Deck 8: Aqueous Solutions Chemistry of the Hydrosphere

Question 1

You make a solution of fuming nitric acid HNO₃, 63.02 g/mol), which has a density of 1.50 g/mL and contains 90.0% HNO₃ by mass.Calculate the theoretical molarity of water in this solution.

A)21.4 M
B)2.14 M
C)8.32 M
D)0.150 M
E)0.832 M

Answer 1

8.32 M

Question 2

How many grams of glucose (C₆H₁₂O₆, 180.16 g/mol) would be required to prepare 2.50 L of a 0.278 M glucose solution that could be used in an IV bag?

A)6.95* 10²g
B)1.11 * 10²g
C)5.01 * 10¹g
D)4.50 * 10²g
E)1.25 * 10²g

Answer 2

1.25 * 10²g

Question 3

If there are 0.505 g of NaCl 58.44 g/mol) left in a beaker that originally contained 75.0 mL of saltwater, what must have been the concentration of the original solution?

A)0.00647 M
B)0.0115 M
C)0.0673 M
D)0.115 M
E)0.673 M

Answer 3

0.115 M

Question 4

What volume of 2.50 M NaOH 40.00 g/mol) contains 0.100 mole of NaOH?

A)0.250 L
B)40.0 mL
C)25.0 mL
D)0.250 mL
E)0.0400 mL

Question 5

A homogeneous mixture of two or more substances is called

A)a compound.
B)an electrolyte.
C)a solution.
D)a solvent.
E)a mess.

Question 6

Assuming that the density of water is 1.00 g/mL, how many moles of water are there in a liter of water?

A)1.00 moles
B)0.0180 moles
C)55.6 moles
D)18.0 moles
E)1.00 * 10² moles

Question 7

A homogeneous mixture containing sodium, potassium, calcium, and chloride ions dissolved in water is

A)an electrically charged solution.
B)an acidic solution.
C)a flammable solution.
D)a poisonous solution.
E)an aqueous solution.

Question 8

How many grams of solid potassium chlorate (KClO₃, 122.55 g/mol) are needed to make 150 mL of 0.50 M solution?

A)0.11 g
B)37 g
C)9.2 g
D)0.41 g
E)2.7*10^-2g

Question 9

If 120 g of NaOH 40.00 g/mol) were used to prepare 500.0 mL of solution, what would the concentration be?

A)1.0 M
B)2.0 M
C)3.0 M
D)4.0 M
E)6.0 M

Question 10

Molarity, M, is defined as

A)moles of solute dissolved in 1 mol of solvent.
B)moles of solute dissolved in 1 kg of solvent.
C)moles of solute dissolved in 1 L of solvent.
D)moles of solute dissolved in 1 L of solution.
E)moles of solute dissolved in the solution.

Question 11

Lead levels in drinking water should be no higher than 15 ppb.What is this in mol/L? Assume the density of drinking water is 1.0 g/mL.

A)7.2 *10^-8 M
B)7.2 *10^-5 M
C)3.1 * 10^-7 M
D)3.1 * 10^-8 M
E)2.0 *10^-8 M

Question 12

Concentrated sulfuric acid contains 4 g of water for every 100 g of solution.The solvent is

A)water.
B)sulfuric acid.
C)concentrated.
D)the same as the solution.
E)the same as the solute in this case.

Question 13

A salt solution is added to a marine aquarium.What mass of sodium chloride NaCl, 58.44 g/mol) is needed to produce 250.0 mL of a solution that has a concentration of 50.0 mM ?

A)731 g
B)731 mg
C)58.5 g
D)2.92 mg
E)2.92 g

Question 14

Calculate parts per million Br^- in a sample of seawater that is 0.865 mM Br^- with a density of 1.025 g/mL.

A)69.1 ppm
B)79.9 ppm
C)94.7 ppm
D)70.8 ppm
E)67.4 ppm

Question 15

Determine the molar concentration of the lead(II) ion in a 26.0 ppb aqueous solution of lead(II) nitrate [Pb(NO₃)₂, 331.22 g/mol].Assume that the density of the solution is 0.998 g/mL.

