9.E: Exercises
- Page ID
- 438384
\( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}} } \)
\( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash {#1}}} \)
\( \newcommand{\dsum}{\displaystyle\sum\limits} \)
\( \newcommand{\dint}{\displaystyle\int\limits} \)
\( \newcommand{\dlim}{\displaystyle\lim\limits} \)
\( \newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\)
( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\)
\( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\)
\( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\)
\( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\)
\( \newcommand{\Span}{\mathrm{span}}\)
\( \newcommand{\id}{\mathrm{id}}\)
\( \newcommand{\Span}{\mathrm{span}}\)
\( \newcommand{\kernel}{\mathrm{null}\,}\)
\( \newcommand{\range}{\mathrm{range}\,}\)
\( \newcommand{\RealPart}{\mathrm{Re}}\)
\( \newcommand{\ImaginaryPart}{\mathrm{Im}}\)
\( \newcommand{\Argument}{\mathrm{Arg}}\)
\( \newcommand{\norm}[1]{\| #1 \|}\)
\( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\)
\( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\AA}{\unicode[.8,0]{x212B}}\)
\( \newcommand{\vectorA}[1]{\vec{#1}} % arrow\)
\( \newcommand{\vectorAt}[1]{\vec{\text{#1}}} % arrow\)
\( \newcommand{\vectorB}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}} } \)
\( \newcommand{\vectorC}[1]{\textbf{#1}} \)
\( \newcommand{\vectorD}[1]{\overrightarrow{#1}} \)
\( \newcommand{\vectorDt}[1]{\overrightarrow{\text{#1}}} \)
\( \newcommand{\vectE}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{\mathbf {#1}}}} \)
\( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}} } \)
\(\newcommand{\longvect}{\overrightarrow}\)
\( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash {#1}}} \)
\(\newcommand{\avec}{\mathbf a}\) \(\newcommand{\bvec}{\mathbf b}\) \(\newcommand{\cvec}{\mathbf c}\) \(\newcommand{\dvec}{\mathbf d}\) \(\newcommand{\dtil}{\widetilde{\mathbf d}}\) \(\newcommand{\evec}{\mathbf e}\) \(\newcommand{\fvec}{\mathbf f}\) \(\newcommand{\nvec}{\mathbf n}\) \(\newcommand{\pvec}{\mathbf p}\) \(\newcommand{\qvec}{\mathbf q}\) \(\newcommand{\svec}{\mathbf s}\) \(\newcommand{\tvec}{\mathbf t}\) \(\newcommand{\uvec}{\mathbf u}\) \(\newcommand{\vvec}{\mathbf v}\) \(\newcommand{\wvec}{\mathbf w}\) \(\newcommand{\xvec}{\mathbf x}\) \(\newcommand{\yvec}{\mathbf y}\) \(\newcommand{\zvec}{\mathbf z}\) \(\newcommand{\rvec}{\mathbf r}\) \(\newcommand{\mvec}{\mathbf m}\) \(\newcommand{\zerovec}{\mathbf 0}\) \(\newcommand{\onevec}{\mathbf 1}\) \(\newcommand{\real}{\mathbb R}\) \(\newcommand{\twovec}[2]{\left[\begin{array}{r}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\ctwovec}[2]{\left[\begin{array}{c}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\threevec}[3]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\cthreevec}[3]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\fourvec}[4]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\cfourvec}[4]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\fivevec}[5]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\cfivevec}[5]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\mattwo}[4]{\left[\begin{array}{rr}#1 \amp #2 \\ #3 \amp #4 \\ \end{array}\right]}\) \(\newcommand{\laspan}[1]{\text{Span}\{#1\}}\) \(\newcommand{\bcal}{\cal