If 990. mL of water is added to 10.0 mL of 0.10 M HCl, what is the pH of the resultant solution?

NetherCraft 0

3 Answers

  • Initial no. of moles of HCl = No. of moles of HCl in the resultant solution

    M₁V₁ = M₂ V₂

    (0.10 M) × (10.0 mL) = M₂ × (999 + 10.0 mL)

    M₂ = 0.1 × (10.0/1000) = 0.0010 M

    1 mole of HCl dissociates to give 1 mole of H⁺ ions.

    In the resultant solution, [H⁺] = [HCl] = 0.0010 M

    pH = -log[H⁺] = -log(0.0010) = 3.0

  • Isn’t that amazing — dilution, adding water, makes the pH bigger!! (Better see why!)

  • M1V1 = M2V2

    M1 = 0.10

    V1 = 10 mL

    V2 = 1000 Ml

    Solve for M2

    Answer: 0.0001 M

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