Consider the titration of (100.0 mathrm{~mL}) of a solution that contains a mixture of (0.050 mathrm{M} mathrm{H}_{2}
Question:
Consider the titration of \(100.0 \mathrm{~mL}\) of a solution that contains a mixture of \(0.050 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}\) and \(0.20 \mathrm{M}\) \(\mathrm{H}_{2} \mathrm{C}_{6} \mathrm{H}_{6} \mathrm{O}_{6}\). Calculate the \(\mathrm{pH}\)
a. before any \(0.10 \mathrm{M} \mathrm{NaOH}\) has been added.
b. after a total of \(100.0 \mathrm{~mL}\) of \(0.10 \mathrm{M} \mathrm{NaOH}\) has been added.
c. after a total of \(300.0 \mathrm{~mL}\) of \(0.10 \mathrm{M} \mathrm{NaOH}\) has been added.
d. after a total of \(500.0 \mathrm{~mL}\) of \(0.10 \mathrm{M} \mathrm{NaOH}\) has been added.
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Step by Step Answer:
To calculate the pH at each point in the titration we need to consider the contributions of both strong and weak acids present in the solution Strong ...View the full answer
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