B}\) \(\newcommand{\ccal}{\cal C}\) \(\newcommand{\scal}{\cal S}\) \(\newcommand{\wcal}{\cal W}\) \(\newcommand{\ecal}{\cal E}\) \(\newcommand{\coords}[2]{\left\{#1\right\}_{#2}}\) \(\newcommand{\gray}[1]{\color{gray}{#1}}\) \(\newcommand{\lgray}[1]{\color{lightgray}{#1}}\) \(\newcommand{\rank}{\operatorname{rank}}\) \(\newcommand{\row}{\text{Row}}\) \(\newcommand{\col}{\text{Col}}\) \(\renewcommand{\row}{\text{Row}}\) \(\newcommand{\nul}{\text{Nul}}\) \(\newcommand{\var}{\text{Var}}\) \(\newcommand{\corr}{\text{corr}}\) \(\newcommand{\len}[1]{\left|#1\right|}\) \(\newcommand{\bbar}{\overline{\bvec}}\) \(\newcommand{\bhat}{\widehat{\bvec}}\) \(\newcommand{\bperp}{\bvec^\perp}\) \(\newcommand{\xhat}{\widehat{\xvec}}\) \(\newcommand{\vhat}{\widehat{\vvec}}\) \(\newcommand{\uhat}{\widehat{\uvec}}\) \(\newcommand{\what}{\widehat{\wvec}}\) \(\newcommand{\Sighat}{\widehat{\Sigma}}\) \(\newcommand{\lt}{<}\) \(\newcommand{\gt}{>}\) \(\newcommand{\amp}{&}\) \(\definecolor{fillinmathshade}{gray}{0.9}\)What is a Solution?
A solution is composed of two main components called __________ and ___________.
Identify the solute and solvent in a 1 liter aqueous solution that contains 126.0 g sodium bicarbonate.
a. Solute: ________________
b. Solvent: ________________
Which of the following is not an example of a solution?
a. Gas in a gas
b. Gas in a liquid
c. Liquid in a liquid
d. Solid in a liquid
e. Solid in a solid
f. All of these are valid.
Given that water, ethanol, and methanol are polar while benzene, hexanes and methylene chloride are non-polar, state if the following combinations are miscible (form a solution) or immiscible (do not form a solution).
a. methylene chloride and water
b. hexanes and benzene
c. water and ethanol
d. methanol and hexanes
Water, a polar substances mixes with acetonitrile. This means that acetonitrile is _________ (polar or non-polar?).
Matching: Match the scenarios describe in each diagram with the following conditions.
diagram 1
diagram 2a. A nonpolar solute and a nonpolar solvent (diagram 1)
b. A nonpolar solute and a polar solvent (diagram 2)
c. A polar solute and a polar solvent (diagram 1)
Below is the structure of acetyl chloride, drawn with bonds and electron dots. Will acetyl chloride form a solution in ethanol a polar solvent?
a. Yes, because acetyl chloride is a non-polar molecule
b. Yes, because acetyl chloride is a polar molecule
c. No, because acetyl chloride is a non-polar molecule
d. No, because acetyl chloride is an ionic compound
(Multi section) Which of the following would be considered liquid solutions?
a. Air
b. Gatorade
c. Sprite
d. Tincture of Iodine
e. Brass
Which of the following would be considered a solid solution?
a. Air
b. Gatorade
c. Sprite
d. Tincture of Iodine
e. Brass
(Multi select) Which of the following would have water as a solvent within the solution?
a. Air
b. Gatorade
c. Sprite
d. Tincture of Iodine
e. Brass
Which of the following would not be considered a solution?
a. Air
b. Coca-cola
c. Normal Saline IV drip
d. Pepto bismol
e. Bronze
Which of the following solutes will dissolve in heptane, a nonpolar solvent?
a. \(\ce{NaCl}\)
b. Wax
c. Water
d. Ethanol
Electrolytes and nonelectrolytes
Indicate if each of the following compounds would form a strong, weak, or a nonelectrolyte.
