Question

12.50 g (about one tablespoon) of table sugar (sucrose, C12H22O11) is dissolved in 242.2 mLof water (density 0.997 g/mL). The final volume is 250.0 mL (about one cup).

1. Calculate the mass percent of sucrose in this solution.

2. Calculate the molarity of sucrose in this solution.

3. Calculate the molality of sucrose in this solution.

Answer #1

A)
A solution is prepared by dissolving 50.4 g sucrose (C12H22O11) in
0.332 kg of water. The final volume of the solution is 355 mL. For
this solution, calculate the molarity. Express the molarity
in units of moles per liter to three significant
figures.
B)
Calculate the molality. Express the molality in units of
moles per kilogram of solvent to three significant
figures.
C)
Calculate the percent by mass.Express the percent by
mass to three significant figures.
D)
Calculate the...

The density of a 1.22 M aqueous sucrose soluton
(C12H22O11) is 1.25 g/mL.
Calculate the molal concentration, mole fraction (sucrose) and the
mass percent (sucrose) of the solution. What volume (mL) of the
solution would contain 100 g of sucrose?

A solution is prepared by dissolving 13.63 g of sucrose
(C12H22O11) in 612 g of water. The final volume of the solution is
635 mL.
For this solution, calculated the concentration in each unit
indicated below.
a.Molarity
b.Molality
c.Mole fraction of glucose

a. A soft drink contains 11.5% sucrose (C12H22O11) by mass. How
much sucrose, in grams, is contained in 355 mL (12 oz) of the soft
drink? (Assume a density of 1.04 g/mL.)
b.Calculate the molarity of a solution made by putting 55.8 g of
NaNO3 into a beaker and diluting to 2.50 L.
c. Calculate the mass percent (m/m) of a solution prepared by
dissolving 50.92 g of NaCl in 156.8 g of H 2 O .

Common table sugar is known as sucrose, and its formula is
C12H22O11. A- Calculate the mass (in grams) of one billion (1X10^9)
sucrose molecules. B- Write a balance chemical equation, including
state symbols, for the reaction of aqueous sucrose with water to
form aqueous ethanol (C2H6O) and carbon dioxide gas. (This is
fermentation, and it is catalyzed by enzymes in yeast.)

What is the molarity of each solution?
39 g of KCl dissolved in enough water to give
375 mL of solution.
85.8 g of sucrose,
C12H22O11, dissolved in enough
water to give 725 mL of solution.
8.4 g of ammonium sulfate,
(NH4)2SO4, dissolved in enough
water to give 2.35 L of solution.

What mass of sucrose (C12H22O11) should be combined with 492 g
of water to make a solution with an osmotic pressure of 8.80 atm at
295 K ? (Assume the density of the solution to be equal to the
density of the solvent.)

What mass of sucrose (C12H22O11) should be combined with 462 g
of water to make a solution with an osmotic pressure of 8.65 atm at
285 K ? (Assume the density of the solution to be equal to the
density of the solvent.)

What is the osmotic pressure of a solution of 12.5 g sucrose
(C12H22O11) in 225 g water at 50.0 °C? Assume that the density of
the solution is 1.00 g/mL

Sucrose (C12H22O11), a nonionic solute, dissolves in water
(normal freezing/melting point 0.0°C) to form a solution. If some
unknown mass of sucrose is dissolved in 150g of water and this
solution has a freezing/melting point of -0.56°C, calculate the
mass of sucrose dissolved. Kfp for water is 1.86°C/m. [must show
work including units to receive credit].

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