A)7.85 *10^-8 M
B)2.60 *10^-8 M
C)7.85 *10^-11 M
D)7.83 *10^-8 M
E)3.92 *10^-8 M

Question 16

The proof of liquor is defined as two times the percent ethanol CH₃CH₂OH) it contains by volume.If vodka is 80 proof, what is the solvent in vodka?

A)water
B)vodka
C)ethanol
D)not enough information to answer
E)the same as the solute in this case

Question 17

Which of the following represents the maximum mercury levels in drinking water, which is approximately 2 ppb? Assume the density of drinking water is 1 g/mL.

A)1 nM
B)10 nM
C)20 nM
D)1 $\mu$ M
E)10 $\mu$ M

Question 18

Determine the molar concentration of ethanol CH₃CH₂OH, 46.08 g/mol) in a wine that is 14% ethanol by mass.The density of this wine is 0.93 g/cm3.

A)0.063 M
B)13.0 M
C)0.14 M
D)2.8 M
E)3.0 M

Question 19

A concentrated aqueous hydrofluoric acid solution has a density of 1.15 g/mL and is 48.0% by mass HF 20.01 g/mol).Determine the molar concentration of this solution.

A)27.6 M
B)33.2 M
C)41.7 M
D)24.0 M
E)20.9 M

Question 20

How many grams of sodium chloride NaCl, 58.44 g/mol) are needed to make up 250.mL of a solution that is 2.00 M ?

A)4.28 g
B)7.30 g
C)14.6 g
D)29.2 g
E)117 g

Question 21

How many moles of ions are present in exactly 150 mL of a 0.260 M ammonium phosphate solution, NH₄)₃PO₄aq)?

A)1.04 mol
B)0.156 mol
C)0.0390 mol
D)0.117 mol
E)0.312 mol

Question 22

How many moles of nitrate ions are present in exactly 275 mL of a 1.25 M copperII) nitrate solution, CuNO₃)₂aq)?

A)0.220 mol
B)0.440 mol
C)0.172 mol
D)0.344 mol
E)0.688 mol

Question 23

In demonstrations of strong and weak electrolytes and nonelectrolytes, a lightbulb apparatus that shows how much a solution conducts electricity by the brightness of the light is often used.When pure water is tested, the bulb does not light.Which of the following aqueous solutions causes the bulb to burn dimly but not brightly?

A)table salt, NaCl
B)isopropyl alcohol, C₃H₇OH
C)fructose, C₆H₁₂O₆
D)methanol, CH₃OH
E)acetic acid, CH₃COOH

Question 24

Which of the following would behave as a strong electrolyte in water?

A)ethanol, C₂H₅OH
B)formaldehyde, CH₂O
C)table sugar, C₁₂H₂₂O₁₁
D)acetic acid, CH₃COOH
E)table salt, NaCl

Question 25

In the dilution of 10.0 mL of a 0.10 M solution of HCl to a volume of 20.0 mL, what remains unchanged?

A)the moles of HCl in the solution
B)the concentration of the HCl solution
C)the volume of the HCl solution
D)the mass of the HCl solution
E)All of the above change.

Question 26

In demonstrations of strong and weak electrolytes and nonelectrolytes, a lightbulb apparatus that shows how much a solution conducts electricity by the brightness of the light is often used.When pure water is tested, the bulb does not light.Which of the following aqueous solutions causes the bulb to burn the brightest?

A)formic acid, HCOOH
B)ammonia, NH₃
C)table sugar, C₁₂H₂₂O₁₁
D)a calcium salt, CaCl₂
E)methanol, CH₃OH

Question 27

If 75.0 mL of a 0.20 M solution of sodium nitrate NaNO₃) is mixed with 25.0 mL of 0.10 M barium nitrate BaNO₃)₂), what is the molar concentration of nitrate in the resulting solution?

