Deck 4: Solution Chemistry: The Hydrosphere

Question 1

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.

Answer 1

sulfuric acid.

Question 2

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.

Answer 2

moles of solute dissolved in 1 L of solution.

Question 3

How many grams of solid magnesium chloride, MgCl₂, are needed to make 250 mL of 0.50 M solution?

A) 9.5 g
B) 48 g
C) 12 g
D) 125 g
E) 4.8 g

Answer 3

12 g

Question 4

Lead is the least toxic to fish compared to zinc, copper, and mercury ions. Fish can tolerate a lead concentration slightly above 0.850 mM. What is this concentration in ppm? Assume the density of the water is 1.00 g/mL.

A) 176 ppm
B) 83 ppm
C) 352 ppm
D) 0.176 ppm
E) 0.352 ppm

Question 5

If 120 g of NaOH were used to prepare 500 mL of solution, what would the concentration be?

A) 1 M
B) 2 M
C) 3 M
D) 4 M
E) 6 M

Question 6

A medical saline solution is prepared by mixing 925 mg sodium chloride (58.44 g/mol) with water to make 100.0 mL solution. What is the molar concentration of this solution?

A) 925 M
B) 9250 M
C) 15.8 M
D) 0.158 M
E) Can't tell, need the volume of water used.

Question 7

Sodium fluoride (NaF) is added to drinking water in some municipalities to protect teeth against cavities. The idea is to convert hydroxyapatite, Ca₁₀(PO₄)₆(OH)₂, into more stable fluorapatite, Ca₁₀(PO₄)₆F₂. The molar mass of hydroxyapatite is 502 g/mol. What is the molarity of a 10.0 mg/L sodium fluoride solution?

A) 2.38 *10^-4 M
B) 1.99 *10^-5 M
C) 2.63*10^-4 M
D) 1.19 *10^-4 M
E) 0.263 M

Question 8

What are the units of molar concentration, M ?

A) mol/L
B) g/L
C) mol/kg
D) ppm
E) mol/mL

Question 9

The amount of blood in the human body is around 5.0 L, and this amount of blood contains about 0.88 g of potassium ions. What is the concentration of potassium ions in blood?

A) 0.88 mM
B) 0.18 mM
C) 23 mM
D) 4.5 mM
E) 2.3 mM

Question 10

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 11

If there are 0.505 g of NaCl 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

Question 12

Determine the molar concentration of an aqueous solution of lead(II) nitrate solution that is 26 ppb (parts per billion) Pb(NO₃)₂. Since the solution is very dilute, assume the density is that of water, 1.00 g/mL.

A) 7.85 *10^-14 M
B) 2.60 *10^-8 M
C) 4.26 *10^-11 M
D) 7.85 *10^-8 M
E) 7.85 *10^-11M

Question 13

A chemistry student attempted to make a 0.2000 M solution of NaCl using a 100.0 mL volumetric flask. She 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 14

The proof of liquor is defined as the percentage of ethanol it contains times two. If vodka is 80 proof, what is the solvent in vodka?

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

Question 15

Determine the molar concentration of ethanol (C₂H₆O) 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 16

Human blood contains about 0.18 g potassium ions per liter and has a density of 1.06 g/mL. What is the concentration of potassium ions in blood expressed in parts per million?

A) 18 ppm
B) 180 ppm
C) 170 ppm
D) 88 ppm
E) 880 ppm

Question 17

Which one of the following mixtures is not a solution?

A) white vinegar
B) bottled spring water
C) filtered dry air
D) clear tea
E) pulpy orange juice

Question 18

A concentrated aqueous ammonia solution has a density of 0.90 g/mL and is 28.0% by mass ammonia. Determine the molar concentration of this solution.

A) 15 M
B) 1.5 M
C) 0.032 M
D) 31 M
E) 3.0 M

Question 19

Lead is the least toxic to fish compared to zinc, copper, and mercury ions. Fish can tolerate a concentration slightly above 0.85 mM. What is the lead concentration in mg/L?

A) 180 mg/L
B) 95 mg/L
C) 360 mg/L
D) 190 mg/L
E) 48 mg/L

Question 20

The National Primary Drinking Water Regulations limit the concentration of lead in drinking water to 0.015 mg/L, which is __________.

A) 0.015 ppb
B) 15 ppm
C) 1.5 ppb
D) 15 ppb
E) 150 ppb

Question 21

The World Health Organization recommends that the maximum allowable concentration of chromium(VI) in drinking water be limited to 0.05 mg/L. If the molar absorptivity of chromium(VI) at 345 nm is 1.5*10³/(M cm), what is the absorbance of a solution that contains 0.050 mg/L in a 10-cm-long cell?

