4.13: Assignment—Chemical Reactions in Aqueous Solution
- Page ID
- 233014
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\(\newcommand{\avec}{\mathbf a}\) \(\newcommand{\bvec}{\mathbf b}\) \(\newcommand{\cvec}{\mathbf c}\) \(\newcommand{\dvec}{\mathbf d}\) \(\newcommand{\dtil}{\widetilde{\mathbf d}}\) \(\newcommand{\evec}{\mathbf e}\) \(\newcommand{\fvec}{\mathbf f}\) \(\newcommand{\nvec}{\mathbf n}\) \(\newcommand{\pvec}{\mathbf p}\) \(\newcommand{\qvec}{\mathbf q}\) \(\newcommand{\svec}{\mathbf s}\) \(\newcommand{\tvec}{\mathbf t}\) \(\newcommand{\uvec}{\mathbf u}\) \(\newcommand{\vvec}{\mathbf v}\) \(\newcommand{\wvec}{\mathbf w}\) \(\newcommand{\xvec}{\mathbf x}\) \(\newcommand{\yvec}{\mathbf y}\) \(\newcommand{\zvec}{\mathbf z}\) \(\newcommand{\rvec}{\mathbf r}\) \(\newcommand{\mvec}{\mathbf m}\) \(\newcommand{\zerovec}{\mathbf 0}\) \(\newcommand{\onevec}{\mathbf 1}\) \(\newcommand{\real}{\mathbb R}\) \(\newcommand{\twovec}[2]{\left[\begin{array}{r}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\ctwovec}[2]{\left[\begin{array}{c}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\threevec}[3]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\cthreevec}[3]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\fourvec}[4]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\cfourvec}[4]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\fivevec}[5]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\cfivevec}[5]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\mattwo}[4]{\left[\begin{array}{rr}#1 \amp #2 \\ #3 \amp #4 \\ \end{array}\right]}\) \(\newcommand{\laspan}[1]{\text{Span}\{#1\}}\) \(\newcommand{\bcal}{\cal B}\) \(\newcommand{\ccal}{\cal C}\) \(\newcommand{\scal}{\cal S}\) \(\newcommand{\wcal}{\cal W}\) \(\newcommand{\ecal}{\cal E}\) \(\newcommand{\coords}[2]{\left\{#1\right\}_{#2}}\) \(\newcommand{\gray}[1]{\color{gray}{#1}}\) \(\newcommand{\lgray}[1]{\color{lightgray}{#1}}\) \(\newcommand{\rank}{\operatorname{rank}}\) \(\newcommand{\row}{\text{Row}}\) \(\newcommand{\col}{\text{Col}}\) \(\renewcommand{\row}{\text{Row}}\) \(\newcommand{\nul}{\text{Nul}}\) \(\newcommand{\var}{\text{Var}}\) \(\newcommand{\corr}{\text{corr}}\) \(\newcommand{\len}[1]{\left|#1\right|}\) \(\newcommand{\bbar}{\overline{\bvec}}\) \(\newcommand{\bhat}{\widehat{\bvec}}\) \(\newcommand{\bperp}{\bvec^\perp}\) \(\newcommand{\xhat}{\widehat{\xvec}}\) \(\newcommand{\vhat}{\widehat{\vvec}}\) \(\newcommand{\uhat}{\widehat{\uvec}}\) \(\newcommand{\what}{\widehat{\wvec}}\) \(\newcommand{\Sighat}{\widehat{\Sigma}}\) \(\newcommand{\lt}{<}\) \(\newcommand{\gt}{>}\) \(\newcommand{\amp}{&}\) \(\definecolor{fillinmathshade}{gray}{0.9}\)To download a copy of the assignment, please click on the link Sample Questions. (Question 17 in the PDF has an error; see question 17 below.)
As you work these matter and measurement problems, consider and explain:
- What type of question is it?
- How do you know what type of question it is?
- What information are you looking for?
- What information do they give?
- How will you go about solving this?
- Show how to solve the problem.
- Be able to answer for a different reaction, number, set of conditions, etc.
Sample Questions
- Consider two organic molecules, ethanol and benzene. One dissolves in water and the other does not. Why?
- They have different molar masses.
- One is ionic, the other is not.
- One is an electrolyte, the other is not.
- Ethanol contains a polar O–H bond, and benzene does not.
- Two of these are correct.
- Which of the following is a strong acid?
- HF
- KOH
- HClO4
- HClO
- HBrO
- Which of the following is not a strong base?
- Ca(OH)2
- KOH
- NH3
- LiOH
- Sr(OH)2
- 1.00 mL of a 2.90 × 10–4M solution of oleic acid is diluted with 9.00 mL of petroleum ether, forming solution A. Then 2.00 mL of solution A is diluted with 8.00 mL of petroleum ether, forming solution B. What is the concentration of solution B?
- 2.90 × 10–6M
- 8.06 × 10–6M
- 5.80 × 10–5M
- 6.44 × 10–5M
- 5.80 × 10–6M
- How many grams of NaCl are contained in 350. mL of a 0.196 M solution of sodium chloride?
- 11.5 g
- 4.01 g
- 8.02 g
- 68.6 g
- none of these
- What volume of 18 M sulfuric acid must be used to prepare 2.00 L of 0.140 M H2SO4
- 16 mL
- 0.28 mL
- 1.3 × 103 mL
- 2.8 mL
- 5.0 mL
- What are the following reactions examples of?
Pb2+ + 2I–→ PbI2
2Ce4+ + 2I– → I2 + 2Ce3+
HOAc + NH3 → NH4+ + OAc–- acid-base reactions
- unbalanced reactions
- precipitation, acid-base, and redox reactions, respectively
- redox, acid-base, and precipitation reactions, respectively
- precipitation, redox, and acid-base reactions, respectively
- You have exposed electrodes of a light bulb in a solution of H2SO4 such that the light bulb is on. You add a dilute solution and the bulb grows dim. Which of the following could be in the solution?