a. \(\ce{Na2SO4}\): __________
b. Sucrose, \(\ce{C12H22O11}\): __________
c. Acetic acid, \(\ce{HC2H3O2}\): __________
Classify the following equations as representations of strong, weak or non-electrolyte:
a. \(\ce{CH3CH2OH} (l) \xrightarrow{\ce{H2O}} \ce{CH3CH2OH} (aq) \)
b. \( \ce{NaNO3} (s) \xrightarrow{\ce{H2O}} \ce{Na^+} (aq) + \ce{NO3^-} (aq) \)
c. \(\ce{NH3} (g) + \ce{H2O} (l) \rightleftarrows \ce{NH4^+} (aq) + \ce{OH^-} (aq) \)
How many equivalents are in 1.5 moles of \(\ce{Fe^{2+}}\)?
a. 0.5 Eq
b. 1.0 Eq
c. 2.0 Eq
d. 2.5 Eq
e. 3.0 Eq
How many equivalents of \(\ce{K^+}\) and \(\ce{SO4^{2-}}\) are in 1.0 L of 1.0 M solution of \(\ce{K2SO4}\)?
The concentration of \(\ce{Ca^{2+}}\) in \(\ce{CaCl2}\) solution is 42 mEq/L. What is a molar concentration (mmol/L, mM) of \(\ce{Ca^{2+}}\)?
A Ringer’s solution consists of 140 mEq/L \(\ce{Na^+}\), 5 mEq/L \(\ce{K^+}\), 4 mEq/L \(\ce{Ca^{2+}}\), and \(\ce{Cl^-}\). What is the \(\ce{Cl^-}\) concentration in mEq/L?
To test whether solutes are electrolytes or non-electrolytes, a student can use an apparatus that consists of a battery and a pair of electrodes connected through wires to a light bulb. The light bulb glows when electricity flows. This tells the presence of ions provided by electrolytes. What is the process of providing ions?
Soluble and Insoluble Ionic Compounds
Table \(\PageIndex{1}\): Solubility Rules for Ionic Compounds in Water
| An ionic compound is soluble in water if it contains one of the following: | |
|---|---|
| Positive Ions | \(\ce{Li^+, Na^+, K^+, Rb^+, Cs^+, NH4^+}\) |
| Negative Ions |
\(\ce{NO3^{-}, C2H3O2^{-}} \) \(\ce{Cl^{-}, Br^{-}, I^{-}}\) except when combined with \(\ce{Ag^+, Pb^{2+},}\) or \(\ce{Hg2^{2+}}\) \(\ce{SO4^{2-}}\) except when combined with \(\ce{Ba^{2+}, Pb^{2+}, Ca^{2+}, Sr^{2+},}\) or \(\ce{Hg2^{2+}}\) |
| Ionic compounds that do not contain at least one of these ions are usually insoluble. |
Use the solubility rules to predict if the following compounds are soluble or insoluble.
a. \(\ce{NaCl}\)
b. \(\ce{CuS}\)
c. \(\ce{AgCl}\)
d. \(\ce{KNO3}\)
Use the solubility rules to predict which of the following compounds is insoluble?
a. \(\ce{NaNO3}\)
b. \(\ce{Na2S}\)
c. \(\ce{(NH4)2SO4}\)
d. \(\ce{Pb(C2H3O2)2}\)
Use the solubility rules to predict which of the following compounds is insoluble?
a. \(\ce{CaSO4}\)
b. \(\ce{KCl}\)
c. \(\ce{RbBr}\)
d. \(\ce{AgNO3}\)
Use the solubility rules to predict which of the following compounds is insoluble?
a. \(\ce{LiCl}\)
b. \(\ce{CsBr}\)
c. \(\ce{BaSO4}\)
d. \(\ce{NaC2H3O2}\)
Does an insoluble compound form when solutions of \(\ce{Ca(NO3)2}\) and \(\ce{K2SO4}\) are mixed? If so, what is the name of a precipitate?
