Chapter 13 Review Ions in Aqueous Solutions and Colligative Properties Multiple Choice
Problem ane
How many moles of ions are contained in i $\mathrm{50}$ of a one $\mathrm{M}$ solution of $\mathrm{KCl} ?$ of $\mathrm{Mg}\left(\mathrm{NO}_{3}\correct)_{2} ?$
Emily H.
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Trouble 2
Use Effigy 1.3 to predict whether each of the post-obit compounds is considered soluble or insoluble:
a. $\mathrm{KCl}$
b. $\mathrm{NaNO}_{iii}$
c. $\mathrm{AgCl}$
d. $\mathrm{BaSO}_{4}$
e. $\mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{ii}$
f. $\mathrm{Lead}\left(\mathrm{ClO}_{iii}\correct)_{2}$
g. $\left(\mathrm{NH}_{iv}\correct)_{2} \mathrm{~S}$
h. $\mathrm{PbCl}_{2}$ (in cold water)
i. FeS
j. $\mathrm{Al}_{2}\left(\mathrm{Then}_{4}\correct)_{3}$
Emily H.
Numerade Educator
Trouble three
What is a net ionic equation?
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Problem 4
a. What is ionization?
b. Distinguish between ionization and dissociation.
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Problem v
a. Define and distinguish between strong electrolytes and weak electrolytes.
b. Give two examples of each type.
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Problem 6
What determines the strength of a solute as an electrolyte?
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Problem 7
Distinguish betwixt the employ of the terms strong and weak and the employ of the terms dilute and concentrated when describing electrolyte solutions.
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Trouble 8
following ionic compounds in water. (Hint: See Sample Trouble A.)
$$
\brainstorm{assortment}{ll}{\text { a. } \mathrm{KI}} & {\text { c. } \mathrm{MgCl}_{2}} \\ {\text { b. NaNO }_{3}} & {\text { d. } \mathrm{Na}_{ii} \mathrm{SO}_{4}}\stop{array}
$$
Emily H.
Numerade Educator
Problem nine
For the compounds listed in the previous trouble, determine the number of moles of each ion produced
likewise as the total number of moles of ions produced when 1 mol of each compound dissolves in water.
Emily H.
Numerade Educator
Trouble x
Write the equation for the dissolution of each of the post-obit in water, and then indicate the full number of moles of solute ions formed.
a. 0.l mol strontium nitrate
b. 0.50 mol sodium phosphate
Emily H.
Numerade Educator
Problem eleven
Using Figure 1.3, write the balanced chemical equation, write the overall ionic equation, identify the spectator ions and possible precipitates, and write the net ionic equation for each of the post-obit reactions. (Hint: See Sample Trouble B.)
a. mercury (2) chloride $(a q)+$ potassium sulfide $(a q) \longrightarrow$
b. sodium carbonate $(a q)+$ calcium chloride $(a q) \longrightarrow$
c. copper(II) chloride $(a q)+$ ammonium phosphate $(a q) \longrightarrow$
Emily H.
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Problem 12
Identify the spectator ions in the reaction between $\mathrm{KCl}$ and $\mathrm{AgNO}_{three}$ in an aqueous solution.
Emily H.
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Trouble thirteen
Copper(Il) chloride and lead(Ii) nitrate react in aqueous solutions past double displacement. Write the balanced chemical equation, the overall ionic equation, and the net ionic equation for this reaction.
If thirteen.45 g of copper(Il) chloride react, what is the maximum corporeality of precipitate that could be formed?
Emily H.
Numerade Educator
Trouble 14
How does the presence of a nonvolatile solute affect each of the following backdrop of the solvent in
which the solute is dissolved?
a. vapor pressure level
b. freezing point
c. boiling point
d. osmotic force per unit area
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Numerade Educator
Trouble 15
Using Figure 2.1 every bit a guide, make a graph of vapor pressure versus temperature that shows the comparison of pure water, a solution with $x$ concentration of solute, and a solution with ii$x$ concentration of solute. What is the relationship between $\Delta t_{f}$ for the $x$ solution and $\Delta t_{f}$ for the 2$x$ solution?
Emily H.