- Ba(OH)2
- NaNO3
- K2SO4
- Cu(NO3)2
- none of these
- Aqueous solutions of potassium sulfate and ammonium nitrate are mixed together. Which statement is correct?
- Both KNO3 and NH4SO4 precipitate from solution.
- A gas is released.
- NH4SO4 will precipitate from solution.
- KNO3 will precipitate from solution.
- No reaction will occur.
- How many of the following salts are expected to be insoluble in water?
- sodium sulfide
- barium nitrate
- ammonium sulfate
- potassium phosphate
- none
- 1
- 2
- 3
- 4
- Which of the following ions is most likely to form an insoluble sulfate?
- K+
- Li+
- Ca2+
- S2–
- Cl–
Use the following to answer questions 12–13: Aqueous solutions of barium chloride and silver nitrate are mixed to form solid silver chloride
and aqueous barium nitrate.
- The balanced molecular equation contains which one of the following terms?
- AgCl (s)
- 2AgCl (s)
- 2Ba(NO3)2 (aq)
- BaNO3 (aq)
- 3AgCl (aq)
- The net ionic equation contains which of the following terms?
- Ag+(aq)
- Ba2+(aq)
- NO3– (aq)
- H+ (aq)
- AgCl (aq)
- The net ionic equation for the reaction of calcium bromide and sodium phosphate contains which of the following species?
- 2Br– (aq)
- PO43– (aq)
- 2Ca3(PO4)2(s)
- 6NaBr (aq)
- 3Ca2+ (aq)
- The net ionic equation for the reaction of aluminum sulfate and sodium hydroxide contains which of the following species?
- 3Al3+(aq)
- OH– (aq)
- 3OH– (aq)
- 2Al3+(aq)
- 2Al(OH)3(s)
- You mix 265.0 mL of 1.20 M lead(II) nitrate with 300.0 mL of 1.55 M potassium iodide. The lead(II) iodide is insoluble. Which of the following is false?
- The final concentration of Pb2+ ions is 0.151 M.
- You form 107 g of lead(II) iodide.
- The final concentration of K+ is 0.823 M.
- The final concentration of NO3– is 0.823 M.
- All are true.
- When solutions of formic acid and sodium hydroxide react, which of the following are NOT present in the net ionic equation?
- hydrogen ion
- formate ion
- sodium ion
- hydroxide ion
- A and B
- A, B, and C
- A and D
- A and C
- B and C
- When solutions of acetic acid and copper(II) react, which of the following are spectator ions?
- hydrogen ion
- acetate ion
- copper(II) ion
- hydroxide ion
- none of these
- A 0.307-g sample of an unknown triprotic acid is titrated to the third equivalence point using 35.2 mL of 0.106 M NaOH. Calculate the molar mass of the acid.
- 247 g/mol
- 171 g/mol
- 165 g/mol
- 151 g/mol
- 82.7 g/mol
- You have separate solutions of HCl and H2SO4 with the same concentrations in terms of molarity. You wish to neutralize a solution of NaOH. Which acid solution would require more volume (in mL) to neutralize the base?
- The HCl solution.
- The H2SO4 solution.
- You need to know the acid concentrations to answer this question.
- You need to know the volume and concentration of the NaOH solution to answer this question.
- C and D
- With what volume of 5.00 M HF will 5.41 g of calium hydroxide react completely, according to the following reaction?
2 HF + Ca(OH)2 → CaF2 + 2H2O- 14.6 mL
- 146 mL
- 730 mL
- 29.2 mL
- 34.2 mL
- A student weighs out 0.557 g of KHP (molar mass = 204.22 g/mol) and titrates to the equivalence point with 36.78 mL of a stock NaOH solution. What is the concentration of the stock NaOH solution? KHP is an acid with one acidic proton.
- 0.00273 M
- 0.100 M
- 0.0151 M
- 0.0742 M
- none of these
- In which of the following does nitrogen have an oxidation state of +4?
- HNO3
- NO2
- N2O
- NH4Cl
- NaNO2
- What is the oxidation state of chlorine in ClO–?
- 0
- +1
- –1
- +3
- –7
- In the reaction 2Ca(s) + O2(g) → 2CaO(s), which species is oxidized?
- O2
- O2–
- Ca
- Ca2+
- none of these
- In the reaction N2(g) + 3H2(g) → 2NH3(g), N2 is
- oxidized
- reduced
- the electron donor
- the reducing agent
- two of these
- Which of the following are oxidation-reduction reactions?
- PCl3 + Cl2 → PCl5
- Cu + 2AgNO3 → Cu(NO3)2 + 2Ag
- CO2 + 2LiOH → Li2CO3 + H2O
- FeCl2 + 2NaOH → Fe(OH)2 + 2NaCl
- III
- IV
- I and II
- I, II, and III
- I, II, III, and IV
- In the reaction Zn + H2SO4 → ZnSO4 + H2, which, if any, element is oxidized?
- zinc
- hydrogen
- sulfur
- oxygen
- none of these
- Balance the following oxidation-reduction reaction using the oxidation number method: Fe3+ + I– → Fe2+ + I2
In the balanced equation, the coefficient of Fe2+ + I2- 1
- 2
- 3
- 4
- none of these
- Given the reaction 2MnO4- + 5H2O2 + 6H+ 2Mn2+ + 8H2O + 5O2 determine the number of electrons involved in this reaction.
- 10
- 8
- 6
- 4
- 2
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- Authored by: Jessica Garber. Provided by: Tidewater Community College. License: CC BY: Attribution