Which one does not form a solid when solutions containing the following ionic compounds are mixed?
a. \(\ce{KCl}\) (aq) and \(\ce{Na2S}\) (aq)
b. \(\ce{AgNO3}\) (aq) and \(\ce{K2S}\) (aq)
c. \(\ce{CaCl2}\) (aq) and \(\ce{Na2SO4}\) (aq)
d. \(\ce{CuCl2}\) (aq) and \(\ce{Li3PO4}\) (aq)
Determine whether each compound is soluble or insoluble in water:
a. \(\ce{NaNO3}\): __________
b. \(\ce{PbCl2}\): __________
c. \(\ce{Mg(OH)2}\): __________
The graph below shows how temperature affects the solubility of select compound. Answer the questions that follow using this graph.
a. Identify the substance whose solubility is least affected by temperature.
b. Identify an ionic compound whose solubility decreases with increasing temperature.
c. Identify the compound with the highest solubility at 20 \(^{\circ}\)C.
d. How many grams of \(\ce{KNO3}\) will dissolve in 100 g \(\ce{H2O}\) at 70 \(^{\circ}\)C?
e. Use the graph to rank these solutes in order of increasing solubility, lowest (1) and highest (4) at 10 \(^{\circ}\)C.
| Solute | Rank |
|---|---|
| \(\ce{NaNO3}\) | |
| \(\ce{KNO3}\) | |
| \(\ce{KI}\) | |
| \(\ce{KClO3}\) |
Based on the associated solubility chart, at what temperature would you need to heat a solution of \(\ce{KCl}\) to dissolve 60.0 g of \(\ce{KCl}\) in 120.0 g of \(\ce{H2O}\)?
a. 10 \(^{\circ}\)C
b. 40 \(^{\circ}\)C
c. 60 \(^{\circ}\)C
d. 75 \(^{\circ}\)C
e. 100 \(^{\circ}\)C
Which of the following represents the net ionic equation for the reaction between \(\ce{CuCl2}\) (aq) and \(\ce{Li3PO4}\) (aq)?
a. \(3\ce{Cu^{2+}} (aq) + 2 \ce{PO4^{3-}} (aq) \rightarrow \ce{Cu3(PO4)2} (s)\)
b. \(3\ce{Cu} (s) + 2\ce{PO4} (s) \rightarrow \ce{Cu3(PO4)2} (s) \)
c. \(\ce{Cu^{2+}} (aq) + \ce{PO4^{3-}} (aq) \rightarrow \ce{Cu3(PO4)2} (s) \)
d. \(\ce{Cu^{2+}} (aq) + \ce{PO4^{3-}} (aq) \rightarrow \ce{CuPO4} (s) \)
e. No solid forms
Solution Concentration and Reactions
Determine the molarity of a solution prepared by dissolving 11.5 g \(\ce{NaOH}\) to form 250 mL solution.
A \(\ce{CaCl2}\) solution is administered to patients to increase their blood calcium levels. If a patient’s recommended dose is 1.50 g \(\ce{CaCl2}\), how many milliliters of a 20.0% (m/v) \(\ce{CaCl2}\) solution should the patient receive?
The pain reliever acetaminophen is sold as an oral suspension of Tylenol:
What is the mass/volume percent of acetaminophen?
a. 3.2% m/V
b. 32% m/V
c. 5.1% m/V
d. 8.3% m/V
A doctor orders 5.0 mg of Compazine, used to treat nausea and migraines. If the stock solution on hand is 2.5% (m/v), how many milliliters are administered to the patient?
a. 0.20 mL
b. 0.10 mL
c. 0.012 mL
d. 200 mL
e. 2 mL
Use the graph to answer the following questions? Note read graph carefully and apply concepts: What is the mass percent of \(\ce{NH4Cl}\) per 100 g water at 60 \(^{\circ}\)C?
a. 35%
b. 22%
c. 55%
d. 280%
How many mL of a 2.50 M \(\ce{K2SO4}\) solution are required to obtain 1.20 moles of \(\ce{K2SO4}\)?
