Respuesta :

N2H4 + H2O = N2H5(+) + OH(-) 

Kb = 1.3 E-06 = [N2H5(+)][OH(-)] / [N2H4] = [OH(-)]^2 / 0.1 

Thus [OH(-)] = 0.000361 

pOH = -log[OH(-)] = 3.44 

pH = 14 - pOH = 10.6

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dsdrajlin

A 0.10 M solution of hydrazine (Kb = 1.3 × 10⁻⁶) has a pH of 10.6.

What is pH?

pH is a figure expressing the acidity or alkalinity of a solution on a logarithmic scale.

We have a 0.10 M (Cb) solution of hydrazine, a weak base with a Kb of 1.3 × 10⁻⁶.

  • Step 1: Calculate the [OH⁻].

We will use the following expression.

[OH⁻] = √(Kb × Cb) = √(1.3 × 10⁻⁶ × 0.10) = 3.6 × 10⁻⁴ M

  • Step 2: Calculate the pOH.

We will use the definition of pOH.

pOH = -log [OH⁻] = -log 3.6 × 10⁻⁴ = 3.4

  • Step 3: Calculate the pH.

We will use the following expression.

pH + pOH = 14.0

pH = 14.0 - pOH = 14.0 - 3.4 = 10.6

A 0.10 M solution of hydrazine (Kb = 1.3 × 10⁻⁶) has a pH of 10.6.

Learn more about pH here: https://brainly.com/question/172153

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