A) 0.0014
B) 0.75
C) 0.014
D) 0.075
E) 14

Question 22

In a demonstration of strong electrolytes, weak electrolytes, and nonelectrolytes, Professor Popsnorkle used a lightbulb apparatus that showed how much a solution conducted electricity by the brightness of the lightbulb. When pure water was tested, the bulb did not light. Then Professor Popsnorkle tested the following aqueous solutions. Which one caused the bulb to burn dimly but not brightly?

A) table salt, NaCl
B) ethanol, CH₃CH₂OH
C) table sugar, C₁₂H₂₂O₁₁
D) acetic acid, CH₃COOH
E) methanol, CH₃OH

Question 23

Diluting 1.0 mL of a 1.0 M solution to 1,000 mL results in a solution that is 0.001 M. Repeating this 1,000-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 24

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) Neither solution contains solute particles.
E) The methanol solution contains twice as many particles as the salt solution.

Question 25

What volume of 12 M HCl solution needs to be diluted to produce 500 mL of 3.0 M HCl solution?

A) 125 mL
B) 250 mL
C) 500 mL
D) 2,000 mL
E) 1,000 mL

Question 26

What volume of 0.25 M hydrochloric acid (HCl) solution contains Avogadro's number of Cl ^- ions?

A) 1.0 L
B) 4 mL
C) 400 mL
D) 4,000 mL
E) 40,000 mL

Question 27

How many grams of sodium chloride, NaCl, are needed to make up 1.00 L of a solution that is 2.00 M?

A) 23.0 g
B) 29.2 g
C) 58.4 g
D) 117 g
E) 35.5 g

Question 28

If 50.0 mL of a 0.10 M solution of sodium chloride is mixed with 50.0 mL of 0.10 M magnesium chloride, what is the molar concentration of chloride in the resulting solution?

A) 0.10 M
B) 0.20 M
C) 0.05 M
D) 0.15 M
E) 0.25 M

Question 29

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 30

In a demonstration of strong electrolytes, weak electrolytes, and nonelectrolytes, Professor Popsnorkle used a lightbulb apparatus that showed how much a solution conducted electricity by the brightness of the lightbulb. When pure water was tested, the bulb did not light. Then Professor Popsnorkle tested the following aqueous solutions. Which one caused the bulb to burn the brightest?

A) table salt, NaCl
B) ethanol, CH₃CH₂OH
C) table sugar, C₁₂H₂₂O₁₁
D) acetic acid, CH₃COOH
E) methanol, CH₃OH

Question 31

If the molar concentration of sodium sulfate (Na₂SO₄) is 0.10 M, what is the concentration of sodium ion?

A) 0.10 M
B) 0.050 M
C) 0.20 M
D) 0.30 M
E) 0.40 M

Question 32

What volume of 3.0 M NaOH contains 0.15 mole of NaOH?

A) 500 mL
B) 50 mL
C) 5.0 mL
D) 0.50 mL
E) 0.050 mL

Question 33

If 100 mL of 3.0 M 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 34

A salt solution is added to a marine aquarium. What mass of sodium chloride (58.44 g/mol) is needed to produce 250.0 mL of a solution that has a concentration of 0.0500 M ?

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

Question 35

A standard adult dose of a cough suppressant is 15.0 mL. This portion contains 5.00 mg of the active ingredient. A pediatrician suggests that this medication can be given to children over the age of 6 years, but only if it is diluted so the dose is 1.00 mg in 20.0 mL. How many milliliters of the adult medicine would you need to use to make 100.0 mL of the child-strength cough suppressant?

A) 1.00 mL
B) 5.00 mL
C) 10.0 mL
D) 15.0 mL
E) 20.0 mL

Question 36

What is the molar concentration of sodium ions in a 0.3 M sodium phosphate (Na₃PO₄, 164 g/mol) solution? Sodium phosphate is used as a cleaning agent, food additive, and stain remover.

A) 0.1 M
B) 0.3 M
C) 0.6 M
D) 0.9 M
E) 1.0 M

Question 37

In a demonstration of strong electrolytes, weak electrolytes, and nonelectrolytes, Professor Popsnorkle used a lightbulb apparatus that showed how much a solution conducted electricity by the brightness of the lightbulb. When pure water was tested, the bulb did not light. When some acetic acid was added to the water, the bulb burned dimly. When more acetic acid was added to the solution, the bulb burned a little more brightly. In his frustration to make the bulb shine brightly with acetic acid, Professor Popsnorkle started over by testing the beaker of the pure acetic acid. What was the result?

A) The bulb did not light.
B) The bulb burned dimly.
C) The bulb burned more than any of the others but still not brightly.
D) The bulb burned brightly.
E) Professor Popsnorkle was electrocuted.

Question 38

Which picture best represents an atomic-level view of a nonelectrolyte solution (water molecules not shown)?