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Trouble 16
a. Why does the level of the more-concentrated solution rise when two solutions of different concentrations are separated by a semipermeable membrane?
b. When does the level of the solution stop ascent?
c. When the level stops rising, what is the net movement of h2o molecules across the membrane?
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Problem 17
a. Compare the effects of nonvolatile electrolytes with the effects of nonvolatile nonelectrolytes on the freezing and boiling points of solvents in which they are dissolved.
b. Why are such differences observed?
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Trouble 18
Why does the actual freezing-point depression of an electrolytic solution differ from the freezing-point
low calculated on the basis of the concentration of particles?
Emily H.
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Problem nineteen
Determine the freezing-bespeak low of $\mathrm{H}_{2} \mathrm{O}$ in each of the post-obit solutions. (Hint: See Sample Problem $\mathrm{C} .$ .
$$
\begin{assortment}{fifty}{\text { a. } 1.50 \text { thousand solution of } \mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{xi} \text { (sucrose) in } \mathrm{H}_{2} \mathrm{O}} \\ {\text { b. } 171 \mathrm{thou} \text { of } \mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{xi} \text { in } 1.00 \mathrm{kg} \mathrm{H}_{2} \mathrm{O}} \\ {\text { c. } 77.0 \mathrm{k} \text { of } \mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{eleven} \text { in } 400 . \mathrm{g} \mathrm{H}_{2} \mathrm{O}}\end{array}
$$
Emily H.
Numerade Educator
Problem 20
Given the following freezing-signal depressions, determine the molality of each solution of an unknown nonelectrolyte in water. (Hint: See Sample Problem D.)
a. $-0.930^{\circ} \mathrm{C}$
b. $-iii.72^{\circ} \mathrm{C}$
c. $-8.37^{\circ} \mathrm{C}$
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Trouble 21
A solution contains 20.0 $\mathrm{thou}$ of $\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}$ (glucose) in $250 .$ 1000 of h2o.
a. What is the freezing-point depression of the solvent?
b. What is the freezing point of the solution?
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Numerade Educator
Problem 22
How many grams of antifreeze, $\mathrm{C}_{2} \mathrm{H}_{iv}(\mathrm{OH})_{2},$ would be required per $500 . \mathrm{g}$ of water to prevent the water from freezing at a temperature of $-twenty.0^{\circ} \mathrm{C} ?$
Emily H.
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Trouble 23
Pure benzene, $\mathrm{C}_{6} \mathrm{H}_{6},$ freezes at $five.45^{\circ} \mathrm{C} .$ A solution
containing 7.24 $\mathrm{k} \mathrm{C}_{two} \mathrm{Cl}_{4} \mathrm{H}_{2}$ in 115 yard of benzene
(specific gravity $=0.879$ ) freezes at $3.55^{\circ} \mathrm{C}$ . Based on these data, what is the molal freezing-betoken constant for benzene?
Emily H.
Numerade Educator
Problem 24
If 1.500 chiliad of a solute that has a molar mass of 125.0 $\mathrm{g}$ were dissolved in 35.00 $\mathrm{g}$ of camphor, what would exist the resulting freezing signal of the solution?
Emily H.
Numerade Educator
Problem 25
Determine the boiling-point peak of $\mathrm{H}_{2} \mathrm{O}$ in each of the post-obit solutions. (Hint: See Sample Problem E.)
a. 2.5$m$ solution of $C_{six} \mathrm{H}_{12} \mathrm{O}_{six}$ (glucose) in $\mathrm{H}_{two} \mathrm{O}$
b. iii.20 $\mathrm{g} \mathrm{C}_{six} \mathrm{H}_{12} \mathrm{O}_{six}$ in 1.00 $\mathrm{kg} \mathrm{H}_{2} \mathrm{O}$
c. 20.0 $\mathrm{thou} \mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}$ (sucrose) in $500 . \mathrm{g} \mathrm{H}_{ii} \mathrm{O}$
Emily H.
Numerade Educator
Trouble 26
Given the following boiling points, determine the molality of each water solution.
$$
\brainstorm{assortment}{fifty}{\text { a. } 100.25^{\circ} \mathrm{C}} \\ {\text { b. } 101.53^{\circ} \mathrm{C}} \\ {\text { c. } 102.805^{\circ} \mathrm{C}}\end{array}
$$
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Numerade Educator
Problem 27
Given 1.00 $\mathrm{m}$ aqueous solutions of each of the following electrolytic substances, determine the expected change in the freezing indicate of the solvent.
