Question

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

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...

A solution is prepared by dissolving 29.0 g of glucose (C6H12O6)
in 360 g of water. The final volume of the solution is 382 mL . For
this solution, calculate each of the following.
A. Mole Fraction
B. Mole Percent

QUESTION 10
A solution is prepared
by dissolving 40.0 g of sucrose
(C12H22O11, MM = 342 g/mol) in
250. g of H2O at 298 K. What is the vapor pressure of
the solution if the vapor pressure of water at 298 K is 23.76 mm
Hg?
0.198 mm Hg
20.5 mm Hg
23.6 mm Hg
28.0 mm Hg

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 20.2 mL of methanol (CH3OH)
in 100.0 mL of water at 25 ∘C. The final volume of the solution is
118 mL. The densities of methanol and water at this temperature are
0.782 g/mL and 1.00 g/mL, respectively. For this solution,
calculate each of the following.
A. Molarity
B. Molality
C. Percent by Mass
D. Mole fraction

A solution is prepared by dissolving 20.2 mL of methanol in
100.0 mL of water. The final volume of this solution is 118ml. The
densities of methanol and water are 0.782 g/mL and 1.00 g/mL,
respectively. For this solution, calculate the following-
molarity
molality
mass %
MOLE FRACTION
VOLUME OF SOLVENT
MASS OF SOLVENT
MOLES OF SOLVENT
VOLUME OF SOLUTE
MOLES OF SOLUTE
MASS OF SOLUTE
VOLUME OF SOLUTION
MASS OF SOLUTION

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.

A
solution is prepared by dissolving 23.7 g of CaCl 2 in 375 g of
water. The density of the resulting solution is 1.05 g/mL. The
concentration of Cl- in this solution is ________ M.
Also, The concentration of HCl in a solution that is prepared
by dissolving 5.5 g of HCl in 200 g of C2H6O is ________
molal.

A solution is prepared by dissolving 61.5 mL of methanol in
115.0 mL of water at 25 ∘C . The final volume of the solution is
173.4 mL . The densities of methanol and water at this temperature
are 0.782 g/mL and 1.00 g/mL , respectively. For this solution,
calculate each of the following. [Molarity, molality, mass
percent]

A solution was prepared by
dissolving 26.0 g of KCl in 225 g of water.
The composition of a solution can be expressed in several
different ways. Four of the most common concentration units are
defined as follows:. mass %=mass of
componenttotal mass of solution×100%; mole fraction (X)=moles of
componenttotal moles of solution; molarity (M)=moles of
soluteliters of solution; molality (m)=moles of
solutemass of solvent (kg)
Part A
Calculate the mass percent of KCl in the solution.
Part B
Calculate...

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