Bonus (a) What is the pH of a solution obtained by mixing equal volumes of a str

Question

Bonus (a) What is the pH of a solution obtained by mixing equal volumes of a strong monoprotic acid solution of pH 3.00 and a strong monobasie solution of pH 11.00 (b) An unknown monoprotic organic acid is dissolved in water and titrated with a solution of NaOH. The pH of the solution is measured after addition of every 0.10 mL of NaOH. The equivalence point is reached when a total of 32.68 mL of the NaOH is added. What is the easiest way to determine the K, of the unknown acid? What volume of NaOH would be required for this determination? (c) Sketch the pH curve for the titration of a weak diprotic acid (analyte) with a strong base (titrant). Correctly label the axes and indicate all important parameters.

Explanation / Answer

for pH = 3 solution, H+ ion concetration = 10-3 M (pH = -log[H+])
for pH =11 solution, H+ ion concetration = 10-11 M. Therefore, OH- concentration = [OH-] = Kw/[H+] 10-14/10-11= 10-3M

Since, we are mixing strong acid and strong bases in equal molar, it will neutralize each other as follows:

H+(aq) + OH(aq) H2O(l)

We have both H+ ion concentration and OH- concentrations are same (10-3 M), and also we are mixing in equal volume, therefore, the resulting will be a neutralization.
At neutralization point we will have pH = 7.
Therefore, the pH of the solution = 7

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