chemistry

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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
is:
3 KOH(aq) + H3PO4(aq) ® K3PO4(aq) + 3 H2O(l)
a) Calculate the molarity of H3PO4 in the original solution. [3]
b) Calculate the percent , by mass, of H3PO4 in the original solution.
Assume the density of the acid is 1.00 g/mL. [2]

A) .154 M

B) Not sure, 5.8 %

  • chemistry -

    woops i mesed up

    here's my answer

    A .120

    b 1.51%

  • chemistry -

    question 3: Calculate the density of COCl2, a poisonous gas at 27.0oC and 733 Torr. [3]

    i got 3.87 g/v

  • chemistry -

    I have 3.8758 g/L which rounds to 3.88 g/L. Note g/L and g/v.

  • chemistry -

    thanks

    looks like im on track

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