when a solution prepared by dissolving 4.00g of an unknown monoprotic acid in 1.00L of water is titrated with 0.600M NaOH, 38.7mL of the NaOH solution is needed to neutralize the acid. What was the molarity of the acid solution? what is the molecular weight of the unknown acid?

1 answer

HA is the acid.
HA + NaOH ==> NaA + H2O

moles NaOH = M x L = 0.6000 x 0.0387 = 0.02322.
Therefore, moles HA = 0.02322
M of HA = moles/L.
moles = grams/molecular weight
m.w. = grams/moles = 4/0.02322 = ?? Then round to 3 significant figures (based on the 38.7)
Similar Questions
    1. answers icon 2 answers
  1. A student is given 3 beakers:Beaker 1- 50.0 ml of a solution produced by dissolving 6.00 grams of a weak monoprotic acid ,HX, in
    1. answers icon 3 answers
  2. What would be the pH of a solution of hy-poiodous acid (HOI) prepared by dissolving 144 grams of the acid in 200 mL of pure
    1. answers icon 2 answers
    1. answers icon 4 answers
more similar questions