Question

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

Answer 1

Hint: 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.