A)0.10 M
B)0.20 M
C)0.30 M
D)0.15 M
E)0.18 M

Question 28

Diluting 1.0 mL of a 1.0 M solution to 1000 mL results in a solution that is 0.001 M.Repeating this 1000-fold dilution process five more times results in a concentration of

A)1.0 *10^-8 M .
B)5.0 *10^-3 M.
C)1.0 *10^-18 M.
D)1.0 *10^-9 M.
E)2.0 *10^-4 M.

Question 29

Which of the following statements is true regarding electrolytes and nonelectrolytes?

A)Molten ionic compounds are usually considered to be weak electrolytes.
B)Because graphite is a good conductor of electricity, it is considered to be a strong electrolyte.
C)All molecular compounds dissolved in water behave as nonelectrolytes.
D)Ionic compounds that dissolve in water contain mobile ions and are strong electrolytes.
E)All acids ionize completely when they dissolve in water.

Question 30

Which of the following would be the best conductor of electricity when dissolved in water?

A)iodine, I₂aq)
B)ethylene glycol, HOCH₂CH₂OHaq)
C)methanol, CH₃OH
D)sodium hydroxide, NaOHaq)
E)carbon dioxide, CO₂aq)

Question 31

What is the molar concentration of sodium ion in a 200.0 mL solution prepared from 1.223 g of sodium phosphate Na₃PO₄, 163.9.4 g/mol), which is a cleaning agent, food additive, and stain remover?

A)0.1119 M
B)0.03731 M
C)0.7338 M
D)0.2486 M
E)0.1243 M

Question 32

If 0.10 L of 3.0 M sucrose solution were diluted to 250 mL, what would the concentration be?

A)0.012 M
B)0.12 M
C)1.2 M
D)12 M
E)120 M

Question 33

A chemistry student attempted to make a 0.2000 M solution of NaCl using a 100.0 mL volumetric flask.The Student added exactly 100.0 mL of water to the flask, then added 0.02000 mol of NaCl, and found that the total volume in the flask was above the 100.0 mL mark.What was the concentration of the solution?

A)exactly 0.2000 M
B)a bit less than 0.2000 M
C)a bit more than 0.2000 M
D)exactly 0.2002 M
E)There is insufficient information to select one of the above responses.

Question 34

Commercial hydrochloric acid is 12.1 M.What volume of commercial HCl solution should be used to prepare 250.0 mL of 3.00 M HCl?

A)139 mL
B)126 mL
C)252 mL
D)62.0 mL
E)83.0 mL

Question 35

Lactated Ringer's solution can be prepared by dissolving 0.6000 g sodium chloride NaCl, 58.44 g/mol), 0.310 g sodium lactate NaC₃H₅O₃ 112.06 g/mol), 30.00 mg potassium chloride KCl, 74.55 g/mol), and 20.00 mg calcium chloride dihydrate CaCl₂.2H₂O, 147.0 g/mol) in water to give a final volume of 100.0 mL.What is the molar concentration of chloride?

A)0.1081 M
B)0.1094 M
C)0.1321 M
D)0.1456 M
E)0.6850 M

Question 36

Which contains more solute particles: a 0.10 M aqueous solution of methanol CH₃OH) or a 0.10 M aqueous solution of salt NaCl)?

A)They contain the same number of solute particles.
B)The salt solution contains twice as many particles as the methanol solution.
C)The methanol solution contains three times as many particles as the salt solution.
D)The salt solution contains three times as many particles as the methanol solution.
E)The methanol solution contains twice as many particles as the salt solution.

Question 37

Which of the following should have the highest conductivity?

A)3.0 M NaCl
B)2.1 M Na₃PO₄
C)2.4 M CaCl₂
D)2.6 M PbCH₃COO)₂
E)3.2 M NH₄NO₃

Question 38

What volume of 12.0 M HCl solution needs to be diluted to produce 500.0 mL of 3.00 M HCl solution?

