Question

The density of water is 1.00 g/mL. When a salt solution is made up of 0.155 L water and 0.025 kg of sodium chloride, what is the mass percent concentration of this solution?

Answer #1

A solution of 5.00 g of sodium chloride in 1.00 kg of water has
a freezing point of –0.299°C. What is the actual (experimental) van
’t Hoff factor for this salt at this concentration?
Kf(water) =
1.86°C/m

A density column was made with 3 mL of 1 M calcium chloride
solution with a density of 1.1 g/mL, 3 ml of dyed distilled water
with a density of 1.00 g/mL, and then 3 mL of ethanol with a
density of 0.80 g/mL. The calcium chloride solution was poured
first followed by the distilled water and then ethanol. Why was the
calcium chloride solution poured into the density column first?

A solution is 40% ethanol (density = 0.789 g/mL) by volume and
60% water (density = 1.00 g/mL). If Tom Titan has 750.0 mL of the
solution, what is the mass of ethanol in solution?

A.) A solution of H2SO4(aq) with a molal concentration of 3.58 m
has a density of 1.200 g/mL. What is the molar concentration of
this solution?
B.) What is the mole fraction of solute in a 3.79 m aqueous
solution?
C.) An aqueous sodium acetate, NaC2H3O2, solution is made by
dissolving 0.155 moles of NaC2H3O2 in 0.650 kg of water. Calculate
the molality of the solution.

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 2.250×10^−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 2.450×10−2M 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 999.3 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 2.650×10?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...

1) A tank contains 10 kg of salt and 2000 L of water. A solution
of concentration 0.025 kg of salt per liter enters a tank at the
rate 7 L/min. The solution is mixed and drains from the tank at the
same rate. a) What is the concentration of our solution in the tank
initially? concentration = ___ (kg/L) b) Find the amount of salt in
the tank after 1.5 hours. amount = ____ (kg) c) Find the
concentration...

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.

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