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3 years ago

BONUS QUESTION

Chemistry

1 answer:

devlian [24]3 years ago

6 0

Answer:

pH = 12.5

Explanation:

The reaction that takes place is

2OH⁻(aq) + Pb⁺²(aq) → Pb(OH)₂(s)

The OH⁻ species come from the metal hydroxide of the solution, and Pb(OH)₂ is the precipitate.

Now we convert 3.81 grams of Pb(OH)₂ into moles, using its molar mass:

3.81 g ÷ 241.12 g/mol = 0.0158 mol Pb(OH)₂

Now we convert 0.0158 Pb(OH)₂ moles into OH⁻ moles, using the stoichiometric coefficients of the reaction:

0.0158 mol Pb(OH)₂ * $\frac{2molOH^-}{1molPb(OH)_2}$ = 0.0316 mol OH⁻

With the given concentration (1 L), we calculate [OH⁻]:

[OH⁻] = 0.0316 mol / 1 L = 0.0316 M

Then we calculate the pOH of the solution:

pOH = - log[OH⁻] = 1.5

And finally we calculate the pH:

pH = 14 - pOH

pH = 12.5

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yawa3891 [41]

Answer:

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