Calculate the pH of a buffer that is 0.225 M HC_2 H_3O_2 and 0.162 M KC_2H_3O_2.

Question

Calculate the pH of a buffer that is 0.225 M HC_2 H_3O_2 and 0.162 M KC_2H_3O_2. The ka for HC_2H_3O_2 is 1.8 Times 10^-5 4.89 9.11 4.74 9.26 4.60 calculate the ph of a solution formed by mixing 250.0mL of 0.15 M NH_4Cl with 100.0 ml of 0.20 M NH_3. The K_b for NH_3 is 1.8 Times 10^-5 9.13 9.25 9.53 4.74 8.98 which of the following is TRUE? An effective buffer has a [base]/[acid] ratio in the range of10- a buffer is most resistant to pH change when [acid] = [conjugate base] an effective buffer has very small absolute concentrations of acid and conjugates base A buffer cannot be destroyed by adding too much strong base. It can only be destroyed by adding too much strong acid None of the above are TRUE? When titrating a monoprotic strong acid with a weak base at 25 degree C, the pH will be 7 at the equivalence point pH will be greater than 7 at the equivalence point A 100.0ml sample of 0.18 M HClO_4 is titrated with 0.27 M LiOH. Determine the pH of the solution before the addition of any LiOH 1.74 1.05 0.74 0.57 1.57 A 100.0ml sample of 0.18 M HClO_4 is titrated with 0.27 M LiOH. Determine the pH of the solution before the addition of 30.0mL LiOH 0.86 1.21

Explanation / Answer

VI.

this will be a buffer

pH = pKa + log(conjugate/acid)

pKa = -log(1.8*10^-5) = 4.75

the conjugate = KC2H3O2

the acid = HC2H3O2

then

pH = pKa + log(conjugate/acid)

p´H = 4.75 + log(0.162/0.225) = 4.6073324

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