What will be the change in the value of pH if the concentration of aqueous solution of HNO₃ is increased to 0.05 M from 0.03 M?Solve the given problem.
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A) when concentration is 0.03 M
Using Arrhenius concepts
pH = -log₁₀[H₃O⁺]
= -log₁₀〈0.03〉 = -log₁₀[3 × 10⁻²]
= 2 -log₁₀〈3〉 = 2 – 0.477
= 1.52
B) When concentration is 0.05 M
Using Arrhenius concepts,
pH = -log₁₀[H₃O⁺]
= -log₁₀〈0.05〉 = -log₁₀[5 × 10⁻²]
= 2 -log₁₀〈5〉 = 2 – 0.699
= 1.30
So the change in pH is = 1.52 – 1.30 = 0.22
Using Arrhenius concepts
pH = -log₁₀[H₃O⁺]
= -log₁₀〈0.03〉 = -log₁₀[3 × 10⁻²]
= 2 -log₁₀〈3〉 = 2 – 0.477
= 1.52
B) When concentration is 0.05 M
Using Arrhenius concepts,
pH = -log₁₀[H₃O⁺]
= -log₁₀〈0.05〉 = -log₁₀[5 × 10⁻²]
= 2 -log₁₀〈5〉 = 2 – 0.699
= 1.30
So the change in pH is = 1.52 – 1.30 = 0.22
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