Question

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

Answer #1

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 56.4 grams of
glucose in 0.178 kilograms of water. the final volume of the
solution is 400 mililiters. calculate mole percent

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 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 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

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...

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 155.0g of 245 g of water.
Calculate the mole fraction of KCl(the formula weight of KCl is
74.6 g/mol. The formula weight of water is 18.0g/mol). Express the
mole fraction of KClto two decimal places.

An aqueous solution of ammonium sulfate is prepared by
dissolving 2.78 g of ammonium sulfate in 8.38×102 g of
water. The density of the solution is 1.73 g
mL-1.
a) Determine the mass percent of ammonium sulfate in the
solution.
b)Determine the mole fraction of ammonium sulfate in the
solution.

A solution is prepared by dissolving 22.0 g off NaOH in 118.0 g
of water. The NaOH solution has a density of 1.15 g/mL.
A) What is the mass percent (m/m) of The NaOH solution?
B) what is the total volume of the solution?
C) what is the mass/ volume percent?
D) what is titsmolarity?

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