If I have .156 M of succinic acid and the density is 1.099g/ml in 10ml of succin

Question

If I have .156 M of succinic acid and the density is 1.099g/ml in 10ml of succinic acid, what would the mass be of succinic acid in 100 g of solution. I titrated it with .35M of NaOH and came out with it taking 26.75 ml of NaOH to neutralize the Succinic acid. How would I determine the mass of succinic acid in 100g of room temperture water.

I figured the balanced equation to be H2C4H4O4 + 6NaOH > 4CO + 6H2O + 6Na, Is this correct? If I have .35 M NaOH and it took 26.75 ml to nuetralize 10.985 g of Succinic acid what is the Molarity of the Succinic acid? Using the density and the molarity of the room temp. succinic acid soution, determine the mass of succinic acid which would be present in 100.g of the solution. Using my answer from that determine te mass of succinic acid which would be dissolved in 100 g of water at room temp. (hint not all of the solution is water. If I know the mass of succic acid dissolved in 100 g solution, I should be able to find out the mas of water it is dissolved in.) This will me my solubility for succinic acid in water at room temp. in units of g succinic acid/100g of water

Explanation / Answer

balanced equation is C4H6O4 + 2NaOH ===> Na2C4H4O4 + 2H2O

moles of NaOH=molarity*Volume=0.35moles/L*0.02675L=0.00936moles

from stochiometric equation

moles of Succinic acid=1/2*moles of NaOH=0.0047moles

mass of succinic acid=moles*molar mass=0.0047moles*118g/mole=0.5524g

case 1 when succinic acid concentration was known (0.156M)

mass of this solution=density*volume=1.099g/ml*10ml=10.99g

moles of succinic acid in this solution=molarity*volume

=0.156moles*0.01L=0.00156moles

mass of succinic acid=0.00156moles*118g/mole=0.184g so

10.99 g solution contain succinic acid=0.184g

100 g solution contain succinic acid=0.184/10.99*100=1.68g

case 2 when succinic acid concentration was unknown

mass of succinic acid=moles*molar mass=0.0047moles*118g/mole=0.5546g

10.985g of succinic acid solution contain succinic acid in it=0.5546g

and 100g succinic acid solution would contain=0.5546/10.985*100=5.05g

moles of succinic acid=mass*molar mass=0.5546g/118g/mole=0.0047moles

volume of 10.985g solution=mass/density=10.985/1.099g/ml=9.995ml=0.009995L

molarity of succinic acid=moles/volume=0.0047moles/0.009995L=0.47M

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