[kzee25]

Ok I have the Molarity of .191M and density of 1.914g/mL of succinic acid. I am supposed to find the mass of succinic acid in a 100.g of the solution. 

The last question I found the moles of succinic acid in 10.0mL of solution  using the equation: H2C4H4O4 + 6NaOH= 4CO+ 6 H2O + 6Na  and using hte molarity of NaOH which was .35.  The found the molarity of the succinic acid.

So I guess my first question is did I get the right Molarity for the succinic acid?
Then how do I go about using the molarity and the density to find the mass of succinic acid which would be present in 100.g of this solution?

Thanks for any help.

[sjb]

What volume would 100g of your solution take up?

[Borek]

Ok I have the Molarity of .191M and density of 1.914g/mL of succinic acid.

Density looks ridiculously high to me.

[kzee25]

Ok I have the Molarity of .191M and density of 1.914g/mL of succinic acid.

Density looks ridiculously high to me.

Well it said to determine the average mass of 10.0 mL fo the solution which was 10.135g.  Then determine the density of the solution.  I just divided the 2, is that wrong?
Ok i see i miss typed it, does 1.014g/mL seem better?

[Borek]

1.014 g/mL looks reasonably

[kzee25]

1.014 g/mL looks reasonably

How do I go from the density i found and the molarity to the mass in  100.g of solution?

[Borek]

Follow question sjb asked.

[kzee25]

Follow question sjb asked.

Do I just use the density and 100g to get the volume? I did that and got 98.6 mL.  How do i then use the molarity to find the mass? Do I put the molarity= m/.0986L

[Borek]

How many moles in that volume?

[kzee25]

How many moles in that volume?

Ok I get it know, thanks for all your *delete me*!