Question

In: Physics

A solution of sucrose is prepared by dissolving 0.5 g in 100 g of water. Calculate:...

A solution of sucrose is prepared by dissolving 0.5 g in 100 g of water. Calculate: a. Percent weight in weight b. The molal concentration of sucrose and water c. The mole fraction of sucrose and water in the solution

Solutions

Expert Solution

Solution of sucrose has 0.5g sucrose in 100g of water

a) Percent weight in weight is given by

m of solution=0.5+100=100.5g

b) Molal concentration or molality is defined as

where m_solvent is mass of water in our case=100g=0.1kg

n_solute is number of moles of sucrose

Molar mass of sucrose=342.3g/mol

Hence number of moles=

c)For mole fraction

Lets calculate number of moles of water

As molar mass of water is 18.02

   moles

Mole fraction sucrose

Mole fraction water


Related Solutions

A) A solution is prepared by dissolving 50.7 g sucrose (C12H22O11) in 0.423 kg of water....
A) A solution is prepared by dissolving 50.7 g sucrose (C12H22O11) in 0.423 kg of water. The final volume of the solution is 355 mL. 1) For this solution, calculate molarity. 2) For this solution, calculate molality. 3) For this solution, calculate percent by mass. 4) For this solution, calculate mole fraction. B) Calculate the vapor pressure at 25 ∘C of a solution containing 55.2 g ethylene glycol (HOCH2CH2OH) and 286.6 g water. The vapor pressure of pure water at...
A solution is prepared by dissolving 50.7 g sucrose (C12H22O11) in 0.394 kg of water. The...
A solution is prepared by dissolving 50.7 g sucrose (C12H22O11) in 0.394 kg of water. The final volume of the solution is 355 mL. calculate: a- molarity b- molality c- percent by mass d- mole fraction
A solution is prepared by dissolving 50.8 g sucrose(C12H22O11) in 0.387 kg of water. The final...
A solution is prepared by dissolving 50.8 g sucrose(C12H22O11) in 0.387 kg of water. The final volume of the solution is 355 mL. For this solution, calculate molarity. For this solution, calculate molality. For this solution, calculate percent by mass. For this solution, calculate mole fraction.
A solution was prepared by dissolving 29.0g KCl in 225 g of water. 1) Calculate the...
A solution was prepared by dissolving 29.0g KCl in 225 g of water. 1) Calculate the mass percent of KCl in the solution. 2)Calculate the mole fraction of the ionic species KCl in the solution. 3) Calculate the molarity of KCl in the solution if the total volume of the solution is 239 mL. 4) Calculate the molarity of KCl in the solution.
A solution is prepared by dissolving 50.4g sucrose (C12H22O11) in 0.332kg of water. The final volume...
A solution is prepared by dissolving 50.4g sucrose (C12H22O11) in 0.332kg of water. The final volume of thesolution is 355 mL. Calculate the concentration of the solution in each unit? Molarity Molality Percent by mass Mole fraction mole percent.
Part A) Calculate the vapor pressure of water above a solution prepared by dissolving 29.5 g...
Part A) Calculate the vapor pressure of water above a solution prepared by dissolving 29.5 g of glycerin in 140 g of water at 343 K Part B) Calculate the mass of ethylene glycol that must be added to 1.00 kg of ethanol to reduce it's vapor pressure by 11.0 torr at 35° C. The vapor pressure of pure ethanol at 35°C is 1.00×10^2 torr.
Calculate the vapor pressure of water above a solution prepared by dissolving 27.0 g of glycerin...
Calculate the vapor pressure of water above a solution prepared by dissolving 27.0 g of glycerin (C3H8O3) in 135 g of water at 343 K. (The vapor pressure of water at 343 K is 233.7 torr.) Ph2o=? Calculate the mass of ethylene glycol (C2H6O2) that must be added to 1.00 kg of ethanol (C2H5OH) to reduce its vapor pressure by 9.00 torr at 35∘C. The vapor pressure of pure ethanol at 35∘C is 1.00×102 torr. m=?
A solution is prepared by dissolving 23.7 g of CaCl2 in 375 g of water. The...
A solution is prepared by dissolving 23.7 g of CaCl2 in 375 g of water. The density of the resulting solution is The mole fraction of Cl- in this solution is __________ M.
A solution is prepared by dissolving 23.7 g of CaCl2 in 375 g of water. The...
A solution is prepared by dissolving 23.7 g of CaCl2 in 375 g of water. The density of the resulting solution is 1.05 g/mL. The concentration of CaCl2 in this solution is M
A solution is prepared by dissolving 29.2 g of glucose (C6H12O6) in 355 g of water....
A solution is prepared by dissolving 29.2 g of glucose (C6H12O6) in 355 g of water. The final volume of the solution is 378 mL . For this solution, calculate each of the following. molarity molality percent by mass mole fraction mole percent
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT