1 ~cm ^3 of 0.01 ~M ~HCl is added to 1 ~L of NaCl solution. The pH of the resulting solution is:

Step-by-step solution

The volume of the HCl solution added is V₁ = 1 cm ^3 = 1 10⁻³ L . The concentration of the HCl solution is M₁ = 0.01 M = 10⁻² M . The total volume of the resulting solution is V₂ = 1 L + 0.001 L 1 L . The number of moles of H ⁺ ions added is n = M₁ V₁ = 10⁻² mol/L 10⁻³ L = 10⁻⁵ mol . The concentration of H ⁺ ions in the final solution is [ H ⁺] = n V₂ = 10⁻⁵ mol 1 L = 10⁻⁵ M . The pH of the solution is given by pH = - [ H ⁺] = - (10⁻⁵) = 5 . Answer: 5