A)0.125 L
B)0.250 L
C)0.500 L
D)2.00 L
E)1.00 L

Question 39

Which of the following would behave as a weak electrolyte in water?

A)barium hydroxide, BaOH)₂
B)ammonium chloride, NH₄Cl
C)ammonia, NH₃
D)sodium nitrate, NaNO₃
E)copperII) sulfate, CuSO₄

Question 40

If the molar concentration of sodium phosphate Na₃PO₄) is 0.30 M, what is the concentration of sodium ions?

A)0.10 M
B)0.45 M
C)0.60 M
D)0.30 M
E)0.90 M

Question 41

What are the products in the molecular equation for the complete neutralization reaction of aqueous barium hydroxide and nitric acid?

A)BaNO₃ aq) + H₂ O™)
B)BaH₂ aq) + 2 NOg)
C)Ba 2Os) + H₂O™) + 2 NO₂ g)
D)BaN₂ s) + 2H₂ O™)
E)BaNO₃ )2 aq) + 2 H₂ O™)

Question 42

Which of the following statements regarding a weak acid is NOT correct?

A)A weak acid has a very low concentration.
B)A weak acid ionizes in water to produce hydronium ions.
C)A weak acid ionizes only to a small extent in water.
D)A weak acid neutralizes bases.
E)Acetic acid is an example.

Question 43

Which of the following best represents the molecular equation for the complete neutralization reaction of sulfuric acid with aqueous potassium hydroxide?

A)H₂ SO₄ (aq) + KOH(aq) $\rightarrow$ HSO₄^-(aq) + KHSO₄ (aq)
B)H₂ SO₄ (aq) + 2 KOH(aq) $\rightarrow$ 2 H₂O(l) + 2 KSO₄ aq)
C)H₂ SO₄ (aq) + KOH(aq) $\rightarrow$ KH(aq) + 2 H₂O(l) + SO₂ (g)
D)H₂SO₄ (aq) + KOH(aq) $\rightarrow$ H₂O(l) + KHSO₄ (aq)
E)H₂SO₄ (aq) + 2 KOH(aq) $\rightarrow$ 2 H₂O(l) + K₂SO₄ (aq)

Question 44

Which of the following is a weak acid?

A)hydrobromic, HBr
B)hydroiodic, HI
C)hydrofluoric, HF
D)hydrochloric, HCl
E)perchloric, HClO₄

Question 45

Identify the acid in the following acid-base reaction:
3 NaHSO₄ (aq) + Fe(OH)₃ (s) $\rightarrow$ Fe ³⁺(aq) +3 SO₄^2-(aq) + 3 Na⁺(aq) +3 H₂O(l)

A)HSO₄-
B)Na⁺
C)Fe³⁺
D)OH^-
E)SO₄^{2 -}

Question 46

Which is the total ionic equation for the reaction of hydrochloric acid with solid chromiumIII) hydroxide? None of the products are solids.

A)3H⁺(aq) +3 Cl^-(aq) + Cr³⁺(aq) + 3 OH^-(aq) $\rightarrow$ Cr³⁺(aq) + 3 Cl ^- (aq) +3H₂O(l)
B)3H⁺(aq) +3 Cl ^- (aq) + Cr(OH)₃ (s) $\rightarrow$ Cr³⁺(aq) + 3 Cl ^-(aq) +3H₂O(l)
C)6H⁺(aq) +6 Cl(aq) + Cr₂O₃ (s) $\rightarrow$ 2 Cr³⁺(aq) + 6 Cl^- (aq) +3H₂O(l)
D)3 HCl (aq)+ Cr OH₃ (s) $\rightarrow$ Cr³⁺(aq) + 3Cl 1^- (aq) +3H₂O(l)
E)H⁺(aq) + Cl ^- (aq) + CrOH₃ (s) $\rightarrow$ Cr³⁺(aq) + Cl ^- (aq) +2H₂O(l)

Question 47

Which of the following is a weak base?

