Question

What is the pH of a $0\cdot 6$ M HNO $_{3}$ solution?

Answer 1

To calculate the pH of an aqueous solution we need to know about the concentration of H $^{+}$ ion (in terms of molarity) present in the solution. Range of pH scale is from ( $0-14)$ $0$ being the most acidic and $14$ being the most basic. pH of a solution can be calculated using the formula pH = - $\log [{{H}^{+}}]$ .

Complete step by step answer:
Before calculating the pH of a solution first we understand what is pH of a solution. pH means power of H i.e., by how much concentration of H $^{^{+}}$ is present in the solution.
pH quantitatively measures the acidity or basicity of an aqueous solution. If the pH of a solution is less than $7$ then solution Is considered to be acidic and if the pH of a solution is greater than $7$ then the solution is considered to be basic and at $7$ pH solution is neutral.
Let’s see how nitric acid dissociates by writing the balanced chemical equation so that we can conclude about the concentration of H $^{+}$ ion in the solution and then we can use the formula. HNO $_{3}$ +H $_{2}$ O $\to$ H $_{3}$ O $^{+}$ + NO $_{3}$ $^{-}$ . HERE $0\cdot 6$ M is the concentration of H $^{+}$ in the solution.
pH = $-{{\log }_{10}}(0\cdot 60)=-(-0\cdot 22)=0\cdot 22$ . $$ this is our desired pH of the solution.

Note:
You can easily calculate pH in one line just by using the above formula pH = - $\log [{{H}^{+}}]$ . Just keep in mind that pH is a unitless quantity and it only tells us about the concentration of H $^{+}$ ion present in the solution.