter 14: Problem 126

Are solutions of the following salts acidic, basic, or neutral? For those that are not neutral, write balanced equations for the reactions causing the solution to be acidic or basic. The relevant \(K_{\mathrm{a}}\) and \(K_{\mathrm{b}}\) values are found in Tables \(14.2\) and \(14.3 .\) a. \(\mathrm{KCl}\) c. \(\mathrm{CH}_{3} \mathrm{NH}_{3} \mathrm{Cl}\) e. \(\mathrm{NH}_{4} \mathrm{~F}\) b. \(\mathrm{NH}_{4} \mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\) d. \(\mathrm{KF}\) f. \(\mathrm{CH}_{3} \mathrm{NH}_{3} \mathrm{CN}\)

Short Answer

Expert verified
The solutions of the given salts are as follows: a. KCl: Neutral c. CH₃NH₃Cl: Acidic (CH₃NH₃⁺(aq) + H₂O(l) ⇌ CH₃NH₂(aq) + H₃O⁺(aq)) e. NH₄F: Slightly basic (F⁻(aq) + H₂O(l) ⇌ HF(aq) + OH⁻(aq)) b. NH₄C₂H₃O₂: Neutral d. KF: Basic (F⁻(aq) + H₂O(l) ⇌ HF(aq) + OH⁻(aq)) f. CH₃NH₃CN: Slightly basic (CN⁻(aq) + H₂O(l) ⇌ HCN(aq) + OH⁻(aq))

Step by step solution

01

Identify the ions in the salts

We must first identify the cations and anions in each salt. These ions may act as acids or bases when dissolved in water. a. KCl: K⁺ (cation) and Cl⁻ (anion) c. CH₃NH₃Cl: CH₃NH₃⁺ (cation) and Cl⁻ (anion) e. NH₄F: NH₄⁺ (cation) and F⁻ (anion) b. NH₄C₂H₃O₂: NH₄⁺ (cation) and C₂H₃O₂⁻ (anion) d. KF: K⁺ (cation) and F⁻ (anion) f. CH₃NH₃CN: CH₃NH₃⁺ (cation) and CN⁻ (anion)
02

Determine the acidic or basic properties of the ions

Now we need to examine the acidic or basic properties of the ions by checking their K_a and K_b values. Keep in mind that neither K⁺ nor Cl⁻ react with water, meaning their corresponding K_a and K_b values are negligible. a. KCl: K⁺ (no reaction) and Cl⁻ (no reaction) - Neutral c. CH₃NH₃Cl: CH₃NH₃⁺ (K_a = 2.3 x 10⁻¹¹) and Cl⁻ (no reaction) e. NH₄F: NH₄⁺ (K_a = 5.6 x 10⁻¹⁰) and F⁻ (K_b = 1.4 x 10⁻¹¹) b. NH₄C₂H₃O₂: NH₄⁺ (K_a = 5.6 x 10⁻¹⁰) and C₂H₃O₂⁻ (K_b = 5.3 x 10⁻¹⁰) d. KF: K⁺ (no reaction) and F⁻ (K_b = 1.4 x 10⁻¹¹) f. CH₃NH₃CN: CH₃NH₃⁺ (K_a = 2.3 x 10⁻¹¹) and CN⁻ (K_b = 2.0 x 10⁻⁵)
03

Determine if the solution is acidic, basic, or neutral and write balanced equations where needed

a. KCl: Neutral - No reaction with water c. CH₃NH₃Cl: Acidic Reaction: CH₃NH₃⁺(aq) + H₂O(l) ⇌ CH₃NH₂(aq) + H₃O⁺(aq) e. NH₄F: Slightly basic due to the higher K_b value of F⁻ compared to the K_a value of NH₄⁺ Reaction: F⁻(aq) + H₂O(l) ⇌ HF(aq) + OH⁻(aq) b. NH₄C₂H₃O₂: Neutral - NH₄⁺ and C₂H₃O₂⁻ have similar acidity and basicity, so their effects cancel each other out. d. KF: Basic Reaction: F⁻(aq) + H₂O(l) ⇌ HF(aq) + OH⁻(aq) f. CH₃NH₃CN: Slightly basic due to the higher K_b value of CN⁻ compared to the K_a value of CH₃NH₃⁺ Reaction: CN⁻(aq) + H₂O(l) ⇌ HCN(aq) + OH⁻(aq)

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Most popular questions from this chapter

Acrylic acid \(\left(\mathrm{CH}_{2}=\mathrm{CHCO}_{2} \mathrm{H}\right)\) is a precursor for many important plastics. \(K_{\mathrm{a}}\) for acrylic acid is \(5.6 \times 10^{-5}\). a. Calculate the \(\mathrm{pH}\) of a \(0.10 \mathrm{M}\) solution of acrylic acid. b. Calculate the percent dissociation of a \(0.10 \mathrm{M}\) solution of acrylic acid. c. Calculate the \(\mathrm{pH}\) of a \(0.050 \mathrm{M}\) solution of sodium acrylate \(\left(\mathrm{NaC}_{3} \mathrm{H}_{3} \mathrm{O}_{2}\right)\)

Calculate the \(\mathrm{pH}\) of a \(0.20 \mathrm{MC}_{2} \mathrm{H}_{5} \mathrm{NH}_{2}\) solution \(\left(K_{\mathrm{b}}=5.6 \times 10^{-4}\right)\).

A solution is prepared by adding \(50.0 \mathrm{~mL}\) concentrated hydrochloric acid and \(20.0 \mathrm{~mL}\) concentrated nitric acid to \(300 \mathrm{~mL}\) water. More water is added until the final volume is \(1.00 \mathrm{~L}\). Calculate \(\left[\mathrm{H}^{+}\right],\left[\mathrm{OH}^{-}\right]\), and the \(\mathrm{pH}\) for this solution. [Hint: Concentrated HCl is \(38 \%\) HCl (by mass) and has a density of \(1.19\) \(\mathrm{g} / \mathrm{mL} ;\) concentrated \(\mathrm{HNO}_{3}\) is \(70 . \% \mathrm{HNO}_{3}\) (by mass) and has a density of \(1.42 \mathrm{~g} / \mathrm{mL} .\) ]

What are the major species present in the following mixtures of bases? a. \(0.050 \mathrm{M} \mathrm{NaOH}\) and \(0.050 \mathrm{M} \mathrm{LiOH}\) b. \(0.0010 \mathrm{M} \mathrm{Ca}(\mathrm{OH})_{2}\) and \(0.020 \mathrm{M} \mathrm{RbOH}\) What is \(\left[\mathrm{OH}^{-}\right]\) and the \(\mathrm{pH}\) of each of these solutions?

A solution is made by adding \(50.0 \mathrm{~mL}\) of \(0.200 \mathrm{M}\) acetic acid \(\left(K_{\mathrm{a}}=1.8 \times 10^{-5}\right)\) to \(50.0 \mathrm{~mL}\) of \(1.00 \times 10^{-3} \mathrm{M} \mathrm{HCl}\) a. Calculate the \(\mathrm{pH}\) of the solution. b. Calculate the acetate ion concentration.
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