A)CH₃OH
B)HCOOH
C)LiOH
D)CH₃NH₂
E)CaOH)₂

Question 48

In its reaction with water, phenol (C₆H₅OH) acts as a weak acid.Which of the following statements is FALSE?

A)Hydronium ions are produced.
B)Ionization is not complete.
C)It generates hydroxide ions.
D)The pH of the solution at 25 $\degree$ C is less than 7.
E)The ionization reaction reaches equilibrium.

Question 49

In its reaction with water, ammonia NH₃)

A)acts as an acid.
B)acts as a base.
C)acts neither as an acid nor as a base.
D)serves as both an acid and as a base.
E)causes a precipitate to form.

Question 50

In demonstrations of strong and weak electrolytes and nonelectrolytes, a lightbulb apparatus that shows how much a solution conducts electricity by the brightness of the light is often used.When pure water is tested, the bulb does not light.When some acetic acid is added to the water, the bulb burns dimly.When more acetic acid is added to the solution, the bulb burns a little more brightly.If pure acetic acid is used, what would be observed?

A)The bulb would not light.
B)The bulb would burn dimly.
C)The bulb would burn more than any of the others but still not brightly.
D)The bulb would burn brightly.
E)The bulb would burn out.

Question 51

Which of the following is a strong acid?

A)carbonic, H₂CO₃
B)phosphoric, H₃PO₄
C)hydrocyanic, HCN
D)hydrosulfuric, H₂S
E)sulfuric, H₂SO₄

Question 52

Which of the following statements regarding a strong monoprotic acid is NOT correct?

A)The acid ionizes completely in water.
B)The acid ionizes in water to produce hydronium ions.
C)The acid neutralizes bases.
D)HCl is an example.
E)The acid is highly concentrated.

Question 53

Which statement below about a sulfuric acid solution is FALSE?

A)H₂SO₄ completely ionizes to form HSO₄^- and H₃O⁺.
B)At equilibrium, the only species present are H₂O, H₃O⁺, and SO₄^{2 -}.
C)There are HSO₄^-ions present at equilibrium.
D)HSO₄^2- is a weaker acid than H₂SO₄.
E)H₂SO₄ is a diprotic acid.

Question 54

Calcium hydroxide is slightly soluble in water.About 1 gram will dissolve in 1 liter.What are the spectator ions in the reaction of such a dilute solution of calcium hydroxide with hydrochloric acid?

A)Ca²⁺and Cl ^-
B)Ca²⁺and OH ^-
C)H₃O⁺and OH 1^-
D)H₃O⁺and Cl ^-
E)Ca²⁺, Cl ^- ,H₃O⁺, and OH ^-

Question 55

Hydroxyapatite [Ca₅PO₄)₃OH)], the major component of tooth enamel, is attacked and decomposed by acids more readily than fluorapatite [Ca₅PO₄)₃F].Which of the following reactions is analogous to the reaction of hydroxyapatite with acid?

A)Ca(s) + 2 HCl (aq) $\rightarrow$ CaCL₂ (s) +2 H⁺
B)CaF₂ (s) + 2H⁺(aq) $\rightarrow$ Ca ²⁺(aq) + 2 HF(aq)
C)Ca(OH)₂ (s) + 2H⁺(aq) $\rightarrow$ Ca²⁺(aq) +2H₂O(l)
D)Ca(s) + 2H⁺(aq) $\rightarrow$ Ca ²⁺(aq) +H₂ (g)
E)Ca₃(PO₄)₂ (s) +6 H⁺(aq) $\rightarrow$ 3 Ca ²⁺(aq) + 2H₃PO₄ (aq)

Question 56

Which of the following is a strong base?