(Hint: See Sample Problem F.)
a. $\mathrm{KI}$
b. CaCl_
c. $\mathrm{Ba}\left(\mathrm{NO}_{3}\correct)_{ii}$
Emily H.
Numerade Educator
Problem 28
What is the expected change in the freezing point of water for a 0.015 m aqueous solution of AlCl $_{three} ?$
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Problem 29
What is the expected freezing point of a solution containing 85.0 g NaCl dissolved in $450 .$ g of water?
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Problem 30
Determine the expected boiling signal of a solution made by dissolving 25.0 $\mathrm{g}$ of barium chloride in 0.150 $\mathrm{kg}$ of water.
Emily H.
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Problem 31
The change in the boiling point of water for an aqueous solution of potassium iodide is $0.65^{\circ} \mathrm{C}$ Determine the molal concentration of potassium iodide.
Emily H.
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Problem 32
The freezing point of an aqueous solution of barium nitrate is $-2.65^{\circ} \mathrm{C}$ . Determine the molal concentration of barium nitrate.
Emily H.
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Problem 33
Calculate the expected freezing point of a solution containing 1.00 $\mathrm{kg} \mathrm{H}_{ii} \mathrm{O}$ and 0.250 $\mathrm{mol} \mathrm{NaCl} .$
Emily H.
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Problem 34
Experimental data for a 1.00 $\mathrm{yard} \mathrm{MgI}_{2}$ aqueous solution indicate an actual change in the freezing point of water of $-4.78^{\circ} \mathrm{C}$ . Find the expected change in the freezing point of water. Suggest a possible reason for the discrepancy between the experimental and expected values.
Emily H.
Numerade Educator
Problem 35
Given 0.01 maqueous solutions of each of the post-obit, arrange the solutions in order of increasing
modify in the freezing betoken of the solution.
a. Nal
b. CaCl_s
c. $\mathrm{K}_{three} \mathrm{PO}_{4}$
d. $\mathrm{C}_{half-dozen} \mathrm{H}_{12} \mathrm{O}_{six}$ (glucose)
Emily H.
Numerade Educator
Problem 36
What is the molal concentration of an aqueous calcium chloride solution that freezes at $-two.43^{\circ} \mathrm{C}$ ?
Emily H.
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Trouble 37
a. Write the balanced formula equation that shows the possible products of a double-deportation reaction between calcium nitrate and sodium chloride.
b. Using Figure $1.iii,$ determine whether in that location is
a precipitate.
c. Does this reaction occur?
Emily H.
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Problem 38
Write a balanced equation to show what occurs when hydrogen bromide dissolves and reacts with water.
Include a hydronium ion in the equation.
Emily H.
Numerade Educator
Problem 39
Write the equation for the dissolution of each of the following in water, and then indicate the full number of moles of solute ions formed.
a. 0.275 mol of potassium sulfide
b. 0.fifteen mol of aluminum sulfate
Emily H.
Numerade Educator
Trouble forty
Calculate the expected change in the boiling bespeak of h2o in a solution made up of 131.two $\mathrm{1000}$ of silver nitrate, $\mathrm{AgNO}_{3}$ , in ii.00 $\mathrm{kg}$ of water.
Emily H.
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Problem 41
Nitrous acrid, HNO, is a weak electrolyte. Nitric acid, $\mathrm{HNO}_{three},$ is a strong electrolyte. Write equations to represent the ionization of each in water. Include the hydronium ion, and show the appropriate kind of arrow in each equation.
Emily H.
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Problem 42
Notice the boiling point of an aqueous solution containing a nonelectrolyte that freezes at $-half dozen.51^{\circ} \mathrm{C} .$
Emily H.
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Problem 43
Write a balanced equation for the dissolution of sodium carbonate, $\mathrm{Na}_{2} \mathrm{CO}_{three},$ in water. Find the number of moles of each ion produced when 0.xx $\mathrm{mol}$ of sodium carbonate dissolves. And then, find the total number of moles of ions.
Emily H.
Numerade Educator
Problem 44
Given the reaction beneath and the data in Figure $one.3,$ write the net ionic equation for the reaction. potassium phosphate $(a q)+\operatorname{lead}(\mathrm{II})$ nitrate $(a q)$
Emily H.
