Chapter 13 Review Ions in Aqueous Solutions and Colligative Properties
Problem 1
How many moles of ions are contained in 1 $\mathrm{50}$ of a 1 $\mathrm{M}$ solution of $\mathrm{KCl} ?$ of $\mathrm{Mg}\left(\mathrm{NO}_{three}\correct)_{2} ?$
Emily H.
Numerade Educator
Problem 2
Use Effigy one.iii to predict whether each of the post-obit compounds is considered soluble or insoluble:
a. $\mathrm{KCl}$
b. $\mathrm{NaNO}_{3}$
c. $\mathrm{AgCl}$
d. $\mathrm{BaSO}_{4}$
due east. $\mathrm{Ca}_{iii}\left(\mathrm{PO}_{4}\right)_{2}$
f. $\mathrm{Pb}\left(\mathrm{ClO}_{iii}\correct)_{2}$
k. $\left(\mathrm{NH}_{4}\correct)_{two} \mathrm{~S}$
h. $\mathrm{PbCl}_{ii}$ (in cold water)
i. FeS
j. $\mathrm{Al}_{2}\left(\mathrm{Then}_{4}\right)_{3}$
Emily H.
Numerade Educator
Problem three
What is a internet ionic equation?
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Numerade Educator
Problem 4
a. What is ionization?
b. Distinguish betwixt ionization and dissociation.
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Numerade Educator
Problem five
a. Ascertain and distinguish between stiff electrolytes and weak electrolytes.
b. Requite two examples of each blazon.
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Trouble 6
What determines the strength of a solute as an electrolyte?
Emily H.
Numerade Educator
Problem 7
Distinguish between the use of the terms stiff and weak and the apply of the terms dilute and full-bodied when describing electrolyte solutions.
Emily H.
Numerade Educator
Problem viii
post-obit ionic compounds in water. (Hint: Meet Sample Problem A.)
$$
\brainstorm{assortment}{ll}{\text { a. } \mathrm{KI}} & {\text { c. } \mathrm{MgCl}_{2}} \\ {\text { b. NaNO }_{3}} & {\text { d. } \mathrm{Na}_{ii} \mathrm{Then}_{4}}\end{array}
$$
Emily H.
Numerade Educator
Problem 9
For the compounds listed in the previous trouble, determine the number of moles of each ion produced
besides as the full number of moles of ions produced when one mol of each chemical compound dissolves in water.
Emily H.
Numerade Educator
Problem 10
Write the equation for the dissolution of each of the post-obit in water, and then bespeak the total number of moles of solute ions formed.
a. 0.fifty mol strontium nitrate
b. 0.50 mol sodium phosphate
Emily H.
Numerade Educator
Problem eleven
Using Effigy 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: Run across Sample Problem B.)
a. mercury (II) 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.
Numerade Educator
Problem 12
Identify the spectator ions in the reaction betwixt $\mathrm{KCl}$ and $\mathrm{AgNO}_{3}$ in an aqueous solution.
Emily H.
Numerade Educator
Problem 13
Copper(Il) chloride and lead(2) nitrate react in aqueous solutions by double deportation. Write the balanced chemical equation, the overall ionic equation, and the net ionic equation for this reaction.
If xiii.45 g of copper(Il) chloride react, what is the maximum amount of precipitate that could be formed?
Emily H.
Numerade Educator
Problem 14
How does the presence of a nonvolatile solute affect each of the post-obit properties of the solvent in
which the solute is dissolved?
a. vapor force per unit area
b. freezing indicate
c. boiling point
d. osmotic pressure level
Emily H.
Numerade Educator
Problem 15
Using Effigy 2.1 as a guide, brand a graph of vapor force per unit area versus temperature that shows the comparison of pure water, a solution with $x$ concentration of solute, and a solution with 2$ten$ 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.
Numerade Educator
Problem sixteen
a. Why does the level of the more-concentrated solution ascent when two solutions of different concentrations are separated past a semipermeable membrane?
b. When does the level of the solution cease rising?
c. When the level stops rising, what is the cyberspace motility of water molecules across the membrane?
