When dissolved in water,hydrogen bromide (HBr) forms hydrobromic acid.Determine the hydroxide ion concentration in a 4,500 mL solution containing 3.78 g hydrogen bromide;K = 1.00 * 10¯¹⁴. A)[OH¯] = 9.63 * 10^-13 M B)[OH¯] = 2.14 *10^-13 M C)[OH¯] = 4.67 *10 10_-2 M D)[OH¯] = 0.0104 M

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Quizplus · Accepted Answer

Hydrogen bromide (HBr) is a strong acid, which dissociates completely in water. First, calculate the molarity of HBr: Molar mass of HBr = 80.91 g/mol. Moles of HBr = 3.78 g / 80.91 g/mol = 0.0467 mol. Volume = 4.5 L, so [H⁺] = 0.0467 mol / 4.5 L = 0.0104 M. Using the ion product of water, Kw = [H⁺][OH⁻] = 1.00 * 10⁻¹⁴, solve for [OH⁻]: [OH⁻] = Kw / [H⁺] = 1.00 * 10⁻¹⁴ / 0.0104 = 9.63 * 10⁻¹³ M.

When Dissolved in Water,hydrogen Bromide (HBr) Forms Hydrobromic Acid