Numerade Educator
Problem 45
Notice the expected freezing point of a water solution that contains 268 $\mathrm{g}$ of aluminum nitrate, $\mathrm{Al}\left(\mathrm{NO}_{iii}\right)_{3}$ in 8.l $\mathrm{kg}$ of h2o.
Emily H.
Numerade Educator
Trouble 46
Applying Models
a. You lot are conducting a freezing-betoken determination in the laboratory by using an aqueous solution of $\mathrm{KNO}_{three}$ . The observed freezing bespeak of the solution is $-i.15^{\circ} \mathrm{C} .$ Using a pure water sample, you recorded the freezing point of the pure solvent on the same thermometer as $0.25^{\circ} \mathrm{C}$ . Make up one's mind the molal concentration of KNO $_{3}$ . Assume that there are no forces of attraction between ions.
b. You are non satisfied with the upshot in part (a) because you doubtable that yous should not ignore
the effect of ion interaction. You accept a 10.00 $\mathrm{mL}$ sample of the solution. After carefully evaporating the water from the solution, you obtain 0.415 $\mathrm{g}$ KNO. Determine the bodily molal concentration of KNO $_{iii}$ and the percentage difference between the concentration observed in the freezing-bespeak determination and the actual concentration of $\mathrm{KNO}_{three}$ . Assume that the solution's density is i.00 $\mathrm{g} / \mathrm{mL}$ .
Emily H.
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Problem 47
Analyzing Data The observed freezing-bespeak depression for electrolyte solutions is sometimes less than the calculated value. Why does this occur? Is the difference greater for concentrated solutions or dilute solutions?
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Problem 48
Analyzing Information The osmotic pressure level of a dilute solution tin can be calculated every bit follows:
$\pi=K R T$
$\pi=$ osmotic pressure
$K=$ concentration in moles per liter
$R=$ ideal gas abiding
$T=$ absolute temperature of the solution
How does the osmotic-pressure equation compare with the ideal gas law?
Emily H.
Numerade Educator
Problem 49
Mutual reactions for Group 13 elements are found in the Elements Handbook (Appendix A). Review this
material, and answer the following:
a. Write cyberspace ionic equations for each of the example reactions listed under "Mutual Reactions" for
Group 13.
b. Which reactions did not change when written in net ionic course? Why?
Problem 50
Mutual reactions for Group 14 elements are establish in the Elements Handbook (Appendix A). Review this
material, and respond the post-obit:
a. Write net ionic equations for each of the case reactions listed nether "Common Reactions" for
Group xiv.
b. Which reactions did non change when written in net ionic grade? Why?
Trouble 51
Find out how much common salt a large northern city, such as New York Metropolis or Chicago, uses on its streets in a
typical winter. What environmental bug event from this utilise of table salt? What substitutes for table salt are
being used to melt water ice and snowfall?
Emily H.
Numerade Educator
Trouble 52
Research the role of electrolytes and electrolytic solutions in your trunk. Find out how electrolytes work in the functioning of nerves and muscles. What are some of the health bug that tin can arise from an imbalance of electrolytes in body fluids?
Problem 53
Operation Determine the freezing point of four different mixtures of water and ethylene glycol (apply
commercial antifreeze). What mixture has the everyman freezing point?
Emily H.
Numerade Educator
Problem 54
Operation Find the optimum mixture of salt and ice for reducing the temperature of the chilling bath
for an ice-foam freezer. Use your data to write a fix of instructions on how to prepare the chilling bath for making ice foam.
Problem 55
Performance Using a depression-voltage dry cell, gather a electrical conductivity apparatus. Secure several unknown
aqueous solutions of equal molality from your instructor, and use the apparatus to distinguish the
electrolytes from the nonelectrolytes. Amidst those identified as electrolytes, rank their relative strengths
as conductors from good to poor.
Problem 56
Performance Using equal volumes of the unknown solutions from the preceding action, explain how
you could utilise the freezing-signal depression concept to distinguish the electrolytes from the nonelectrolytes. Explicate how you could determine the number of ions contained per molecule among the solutes identified as electrolytes. Design and conduct an experiment to exam your theories.
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