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Numerade Educator
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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Numerade Educator
Problem eighteen
Why does the actual freezing-signal depression of an electrolytic solution differ from the freezing-signal
depression calculated on the basis of the concentration of particles?
Emily H.
Numerade Educator
Trouble 19
Determine the freezing-point depression of $\mathrm{H}_{2} \mathrm{O}$ in each of the following solutions. (Hint: Encounter Sample Trouble $\mathrm{C} .$ .
$$
\begin{array}{50}{\text { a. } 1.50 \text { grand solution of } \mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11} \text { (sucrose) in } \mathrm{H}_{2} \mathrm{O}} \\ {\text { b. } 171 \mathrm{g} \text { of } \mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11} \text { in } 1.00 \mathrm{kg} \mathrm{H}_{two} \mathrm{O}} \\ {\text { c. } 77.0 \mathrm{m} \text { of } \mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11} \text { in } 400 . \mathrm{yard} \mathrm{H}_{2} \mathrm{O}}\end{assortment}
$$
Emily H.
Numerade Educator
Problem 20
Given the following freezing-point depressions, decide the molality of each solution of an unknown nonelectrolyte in water. (Hint: Run into Sample Problem D.)
a. $-0.930^{\circ} \mathrm{C}$
b. $-three.72^{\circ} \mathrm{C}$
c. $-8.37^{\circ} \mathrm{C}$
Emily H.
Numerade Educator
Problem 21
A solution contains 20.0 $\mathrm{thousand}$ of $\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{six}$ (glucose) in $250 .$ thou of h2o.
a. What is the freezing-point depression of the solvent?
b. What is the freezing bespeak of the solution?
Emily H.
Numerade Educator
Problem 22
How many grams of antifreeze, $\mathrm{C}_{two} \mathrm{H}_{4}(\mathrm{OH})_{2},$ would be required per $500 . \mathrm{g}$ of water to prevent the h2o from freezing at a temperature of $-twenty.0^{\circ} \mathrm{C} ?$
Emily H.
Numerade Educator
Problem 23
Pure benzene, $\mathrm{C}_{6} \mathrm{H}_{6},$ freezes at $5.45^{\circ} \mathrm{C} .$ A solution
containing 7.24 $\mathrm{g} \mathrm{C}_{two} \mathrm{Cl}_{four} \mathrm{H}_{2}$ in 115 g of benzene
(specific gravity $=0.879$ ) freezes at $3.55^{\circ} \mathrm{C}$ . Based on these data, what is the molal freezing-signal constant for benzene?
Emily H.
Numerade Educator
Problem 24
If 1.500 m of a solute that has a tooth mass of 125.0 $\mathrm{g}$ were dissolved in 35.00 $\mathrm{g}$ of camphor, what would exist the resulting freezing point of the solution?
Emily H.
Numerade Educator
Problem 25
Determine the boiling-point tiptop of $\mathrm{H}_{2} \mathrm{O}$ in each of the following solutions. (Hint: Come across Sample Problem Due east.)
a. 2.5$chiliad$ solution of $C_{vi} \mathrm{H}_{12} \mathrm{O}_{six}$ (glucose) in $\mathrm{H}_{2} \mathrm{O}$
b. three.twenty $\mathrm{g} \mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}$ in 1.00 $\mathrm{kg} \mathrm{H}_{ii} \mathrm{O}$
c. xx.0 $\mathrm{k} \mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{eleven}$ (sucrose) in $500 . \mathrm{g} \mathrm{H}_{ii} \mathrm{O}$
Emily H.
Numerade Educator
Problem 26
Given the post-obit humid points, decide the molality of each water solution.
$$
\begin{array}{l}{\text { a. } 100.25^{\circ} \mathrm{C}} \\ {\text { b. } 101.53^{\circ} \mathrm{C}} \\ {\text { c. } 102.805^{\circ} \mathrm{C}}\stop{array}
$$
Emily H.
