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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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.

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Buffer Solutions

A buffer solution is a system that resists changes in pH upon the addition of small amounts of acid or base. It typically consists of a weak acid and its conjugate base or a weak base and its conjugate acid. In this case, hydroxylamine acts as a weak base, while HCl provides the conjugate acid, allowing the solution to maintain a relatively stable pH.

Henderson-Hasselbalch Equation

The Henderson-Hasselbalch equation is a mathematical formula used to calculate the pH of a buffer solution. It is expressed as pH = pKa + log([A-]/[HA]), where pKa is the negative logarithm of the acid dissociation constant (Ka). For this problem, we need to determine the pKa of hydroxylamine from its Kb to find the pH of the buffer solution.

Dissociation Constants (Ka and Kb)

Dissociation constants are equilibrium constants that describe the extent to which an acid or base dissociates in solution. Kb is the base dissociation constant, while Ka is the acid dissociation constant. The relationship between Ka and Kb for a conjugate acid-base pair is given by the equation Kw = Ka × Kb, where Kw is the ion product of water. This relationship is essential for converting Kb to Ka when calculating pH.

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Ka and Kb Relationship

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