A)HNO₃
B)AIOH)₃
C)NH₃
D)FeOH)₃
E)RbOH

Question 57

What are the products in the complete ionic equation for the following reaction?
HBr(aq) + KOH(aq) $\rightarrow$ products

A)H₂ O(l) and KBrs)
B)K⁺(aq), Br^-(aq), and H₂ O(l)
C)H₂ O(l), K⁺(aq), and Br₂ (aq)
D)KH(aq), H₂ O(l), and BrOH(aq)
E)KH(aq) and BrOH(aq)

Question 58

The layers in a particular gumball are 1) an outer layer of citric acid and malonic acid; 2) a layer of sugar and flavoring; 3) a layer of sodium bicarbonate NaHCO₃); and 4) gum.When a person starts to eat one of these gumballs, s/he puckers, smiles, and then foams at the mouth before starting to chew the gum itself.Where did the foam come from?

A)The sodium bicarbonate reacts with sugar, making carbon dioxide gas.
B)The sodium bicarbonate explodes when exposed to moisture.
C)The acids react with the sodium bicarbonate, making unstable carbonic acid.
D)The flavoring contains a foaming agent.
E)The acids react with the sugar, making a carbon volcano.

Question 59

Select the net ionic equation for the reaction of sodium carbonate with hydrobromic acid.

A)Na₂CO₃ (aq) $\rightarrow$ 2Na ⁺(aq) + CO₃^{2 -} (aq)
B)HBrO₃ (aq) $\rightarrow$ H⁺(aq) + BrO₃^- (aq)
C)Na⁺(aq) + Br ^- (aq) $\rightarrow$ NaBr (aq)
D)2 Na⁺(aq) + CO₃^{2 -} (aq) +2H ^- (aq) +2Br^- (aq) $\rightarrow$ H₂O(l)+ 2Na(s) +CO₂ (g) + Br₂ (l)
E)2H⁺(aq) + CO₃^{2 -} (aq) $\rightarrow$ H₂O(l) + CO₂ (g)

Question 60

Select the net ionic equation for the reaction of rubidium hydroxide with nitric acid.

A)Rb OH(aq) $\rightarrow$ Rb⁺(aq) + OH^-(aq)
B)HNO₃ (aq) $\rightarrow$ H⁺(aq) + NO₃(aq)
C)Rb⁺(aq) + NO₃^-(aq) $\rightarrow$ RbNO₃ (aq)
D)H⁺(aq) + OH1^-aq) $\rightarrow$ H₂ O(l)
E)Rb⁺(aq) + OH^-(aq) +H⁺(aq) + NO₃ ^-(aq) $\rightarrow$ H₂O(l) + RbNO₃ (aq)

Question 61

What is the formula of the precipitate that forms when aqueous NaCl and aqueous Hg₂NO₃)₂ are mixed?

A)HgCl₂
B)Hg₂Cl₂
C)HgCl
D)Hg₂Cl
E)NaNO₃

Question 62

Oxalic acid H₂C₂O₄), a diprotic acid that is used in many cleaning and bleaching applications, can be toxic in high amounts when ingested.In 100 grams of parsley, there are about 0.02 moles of oxalic acid.Which of the following would completely neutralize this quantity of oxalic acid?

A)1 L of 0.02 M NaOH
B)0.4 L of 0.1 M KOH
C)0.5 L of 0.02 M BaOH)₂
D)0.25 L of 0.08 M KOH
E)0.1 L of 0.04 M CaOH)₂

Question 63

If 12.8 g lead(II) sulfate 303.26 g/mol) precipitates when excess potassium chloride is added to 1.65 L of a water sample, what is the molar concentration of Pb^₂+ in the sample?

A)0.0696 M
B)0.0422 M
C)0.0256 M
D)0.129 M
E)0.776 M

Question 64

Which of the following ionic compounds is insoluble in water?

A)Cu₃PO₄)₂
B)FeCl₃
C)NH₄CH₃COO
D)AgNO₃
E)KSCN

Question 65

Approximately 192 grams of ammonium nitrate (80.04 g/mol) will dissolve in 100 grams of water at 20 $\degree$ C.If 21.0 mol NH₄NO₃ is dissolved in 875 g H₂O, the solution is

A)unsaturated.
B)supersaturated.
C)saturated.
D)dilute.
E)reactive.

