A student discovers a bottle of a highly corrosive monoprotic acid with the label partially destroyed. How can the concentration of the unknown acid be determined without using a pH meter?
A) The student can set-up a titration experiment, where a standardized NaOH solution is used to titrate the unknown strong acid. The moles of OH- added would be equal to moles of H+ in the unknown at the half-way point, therefore, the concentration of the unknown can be calculated.
B) The student can set-up a titration experiment, where a standardized NaOH solution is used to titrate the unknown strong acid. The moles of OH- added would be equal to moles of H+ in the unknown at the equivalence point, therefore, the concentration of the unknown can be calculated.
C) The student can set-up a titration experiment, where a standardized NaOH solution is used to titrate the unknown strong acid. The pH at the equivalence point should be 7 since this is a neutralization reaction, therefore, the concentration of the unknown acid is 1 x 10-7 M.
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