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3 years ago

If you have a pH of 3.35, what is the hydrogen ion concentration of the solution?

Chemistry

1 answer:

melamori03 [73]3 years ago

3 0

Answer: 4.46 x 10^-4M

Explanation:

The pH of a solution is the concentration of hydrogen ion concentration in the solution. Mathematically, it is expressed as pH = -log(H+), where H+ is the concentration of hydrogen ion

On the pH scale, readings are from 1 to 14.

- pH values less than 7 are regarded as acidic. So, the solution with pH 3.35 is said to be acidic, and will produce hydrogen ions.

3.35 = -log(H+)

(H+) = Antilog (-3.35)

(H+) = 0.000446M

Place (H+) in standard form

(H+) = 4.46 x 10^-4M

Thus, the concentration of hydrogen ion in the solution with pH 3.35 is 4.46 x 10^-4M

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Determine the equilibrium constant for the acid-base reaction between ethanol and hydrobromic acid? Acid pKa Hydrobromic Acid −5

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$10^{-3.4$

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Let us first take a look at the image below;

In the acid - base reaction; we can see the transfer of electrons that takes place;

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The stronger acid is shown with the one with more negative $P_{Ka}$ Value.

∴ The equilibrium constant for the acid-base reaction is expressed as:

$K_{eq}= \frac{K_a of reactant acid}{K_a of product acid}$

$= \frac{10^{-pK} of reactant acid}{10^{-pk} of product acid}$

From $P_{Ka}$ Value (shown in the image below), it is clear and vivid that hydrobromic acid is a stronger acid than the ethyloxonium ion, therefore the equilibrium lies to the right.

From the chemical equation (shown in the attached image); the equilibrium constant for the acid-base reaction can be expressed as:

$K_{eq}=\frac{10^{-pK} of hydrobromic acid}{10^{-pk} of Ethyloxonium acid}$

$K_{eq}=\frac{10^{-5.8} of hydrobromic acid}{10^{-2.4} of Ethyloxonium acid}$

$= 10^{-3.4}$

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