a. 3.00 mL
b. 208 mL
c. 480 mL
d. 2.08 mL
e. 0.480 mL
Diuril is a prescription drug used to treat hypertension. You are given a 2.5 g vial of Diuril of negligible volume and asked to prepare a solution by combining with 20.0 mL of sterile water. What is the final concentration in mg/mL?
a. 0.01 mg/mL
b. 0.05 mg/mL
c. 0.125 mg/mL
d. 125 mg/mL
e. 250 mg/mL
A bottle contains 72 mL of vanilla extract solution. If the solution contains 59 mL of alcohol, what is the volume percent (v/v) of the alcohol in the extract solution?
What is the molarity of a solution containing 25.5 g \(\ce{KBr}\) dissolved in enough water to make 1.75 L of solution?
Complete and balance each equation. If no reaction occurs, write NO REACTION:
a. \(\ce{K2CO3} (aq) + \ce{AgF} (aq) \rightarrow \)
b. \(\ce{LiOH} (aq) + \ce{AlCl3} (aq) \rightarrow \)
c. \(\ce{(NH4)2SO4} (aq) + \ce{CuNO3} (aq) \rightarrow \)
For the following reaction, how many mL of 0.200 M \(\ce{NaOH}\) solution are needed to react with 18.0 mL of a 0.500 M \(\ce{NiCl2}\) solution?
\[\ce{NiCl2} (aq) + 2\ce{NaOH} (aq) \rightarrow \ce{Ni(OH)2} (s) + 2\ce{NaCl} (aq) \nonumber\]
a. 180 mL
b. 18.0 mL
c. 45.0 mL
d. 36.0 mL
e. 90.0 mL
Dilution of Solutions
To what volume should you dilute 25 mL of an 18.0 M solution of \(\ce{H2SO4}\) to obtain a 0.75 M solution?
What is the molarity (M) of a solution prepared by diluting 125 mL of 0.500 M \(\ce{H2SO4}\) to 375 mL?
You are asked to prepare a bolus IV injection of a new, experimental MRI contrast agent. The reconstituted stock solution of the contrast agent has a concentration of 0.60 M. What volume of the stock solution do you need in order to prepare 5.0 mL of 0.20 M contrast agent?
a. 0.60 mL
b. 1.7 mL
c. 1.5 mL
d. 15 mL
e. 1.0 mL
How much water needs to be added to a 300 mL of 3.0 M solution to obtain a final solution with 2.0 M?
Which of the following is not affected by the process of dilution?
a. Concentration
b. Volume
c. The amount of solute
d. The amount of solvent
Properties of Solutions
A red blood cell has been placed into three different solutions (isotonic, hypotonic and hypertonic). Match each image that follows to correct solution in which the red blood cell is placed in.
a. 
b. 
c. 
Rank the solutions in order of increasing boiling point with lowest (1) and highest (4).
a. 1 mole of \(\ce{LiCl}\) in 1.5 L of water: __________
b. 1 mole of \(\ce{BaCl2}\) in 1.5 L water: __________
c. 1 mole of \(\ce{AlCl3}\) in 1.5 L water: __________
d. 1 mole of glucose (\(\ce{C6H12O6}\)) in 1.5 L water: __________
Considering the \(\ce{NaCl}\) salt concentration in a cell is 0.9% Indicate if each of the following solutions is isotonic, hypotonic, or hypertonic.
a. 2% \(\ce{NaCl}\) solution: __________
b. 2% glucose solution: __________
c. 0.5% \(\ce{NaCl}\) solution: __________
d. 5% glucose solution: __________
e. 0.9% \(\ce{NaCl}\) solution: __________
f. 20% glucose solution: __________
Which of the following is not correct about suspensions?
a. Suspensions have very large particles that may be visible.
b. The particles settle slowly.
c. Particles can be separated by filters.
d. Kaopectate and calamine lotion are suspensions.