Question 66

How many grams of nickelII) phosphate (366.02 g/mol) will precipitate if excess sodium phosphate is added to 1.20 L of 0.684 M nicke(lII) acetate?

A)1.00 *10²g
B)2.00 * 10²g
C)3.00 * 10²g
D)6.00 *10²g
E)1.67* 10²g

Question 67

Which of the following compounds is most soluble in water?

A)PbF₂
B)FeOH)₃
C)Cr₂S₃
D)CuNO₃)₂
E)PbCrO₄

Question 68

Most chloride salts are soluble.Which of the following is an exception to this generalization?

A)NH₄Cl
B)AlCl₃
C)ZnCl₂
D)CuCl₂
E)PbCl₂

Question 69

What is the formula of the precipitate that forms when aqueous ammonium phosphate and aqueous copperII) chloride are mixed?

A)Cu₃P₂
B)CuNH₄)₂
C)Cu₂PO₃
D)Cu₂ClO₃
E)Cu₃PO₄)₂

Question 70

Write the net ionic equation for the reaction that takes place between aqueous copperII) nitrate and aqueous potassium phosphate.

A)Cu(NO₃ )₂(aq) +K₃PO₄(aq) $\rightarrow$ CuPO₄(s) +K₃(NO₃)₂(aq)
B)3 Cu(NO₃)₂(aq) + 2 K₃PO₄(aq) $\rightarrow$ Cu₃(PO₄)₂(s) + 6 KNO₃(aq)
C)Cu²⁺(aq)+PO₄^3-(aq) $\rightarrow$ CuPO₄ (s)
D)3 Cu²⁺(aq) + 2 PO₄^{3 -} (aq) $\rightarrow$ Cu₃(PO₄)₂(s)
E)3 Cu²⁺(aq) + 2 PO₄³ 1^- (aq) $\rightarrow$ 3 CuO(s) +P₂O₅ (s)

Question 71

What is the formula of the precipitate that forms when aqueous potassium sulfide and aqueous silver nitrate are mixed?

A)Ag₃N
B)KNO₃
C)K₂SO₄
D)Ag₂S
E)Ag₂SO₄

Question 72

How many grams of ironIII) hydroxide 106.87 g/mol) will precipitate if excess ironIII) nitrate is added to 0.850 L of 1.26 M sodium hydroxide?

A)114 g
B)38.2 g
C)90.9 g
D)135 g
E)343 g

Question 73

Write the net ionic equation for the reaction that takes place between aqueous magnesium chloride and aqueous sodium hydroxide.

A)MgCL₂(aq)+ NaOH(aq) $\rightarrow$ MgOH(s) +NaCL₂(aq)
B)MgCL₂(aq) + 2 NaOH(aq) $\rightarrow$ Mg(OH)₂(s)+ 2 NaCl(aq)
C)Mg²⁺(aq)+ 2 OH ^- (aq) $\rightarrow$ Mg(OH)₂ (s)
D)Mg²⁺(aq) + 2 Cl ^- (aq) + 2 Na ⁺ (aq) + 2 OH ^- (aq) $\rightarrow$ Mg(OH)₂(s) + 2 NaCl(s)
E)Mg²⁺(aq) +OH ^- (aq) $\rightarrow$ MgOH(s)

Question 74

Hard water, which contains Mg²⁺ and Ca ²⁺ ions, tends to form a ring in a bathtub due to its reaction with the soluble anions in soap.The formation of this insoluble material is an example of

A)an acid-base reaction.
B)a precipitation reaction.
C)a redox reaction.
D)a combustion reaction.
E)a decomposition reaction.

Question 75

What is the formula of the precipitate that forms when aqueous FeNO₃)₃ and aqueous Na₂CO₃ are mixed?

