Molarity = 0.053 M
pH = 1.276
Further explanation
Given
5 g of HNO₃
1.5 L solution
Required
Molarity
pH
Solution
Molarity shows the number of moles of solute in every 1 liter of solution.
mol HNO₃(MW=63 g/mol) :
= mass : MW
= 5 g : 63 g/mol
= 0.079
Molarity :
=0.079 : 1.5 L
= 0.053 M
pH = -log [H⁺]
For strong acids like HNO₃ :
[H⁺] = a.M
a = valence of acid / amount of H⁺ released
M = acid concentration.
HNO₃ ⇒ H⁺ + NO₃⁻⇒ valence 1(amount of H⁺=1)
[H⁺]=1 x 0.053
[H⁺]= 0.053 M
pH= - log 5.3 x 10⁻²
pH = 2 - log 5.3
pH= 1.276
