What is the hydronium ion concentration, [H₃O⁺], of an aqueous 0.083 M hydroxylamine, HONH₂, solution?
Hydroxylamine is a basic substance when dissolved in water. K _b(HONH₂) = 1.1×10^{- 8}

Question

What is the hydronium ion concentration, [H₃O⁺], of an aqueous 0.083 M hydroxylamine, HONH₂, solution? Hydroxylamine is a basic substance when dissolved in water. K _b(HONH₂) = 1.1×10^{- 8}

Quizplus · Accepted Answer

First, we need to write out the chemical equation for the dissociation of HONH₂ in water: HONH₂ + H2O ⇌ H₃O⁺ + OH- Using the given equilibrium constant, we can set up an ICE table: I: HONH₂ H2O no products initially C: -x -x +x +x E: 0.083 M - x (55.5 - x) x 1.1×10^{- 8} Note that we assume x is small compared to both the initial concentration of HONH₂ and the auto-ionization of water (which is why we can ignore x when calculating the concentration of OH-). Now use the equilibrium constant expression to solve for x: K _b = [H₃O⁺][OH-] / [HONH₂] 1.1×10^{- 8} = (x)(1.1×10^{- 14} - x) / (0.083 - x) Assuming x is small, we can simplify: 1.1×10^{- 8} = (x)(1.1×10^{- 14}) / (0.083) Solving for x gives: x = 3.3×10^{- 10} M This is the concentration of OH-, so the concentration of H3O+ (or [H₃O⁺]) will be: [H₃O⁺] = 1.0×10^{- 14} / 3.3×10^{- 10} [H₃O⁺] = 3.0×10^{- 5} M Therefore, the answer is (C).

What Is the Hydronium Ion Concentration, [H3O+], of an Aqueous

What Is the Hydronium Ion Concentration, [H₃O⁺], of an Aqueous