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Ch.17 - Aqueous Ionic Equilibrium
All textbooksTro 4th EditionCh.17 - Aqueous Ionic EquilibriumProblem 131
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Chapter 17, Problem 131

The Kb of hydroxylamine, NH2OH, is 1.10 * 10^-8. A buffer solution is prepared by mixing 100.0 mL of a 0.36 M hydroxylamine solution with 50.0 mL of a 0.26 M HCl solution. Determine the pH of the resulting solution.

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1
Calculate the moles of hydroxylamine (NH2OH) using the formula: moles = concentration (M) * volume (L).
Calculate the moles of HCl using the formula: moles = concentration (M) * volume (L).
Determine the moles of NH2OH remaining after the reaction with HCl, considering the stoichiometry of the reaction: NH2OH + HCl -> NH3OH+ + Cl-.
Calculate the concentration of NH2OH and NH3OH+ in the final solution by dividing the moles of each by the total volume of the solution in liters.
Use the Henderson-Hasselbalch equation to find the pH: pH = pKa + log([base]/[acid]), where pKa = -log(Ka) and Ka = Kw/Kb.
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Open Question
What is the mass of sodium formate required to be dissolved in 250.0 cm³ of a 1.4 M formic acid solution to prepare a buffer solution with a pH of 3.36?