Question

A 2.450×10^{−2}*M* solution of NaCl in water is
at 20.0∘C. The sample was created by dissolving a sample of NaCl in
water and then bringing the volume up to 1.000 L. It was determined
that the volume of water needed to do this was 999.3 mL . The
density of water at 20.0∘C is 0.9982 g/mL.

**Part A**

Calculate the molality of the salt solution.

**Part B**

Calculate the mole fraction of salt in this solution.

**Part C**

Calculate the concentration of the salt solution in percent by mass.

**Part D**

Calculate the concentration of the salt solution in parts per million.

Answer #1

A 2.050×10−2M solution of NaCl in water is
at 20.0∘C. The sample was created by dissolving a sample of NaCl in
water and then bringing the volume up to 1.000 L. It was determined
that the volume of water needed to do this was 999.4 mL . The
density of water at 20.0∘C is 0.9982 g/mL.
Part A
Calculate the molality of the salt solution.
Express your answer to four significant figures and include the
appropriate units.
Part B
Calculate...

A 2.650×10?2 M solution of NaCl in water is at 20.0?C. The
sample was created by dissolving a sample of NaCl in water and then
bringing the volume up to 1.000 L. It was determined that the
volume of water needed to do this was 999.3 mL . The density of
water at 20.0?C is 0.9982 g/mL. Part A. Calculate the molality of
the salt solution. Part B.Calculate the mole fraction of salt in
this solution Part C Calculate the...

A 2.250×10^−2 M solution of NaCl in water is at 20.0∘C. The
sample was created by dissolving a sample of NaCl in water and then
bringing the volume up to 1.000 L. It was determined that the
volume of water needed to do this was 999.4 mL . The density of
water at 20.0∘C is 0.9982 g/mL.
a. Calculate the molality of the salt solution.
b. Calculate the mole fraction of salt in this solution.
c. Calculate the concentration of...

A 2.650×10−2 M solution of NaCl in water is at 20.0∘C. The
sample was created by dissolving a sample of NaCl in water and then
bringing the volume up to 1.000 L. It was determined that the
volume of water needed to do this was 999.3 mL . The density of
water at 20.0∘C is 0.9982 g/mL.
Calculate the mole fraction of salt in this solution.
Calculate the concentration of the salt solution in percent by
mass.
Calculate the...

A 2.100×10−2 M solution of NaCl in water is at 20.0∘C. The
sample was created by dissolving a sample of NaCl in water and then
bringing the volume up to 1.000 L. It was determined that the
volume of water needed to do this was 999.4 mL . The density of
water at 20.0∘C is 0.9982 g/mL.
Part A
Calculate the molality of the salt solution.
Express your answer to four significant figures and include the
appropriate units.
Part B...

A 2.350×10−2 M solution of NaCl in water is at 20.0∘C. The
sample was created by dissolving a sample of NaCl in water and then
bringing the volume up to 1.000 L. It was determined that the
volume of water needed to do this was 999.4 mL . The density of
water at 20.0∘C is 0.9982 g/mL. Calculate the concentration of the
salt solution in percent by mass.

A
0.02350 M solution of NaCl in water is at 20degrees. The sample was
created by dissolving a sample of NaCl in water and then bringing
the volume up to 1.000 L. It was determined that the volume of
water needed to do this was 999.4ml The density of water @20
degrees is 0.9982g/mL.
Calculate the morality of the salt solution, the mole fraction
of salt in this solution, the concentration of the salt solution in
% by mass, &...

1) Use Henry's law to determine the molar solubility of helium
at a pressure of 1.9 atm and 25 ∘C. Henry’s law constant for helium
gas in water at 25 ∘C is 3.70⋅10−4M/atm.
2) A 2.800×10−2M solution of NaCl in water
is at 20.0∘C. The sample was created by dissolving a sample of NaCl
in water and then bringing the volume up to 1.000 L. It was
determined that the volume of water needed to do this was 999.2 mL...

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 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

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