Question

a) A sucrose solution is prepared to a final concentration of
0.160 M . Convert this value into terms of g/L, molality, and mass
% (molecular weight, MWsucrose = 342.296 g/mol ; density, ρsol′n =
1.02 g/mL ; mass of water, mwat = 965.2 g ). Note that the mass of
solute is included in the density of the solution. Express the
concentrations in grams per liter, molality, and mass percent to
three significant figures separated by commas. Hints Sucrose
concentrations = g/L, m, % **Express the concentrations in
grams per liter, molality, and mass percent to three significant
figures separated by commas.**

B) Suppose 209.1 mg of PbCl2 was added to 15.0 mL of water in a flask, and the solution was allowed to reach equilibrium at 20.0 oC. Some solute remained at the bottom of the flask after equilibrium, and the solution was filtered to collect the remaining PbCl2, which had a mass of 60.5 mg . What is the solubility of PbCl2 (in g/L)? Express the concentration in grams per liter to three significant figures. Solubility of PbCl2 = g/L

Answer #1

(a)

(i)

Molarity = 0.160 M

Means that 0.160 mol of sucrose is in 1 L of solution

Mass of sucrose = moles * molar mass = 0.160 * 342.296 = 54.767 g.

Therefore, concentration in g/L = 54.767 g/L

(ii)

density of solution = 1.02 g/mL

Mass of 1000 mL of solution = 1.02 * 1000 = 1020 g.

Mass of solute = 54.767 g.

Mass of solvent = 1020 - 54.767 = 945.2 g. = 0.9452 kg.

Molality = moles / kg of solvent = 0.160 / 0.9452 = 0.1693 mol / kg

(iii)

Mass percentage = mass of sucrose * 100 / mass of solution = 54.767 * 100 / 1020 = 5.37 %

Part C
A sucrose solution is prepared to a final concentration of 0.280
M . Convert this value into terms of g/L, molality, and mass %
(molecular weight, MWsucrose = 342.296 g/mol ;
density, ρsol′n = 1.02 g/mL ; mass of water, mwat
= 924.2 g ). Note that the mass of solute is included in the
density of the solution.
Express the concentrations in grams per liter, molality, and
mass percent to three significant figures separated by commas.
View...

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...

An aqueous NaCl solution is made using 111 g of NaCl diluted to
a total solution volume of 1.10 L . Part A Calculate the molarity
of the solution. Express your answer using three significant
figures. Part B Calculate the molality of the solution. (Assume a
density of 1.08 g/mL for the solution.) Express your answer using
two significant figures. Part C Calculate the mass percent of the
solution. (Assume a density of 1.08 g/mL for the solution.) Express
your...

Consider that you prepared a solution by mixing 0.23 g solute
with 9.10 g of solvent. If you measured that the solution had a
molality of 0.168 m, what is the molar mass of the
solute?
Express your answer numerically to three significant
figures.

Consider that you prepared a solution by mixing 0.17 g solute
with 8.26 g of solvent. If you measured that the solution had a
molality of 0.157 m, what is the molar mass of the solute? Express
your answer numerically to three significant figures.

Part A
Calculate the mass percent (m/m) of a solution prepared by
dissolving 52.18 g of NaCl in 152.8 g of H2O.
Express your answer to four significant figures.
Part B
Vinegar is a solution of acetic acid in water. If a 185 mL bottle
of distilled vinegar contains 26.5 mL of acetic acid, what is the
volume percent (v/v) of the solution?
Express your answer to three significant figures.
Part C
Calculate the mass/volume percent (m/v) of 24.0 g...

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 solution of Lithium chloride (LiCl) has a concentration of
7.700 mol/L and a density of 1.1658 g/ml. Find the molality and the
percent (mass/mass) concentration.

1. The density at 20 ∘C of a 0.258 m solution of glucose in
water is 1.0173 g/mL, and the molar mass of glucose is 180.2 g/mol.
What is the molarity of the solution?
2. Household bleach is a 3.0 mass % aqueous solution of sodium
hypochlorite, NaOCl.
3.
A. What is the molality of the bleach? (Express your answer
using two significant figures.)
B. What is the mole fraction of NaOCl in the bleach? (Express
your answer using two...

1.Percent by mass to parts per million. Convert 4.45% NaOH(aq)
solution to parts per million NaOH in the solution. Do NOT assume a
dilute aqueous solution! Use the molar mass of the entire salt
formula, not either ion alone. The solution density is 1.047 g/mL.
Answer to 3 significant figures with appropriate units.
2. Molarity to parts per million. Convert 1.672 mol/L MgCl2(aq)
solution to parts per million Mg2+ in the solution. Do NOT assume
this is a dilute aqueous...

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 5 minutes ago

asked 5 minutes ago

asked 7 minutes ago

asked 8 minutes ago

asked 11 minutes ago

asked 11 minutes ago

asked 14 minutes ago

asked 19 minutes ago

asked 21 minutes ago

asked 21 minutes ago

asked 21 minutes ago

asked 28 minutes ago