250.0g citric acid is dissolved in 750.0g H2O. The density of the resulting solu

Question

250.0g citric acid is dissolved in 750.0g H2O. The density of the resulting solution is 1.150g/ml.
What is the molarity of the citric acid solution?
What is the molality of the citric acid solution?
What is the mole fraction of the citric acid solution? 250.0g citric acid is dissolved in 750.0g H2O. The density of the resulting solution is 1.150g/ml.
What is the molarity of the citric acid solution?
What is the molality of the citric acid solution?
What is the mole fraction of the citric acid solution?
What is the molarity of the citric acid solution?
What is the molality of the citric acid solution?
What is the mole fraction of the citric acid solution?

Explanation / Answer

For the given citric acid solution,

Volume of solution = (250 + 750)g/1.150 g/ml = 869.565 ml

molarity = moles/L of solution

              = 250 g/192.124 g/mol x 0.8695 L

              = 1.496 M

molality = moles/kg of solvent

             = 250 g/192.124 g/mol x 0.750 kg

             = 1.734 m

moles fraction of citric acid = moles of citric acid/total moles

                                           = (250/192.124)/((250/192.124)+(750/18)

                                          = 0.03               

Related Questions

Navigate

• Browse (All)
• Browse 2
• Subjects

---