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2 years ago

What is the pH of a 0.75 M HNO3 solution

Chemistry

2 answers:

pogonyaev2 years ago

6 0

Answer: The pH of the solution is 0.125

Explanation:

pH is the negative logarithm of hydrogen ion concentration present in a solution.

To calculate the pH of the reaction, we use the equation:

$pH=-\log[H^+]$

The chemical equation for the dissociation of nitric acid follows:

$HNO_3\rightarrow H^++NO_3^-$

By stoichiometry of the reaction:

1 mole of nitric acid produces 1 mole of hydrogen ions and 1 mole of nitrate ions.

So,

$[H^+]=0.75M$

Putting values in above equation, we get:

$pH=-\log(0.75)\\\\pH=0.125$

Hence, the pH of the solution is 0.125

Sauron [17]2 years ago

4 0

Hello!

The dissociation reaction of HNO₃ is the following:

HNO₃ → H⁺ + NO₃⁻

This is a strong acid, so the concentration of HNO₃ would be the same as the concentration of H⁺. The formula for pH is the following:

$pH=-log([H_3O^{+}])=-log(0,75M)=0,12$

So, the pH would be 0,12

Have a nice day!

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2 years ago

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luda_lava [24]

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