Numerade Educator
Problem 27
Given 1.00 $\mathrm{m}$ aqueous solutions of each of the post-obit electrolytic substances, decide the expected change in the freezing point of the solvent.
(Hint: See Sample Problem F.)
a. $\mathrm{KI}$
b. CaCl_
c. $\mathrm{Ba}\left(\mathrm{NO}_{iii}\right)_{2}$
Emily H.
Numerade Educator
Trouble 28
What is the expected alter in the freezing point of h2o for a 0.015 m aqueous solution of AlCl $_{3} ?$
Emily H.
Numerade Educator
Problem 29
What is the expected freezing bespeak of a solution containing 85.0 g NaCl dissolved in $450 .$ thousand of water?
Emily H.
Numerade Educator
Trouble 30
Decide the expected boiling point of a solution made by dissolving 25.0 $\mathrm{one thousand}$ of barium chloride in 0.150 $\mathrm{kg}$ of water.
Emily H.
Numerade Educator
Problem 31
The modify in the boiling indicate of water for an aqueous solution of potassium iodide is $0.65^{\circ} \mathrm{C}$ Determine the molal concentration of potassium iodide.
Emily H.
Numerade Educator
Problem 32
The freezing betoken of an aqueous solution of barium nitrate is $-2.65^{\circ} \mathrm{C}$ . Determine the molal concentration of barium nitrate.
Emily H.
Numerade Educator
Trouble 33
Calculate the expected freezing betoken of a solution containing 1.00 $\mathrm{kg} \mathrm{H}_{ii} \mathrm{O}$ and 0.250 $\mathrm{mol} \mathrm{NaCl} .$
Emily H.
Numerade Educator
Trouble 34
Experimental data for a 1.00 $\mathrm{yard} \mathrm{MgI}_{ii}$ aqueous solution indicate an actual change in the freezing indicate of h2o of $-4.78^{\circ} \mathrm{C}$ . Detect the expected change in the freezing betoken of water. Propose 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 following, suit the solutions in order of increasing
change in the freezing point of the solution.
a. Nal
b. CaCl_s
c. $\mathrm{Thou}_{3} \mathrm{PO}_{4}$
d. $\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}$ (glucose)
Emily H.
Numerade Educator
Trouble 36
What is the molal concentration of an aqueous calcium chloride solution that freezes at $-2.43^{\circ} \mathrm{C}$ ?
Emily H.
Numerade Educator
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 $1.iii,$ decide whether there is
a precipitate.
c. Does this reaction occur?
Emily H.
Numerade Educator
Problem 38
Write a counterbalanced equation to bear witness what occurs when hydrogen bromide dissolves and reacts with water.
Include a hydronium ion in the equation.
Emily H.
Numerade Educator
Trouble 39
Write the equation for the dissolution of each of the following in h2o, and then indicate the total number of moles of solute ions formed.
a. 0.275 mol of potassium sulfide
b. 0.15 mol of aluminum sulfate
Emily H.
Numerade Educator
Problem 40
Calculate the expected change in the boiling betoken of h2o in a solution made up of 131.2 $\mathrm{chiliad}$ of silver nitrate, $\mathrm{AgNO}_{3}$ , in 2.00 $\mathrm{kg}$ of water.
Emily H.
Numerade Educator
Problem 41
Nitrous acid, HNO, is a weak electrolyte. Nitric acid, $\mathrm{HNO}_{iii},$ is a strong electrolyte. Write equations to correspond the ionization of each in water. Include the hydronium ion, and prove the appropriate kind of pointer in each equation.
Emily H.
Numerade Educator
Problem 42
Find the boiling point of an aqueous solution containing a nonelectrolyte that freezes at $-6.51^{\circ} \mathrm{C} .$
Emily H.
Numerade Educator
Problem 43
Write a balanced equation for the dissolution of sodium carbonate, $\mathrm{Na}_{2} \mathrm{CO}_{three},$ in h2o. Find the number of moles of each ion produced when 0.20 $\mathrm{mol}$ of sodium carbonate dissolves. Then, detect the total number of moles of ions.
