Posted by dan on .
A 10.0 mL sample of 3.00 M KOH(aq) is transferred to a 250.0 ml
volumetric flask and diluted to the mark. It was found that 38.5 ml of
this diluted solution was needed to react the stoichimetric point in a
titration of 10.0 mL of a phosphoric acid, H3PO4, solution. The reaction
3 KOH(aq) + H3PO4(aq) ® K3PO4(aq) + 3 H2O(l)
a) Calculate the molarity of H3PO4 in the original solution. 
b) Calculate the percent , by mass, of H3PO4 in the original solution.
Assume the density of the acid is 1.00 g/mL. 
A) .154 M
B) Not sure, 5.8 %
woops i mesed up
here's my answer
question 3: Calculate the density of COCl2, a poisonous gas at 27.0oC and 733 Torr. 
i got 3.87 g/v
I have 3.8758 g/L which rounds to 3.88 g/L. Note g/L and g/v.
looks like im on track