A 5.00 mL sample of hydrochloric acid is titrated with 0.1293 M ammonia (a base). If the titration required 28.15 mL of ammonia, determine t

Question

A 5.00 mL sample of hydrochloric acid is titrated with 0.1293 M ammonia (a base). If the titration required 28.15 mL of ammonia, determine the following:
the original concentration of the acid
the original pH of the acid

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Gerda 3 months 2021-08-04T19:20:19+00:00 1 Answers 5 views 0

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    2021-08-04T19:21:42+00:00

    Answer:

    1. C = 0.73 M.

    2. pH = 0.14

           

    Explanation:

    The reaction is the following:

    HCl + NH₃ ⇄ NH₄⁺Cl⁻

    From the titration, we can find the number of moles of HCl that were neutralized by the ammonia.

     n_{a} = n_{b}

    Where “a” is for acid and “b” is for base.

    The number of moles is:

     n = C*V  

    Where “C” is for concentration and “V” for volume.

     C_{a}V_{a} = C_{b}V_{b}

     C_{a} = \frac{0.1293 M*28.15 mL}{5.00 mL} = 0.73 M

    Hence the initial concentration of the acid is 0.73 M.

    The original pH of the acid is given by:

     pH = -log([H^{+}])

     pH = -log(0.73) = 0.14          

    Therefore, the original pH of the acid is 0.14.

    I hope it helps you!                  

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