A)Na₂NO₃)₃
B)FeCO₃
C)Fe₂CO₃)₃
D)Na₂Fe
E)CO₃NO₃

Question 76

Chalk contains calcium carbonate.What would be the best solution for cleaning the chalk off a sidewalk?

A)ammonia
B)plain water
C)olive oil
D)paint thinner
E)vinegar

Question 77

Limescale that builds up in showers, kettles, and pipes is often primarily composed of calcium carbonate.One limescale remover contains sulfamic acid (H₃NSO₃), which can be considered to be a strong monoprotic acid.Which reaction summarizes the action of sulfamic acid on limescale?

A)H ⁺ (aq)+ H₂NSO₃ ^- (aq) + CaCO₃ (s) $\rightarrow$ HCO₃ ^- (aq) + HNSO3^{2 -} (aq) + Ca ⁺ (aq)
B)3H ⁺ (aq) + NSO₃ ^- (aq) + CaCO₃ (s) $\rightarrow$ Ca ^{2 +} (aq) + HSO₃ ^- (aq) + NO₂ (g) + CO₂ (g) +H₂O (l)
C)2H ⁺ aq) +2 H₂NSO₃ ^- (aq) + CaCO₃ (s) $\rightarrow$ CO₂ (g) +2 H₂NSO₃ ^- (aq) + Ca ^{2 +} (aq) +H₂O (l)
D)3H ⁺ (aq) + NSO₃^{3 -} (aq) + CaCO₃ (s) $\rightarrow$ Ca ^{2 +} (aq) + NSO₃^{3 -} (aq) + CO₂ (g) + 3 HNO₂ (aq)
E)3H⁺(aq) + NSO₃ ^- (aq) + CaCO₃ (s) $\rightarrow$ CaS(s) + HCN(g) +3H₂O(l)

Question 78

What mass of silver chloride will be recovered if excess sodium chloride is added to 0.500 L of solution containing 10.79 g of Ag⁺?

A)10.8 g
B)21.6 g
C)28.6 g
D)7.21 g
E)14.3 g

Question 79

Which best describes the reaction that takes place between aqueous leadII) acetate and aqueous ammonium chloride?

A)Pb(CH₃COO)₂(aq) + NH₄Cl(aq) $\rightarrow$ PbCl(s) +NH₄(CH₃COO)₂(aq)
B)Pb(CH₃COO)₂(aq) + 2 NH₄Cl(aq) $\rightarrow$ PbCL₂(s) + 2 NH₄CH₃COO(aq)
C)PbCH₃COO(aq) + NH₄Cl(aq) $\rightarrow$ PbCl(s) +NH₄CH₃COO(aq)
D)Pb₂CH₃COO(aq) + 2 NH₄Cl(aq) $\rightarrow$ 2 PbCl(s) + 2 NH₄CH₃COO(aq)
E)Pb(CH₃COO)₂(aq) + 2 NH₄Cl(aq) $\rightarrow$ PbCL₂(s) +(NH₄)₂(CH₃COO)₂(aq)

Question 80

Which best describes the reaction that takes place between aqueous barium nitrate and aqueous sodium sulfate?

A)Ba(NO₃)₂(aq) + Na₂SO₄(aq) $\rightarrow$ BaSO₄(s) + 2 NaNO₃(aq)
B)BaNO₃(aq) +NaSO₄(aq) $\rightarrow$ BaSO₄(s) + NaNO₃(aq)
C)2 Ba(NO₃)(aq) +Na₂SO₄(aq) $\rightarrow$ Ba₂SO₄(s) + 2 NaNO₃(aq)
D)Ba(NO₃)₂(aq) + 2 NaSO₄(aq) $\rightarrow$ Ba(SO₄)₂(s) + 2 NaNO₃(aq)
E)Ba(NO₃)₂(aq) +Na₂SO₄(aq) $\rightarrow$ BaSO₄(aq) + 2 NaNO₃(s)