Question

If you titrate 12.6 mL of an unknown monoprotic (one H) acid with 13.0 mL of 0.140 M NaOH, what will be the concentration of the acid?

If you add 23.5g of NaCl to 1.2 kg of water, what will be the boiling point and the freezing point of the new solution? (Kf=1.86, Kb=0.52)

((i appreciate every help i can get, tho i prefer to know how to solve for it)) THANK you so much

Answer 1

<If you titrate 12.6 mL of an unknown monoprotic (one H) acid with 13.0 mL of 0.140 M NaOH, what will be the concentration of the acid?>

As the missing information is the concentration of the unknown acid I assume that is what is being asked for here. The question is poorly worded.

As always start with a balanced equation

HA + NaOH -> NaA + H2O

so 1 mole of HA reacts with 1 mole of NaOH

number of millimoles of NaOH used =
13.0 x 0.140

which must be the same as the original number of millimoles fo HA in solution = 12.6 x X

13.0 x 0.140 = 12.6 x X

find X the concentration of the acid