Problem: In lab you need to prepare at least 100 mL of each of the following solutions. Explain how you would proceed using the given information. d. 0.10 mole fraction of C6H12O6 in water (d = 1.00 g/cm3)

FREE Expert Solution
  • Recall that mole fraction is equal to:

  • Total moles of solution is equal to the moles of water and moles of glucose

Moles of solution = moles water + moles glucose

  • We can get the the moles of C6H12O6 , eventually the mass, using the provided volume of solution
View Complete Written Solution
Problem Details

In lab you need to prepare at least 100 mL of each of the following solutions. Explain how you would proceed using the given information. 

d. 0.10 mole fraction of C6H12O6 in water (d = 1.00 g/cm3)

Learn this topic by watchingMole Fraction Concept Videos
All Chemistry Practice Problems Mole Fraction Practice Problems
Q.Label each variable in the equation below with the correct units.
Q.A solution with the same osmotic pressure as the blood is A) isotonic to the blood. B) hypotonic to the blood. C) hypertonic to the bloodD) nontonic t...
Q.Explain why molarity is temperature-dependent, whereas molality is not. Is mole fraction volume percent? Is mass percent? 
Q.The normal boiling point of diethyl ether is 34.5°C. A solution containing a nonvolatile solute dissolved in diethyl ether has a vapor pressure of 698...
Q.A 1.37-M solution of citric acid (H3C6H5O7) in water has a density of 1.10 g/cm3. Calculate the mass percent, molality, mole fraction, and normality o...
Q.A solution is prepared by mixing 50.0 mL toluene (C6H5CH3, d = 0.867 g/cm3) with 125 mL benzene (C6H6, d = 0.874 g/cm3). Assuming that the volumes add...
Q.A solution is prepared by mixing 25 mL pentane (C5H12, d = 0.63 g/cm3) with 45 mL hexane (C6H14, d = 0.66 g/cm3). Assuming that the volumes add on mix...
See all problems in Mole Fraction