A chemistry problem by Dhruv Singh

Chemistry Level 2

Find the pH of the solution formed when 0.02 mol 0.02\text{ mol} of H C l \ce{HCl} is added to water to make the total volume as 2.0 L 2.0\text{ L} .

10.54 1.67 2.0 5

Dhruv Singh by Dhruv Singh , 19, India

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1 solution

Tapas Mazumdar
Dec 24, 2016

Molarity of HCl solution = No. of moles of HCl Volume of solution (in litres) ⟹ M = 0.02 2 = 1 100 = 1 0 − 2 ⟹ p H ( HCl ) = − log ⁡ 10 1 0 − 2 = 2.0 \text{Molarity of HCl solution } = \dfrac{\text{No. of moles of HCl}}{\text{Volume of solution (in litres)}} \\ \implies M = \dfrac{0.02}{2} = \dfrac{1}{100} = 10^{-2} \\ \implies \text{p}^{\text{H}} (\text{HCl}) = -\log_{10} 10^{-2} = \boxed{2.0}

3 Helpful 0 Interesting 0 Brilliant 0 Confused

Well explained. Just one thing missing. You have to state that hydronium ions come from water too, but its its dissocitaion constant is 10 − 14 {10}^{-14} which is negligible compared to the amount of hydronium ions coming from the strong acid HCl.

Ashish Menon - 4 years, 5 months ago

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