Question

What is the pH of a 0.056 m hno3 solution

Answer 1

Answer : The pH of the solution is, 1.25

Explanation : Given,

Concentration (C) = 0.056 M

The equilibrium reaction will be,

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

From the balanced chemical reaction, we conclude that

1 mole of $HNO_3$ dissociate to give 1 mole of $H^+$ ion

So, the concentration of $H^+$ = the concentration of $HNO_3$ = 0.056 M

Now we have to calculate the pH.

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

$pH=-\log (0.056)$

$pH=1.25$

Therefore, the pH of the solution is, 1.25

Answer 2

The pH of a 0.056 M ${\text{HN}}{{\text{O}}_{\text{3}}}$ solution is $\boxed{1.25}$.

Further Explanation:

pH:

The acidic strength of an acid can be determined by pH value. The negative logarithm of hydronium ion concentration is defined as pH of the solution. Lower the pH value of an acid, the stronger will be the acid. Acidic solutions are likely to have pH less than 7. Basic or alkaline solutions have pH more than 7. Neutral solutions have pH equal to 7.

The formula to calculate pH of an acid is as follows:

${\text{pH}}=-{\text{log}}\left[{{{\text{H}}^+}}\right]$                    …… (1)

Here,

$\left[ {{{\text{H}}^+}}\right]$ is hydrogen ion concentration.

The given reaction occurs as follows:

${\text{HN}}{{\text{O}}_3}\rightleftharpoons{{\text{H}}^+}+{\text{NO}}_3^-$

${\text{HN}}{{\text{O}}_3}$ is a strong acid and therefore it dissociates completely to produce one ${{\text{H}}^+}$ and one ${\text{NO}}_3^-$ ion. So the concentration of ${{\text{H}}^+}$ becomes equal to that of ${\text{HN}}{{\text{O}}_3}$ and therefore the concentration of ${{\text{H}}^+}$ is 0.056 M.

Substitute 0.056 M for $\left[ {{{\text{H}}^ + }} \right]$ in equation (1).

$\begin{aligned}{\text{pH}}&=-{\text{log}}\left({0.056}\right)\\&=1.25\\\end{aligned}$

Therefore the pH of the solution is 1.25.

Learn more:

1. The reason for the acidity of water: brainly.com/question/1550328

2. Reason for the acidic and basic nature of amino acid: brainly.com/question/5050077

Answer details:

Grade: High School

Subject: Chemistry

Chapter: Acid, base and salts

Keywords: pH, 1.25, HNO3, H+, NO3-, strong acid, 0.056 M, negative logarithm, hydronium ion concentration, acidic solutions, less than 7, alkaline solutions, more than 7, neutral solutions.