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3 years ago

What is the pH of a 0.65 M solution of pyridine, C5H5N?

Chemistry

1 answer:

Arada [10]3 years ago

3 0

Hey there!

The pH of a weak base (in this case, pyridine is a weak base) is calculated by using the weak base equation, and then solving it.

C5H5N; Kb= 1.7 x 10⁻⁹

pH = -log [H⁺]

we can also say that pH = 14 + log [OH⁻]

Plugging into the weak base equation, we know that Kb = [OH⁻][BH⁺] / [B]

This can be solved using an ice chart, which will then simplify to :

Kb = [x][x] / [0.50-x]

We can assume that x is very small in comparison to the 0.5 , so we consider it zero.

Then plug in and solve for x. 1.79 *10-9 = x² / 0.5

x = 2.992 * 10⁻⁵

ince X is equal to the [OH⁻] concentration, we can plug it into the second pH equation, and get the pH!

pH = 14+ log 2.99 * 10⁻⁵

pH = 9.48

Hope that helps!

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mel-nik [20]

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Eva8 [605]

<span>Data:
pH = 5.2
[H+] = ?

Knowing that: (</span><span>Equation to find the pH of a solution)</span>
$pH = -log[H+]$
<span>
Solving:
</span> $pH = -log[H+]$
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Knowing that the exponential is the opposite operation of the logarithm, then we have:
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$\boxed{\boxed{[H+] = 6.30*10^{-6}}}\end{array}}\qquad\quad\checkmark$

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