Emily H.
Numerade Educator
Problem 44
Given the reaction below and the information in Figure $i.3,$ write the internet ionic equation for the reaction. potassium phosphate $(a q)+\operatorname{pb}(\mathrm{II})$ nitrate $(a q)$
Emily H.
Numerade Educator
Problem 45
Find the expected freezing point of a h2o solution that contains 268 $\mathrm{k}$ of aluminum nitrate, $\mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}$ in viii.50 $\mathrm{kg}$ of water.
Emily H.
Numerade Educator
Trouble 46
Applying Models
a. You are conducting a freezing-point decision in the laboratory by using an aqueous solution of $\mathrm{KNO}_{three}$ . The observed freezing point of the solution is $-ane.15^{\circ} \mathrm{C} .$ Using a pure water sample, you lot recorded the freezing point of the pure solvent on the same thermometer as $0.25^{\circ} \mathrm{C}$ . Determine 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 office (a) because yous suspect that you should not ignore
the effect of ion interaction. Yous take a 10.00 $\mathrm{mL}$ sample of the solution. Afterwards carefully evaporating the water from the solution, yous obtain 0.415 $\mathrm{g}$ KNO. Determine the bodily molal concentration of KNO $_{3}$ and the percentage departure between the concentration observed in the freezing-betoken determination and the bodily concentration of $\mathrm{KNO}_{3}$ . Assume that the solution's density is ane.00 $\mathrm{g} / \mathrm{mL}$ .
Emily H.
Numerade Educator
Problem 47
Analyzing Data The observed freezing-point 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?
Emily H.
Numerade Educator
Problem 48
Analyzing Information The osmotic pressure of a dilute solution can be calculated as follows:
$\pi=Thou R T$
$\pi=$ osmotic pressure
$M=$ concentration in moles per liter
$R=$ ideal gas abiding
$T=$ absolute temperature of the solution
How does the osmotic-force per unit area equation compare with the platonic gas police force?
Emily H.
Numerade Educator
Problem 49
Mutual reactions for Group xiii elements are found in the Elements Handbook (Appendix A). Review this
material, and answer the following:
a. Write net ionic equations for each of the case reactions listed under "Mutual Reactions" for
Group 13.
b. Which reactions did non change when written in net ionic form? Why?
Problem l
Common reactions for Group 14 elements are plant in the Elements Handbook (Appendix A). Review this
material, and respond the post-obit:
a. Write net ionic equations for each of the example reactions listed under "Common Reactions" for
Group 14.
b. Which reactions did not change when written in net ionic form? Why?
Problem 51
Detect out how much table salt a large northern city, such equally New York City or Chicago, uses on its streets in a
typical winter. What environmental problems result from this use of salt? What substitutes for salt are
existence used to cook ice and snow?
Emily H.
Numerade Educator
Problem 52
Enquiry the role of electrolytes and electrolytic solutions in your body. Notice out how electrolytes work in the functioning of nerves and muscles. What are some of the health problems that tin ascend from an imbalance of electrolytes in body fluids?
Problem 53
Performance Determine the freezing point of iv different mixtures of water and ethylene glycol (utilise
commercial antifreeze). What mixture has the everyman freezing point?
Emily H.
Numerade Educator
Problem 54
Functioning Find the optimum mixture of salt and ice for reducing the temperature of the chilling bath
for an ice-cream freezer. Employ your data to write a gear up of instructions on how to gear up the chilling bath for making ice cream.
Trouble 55
Performance Using a low-voltage dry prison cell, get together a conductivity apparatus. Secure several unknown
aqueous solutions of equal molality from your teacher, and employ the apparatus to distinguish the
electrolytes from the nonelectrolytes. Amongst 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 activity, explain how
you could utilise the freezing-point low concept to distinguish the electrolytes from the nonelectrolytes. Explain how you could determine the number of ions independent per molecule among the solutes identified as electrolytes. Design and carry an experiment to test your theories.
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