A)
B)
C)
D)

Question 39

What volume of 0.25 M hydrochloric acid (HCl) solution contains 0.15 mol HCl?

A) 6.0 mL
B) 60 mL
C) 600 mL
D) 1.7 L
E) 170 mL

Question 40

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 41

Two phosphoric acid molecules can combine to make pyrophosphoric acid and another molecule as shown here. The pyrophosphoric acid molecule is a phosphoester and is a structural element in the ADP/ATP metabolic energy system. What molecule is represented by the question mark in the structural reaction equation below?

A) O₂
B) OH^-
C) H₂O
D) PO
E) H₂

Question 42

Hydroxyapatite, [Ca₅(PO₄)₃(OH)], the major component of tooth enamel, is attacked and decomposed by acids more readily than fluorapatite, [Ca₅(PO₄)₃F]. Which one of the following reactions is analogous to the reaction of hydroxyapatite?

A) Ca(s) + 2HCl(aq) $\rightarrow$ CaCl₂(s) + 2H⁺
B) CaF₂(s) + 2H⁺(aq) $\rightarrow$ Ca²⁺(aq) + 2HF(aq)
C) Ca(OH)₂(s) + 2H⁺(aq) $\rightarrow$ Ca²⁺(aq) + 2H₂O(l)
D) Ca(s) + 2H⁺(aq) $\rightarrow$ Ca²⁺(aq) + H₂(g)
E) Ca₃(PO₄)₂(s) + 6H⁺(aq) $\rightarrow$ 3Ca²⁺(aq) + 2H₃PO₄(aq)

Question 43

If one regular antacid tablet contains 500 mg of solid CaCO₃ (100 g/mol), how many mL of 1.0 M stomach acid (HCl) could it neutralize?

A) 5 mL
B) 10 mL
C) 50 mL
D) 100 mL
E) 15 mL

Question 44

If 1.0 L of 1.0 M HCl spilled and needed to be neutralized, how many grams of the solid sodium carbonate (Na₂CO₃, 106 g/mol) would be required?

A) 53 g
B) 106 g
C) 1,060 g
D) 530 g
E) 212 g

Question 45

What would be the products in the overall ionic equation for the following reaction?
2HBr(aq) + 2KOH(aq) $\rightarrow$ products
I. K⁺(aq) and Br ^-(aq);
II. KH(aq);
III. H₂O(l );
IV. KBr(s);
V. BrOH(aq);
VI. KBr(aq)

A) I and III
B) III and IV
C) III and VI
D) II, III, and V
E) II and V

Question 46

Which picture best represents an atomic-level view of hydrochloric acid, which is a strong acid, in aqueous solution (water molecules not shown)?

A)
B)
C)
D)

Question 47

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^-
D) H₃O⁺ and Cl^-
E) Ca²⁺, Cl^-, H₃O⁺, and OH^-

Question 48

Which one of the following is not a polyprotic acid?

A) sulfuric acid, H₂SO₄
B) phosphoric acid, H₃PO₄
C) carbonic acid, H₂CO₃
D) hydrogen sulfide, H₂S
E) acetic acid, CH₃COOH

Question 49

Identify the base in the following acid-base reaction.
PbCO₃(s) + H₂SO₄(aq) $\rightarrow$ PbSO₄(s) + CO₂(g) + H₂O(l)

A) CO₃^2-
B) CO₂
C) SO₄^2-
D) H₂O
E) H₂SO₄

Question 50

Hartmann's solution is used in intravenous therapy to replace lost body fluid and mineral salts. Hartmann's solution contains 5.00 mM potassium chloride, 2.00 mM calcium chloride, and
102 mM sodium chloride. What is the total chloride ion concentration in Hartmann's solution?

A) 109 mM
B) 107 mM
C) 111 mM
D) 104 mM
E) 218 mM

Question 51

Which one of the following statements regarding a strong acid is not correct?

A) A strong acid ionizes completely in water.
B) A strong acid ionizes in water to produce hydronium ions.
C) A strong acid neutralizes bases.
D) HCl is an example of a strong acid.
E) Acids are only strong at a high concentration.

Question 52

What is the molar concentration of sodium in a 200.0 mL solution prepared from 1.223 g of sodium phosphate (Na₃PO₄, 163.9 g/mol), which is a cleaning agent, food additive, and stain remover?

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

Question 53

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

A) A weak acid ionizes only to a small extent in water.
B) A weak acid ionizes in water to produce hydronium ions.
C) A weak acid neutralizes bases.
D) Acetic acid is an example of a weak acid.
E) All acids are weak at low concentrations.

Question 54

Identify the acid in the following acid-base reaction.
PbCO₃(s) + H₂SO₄(aq) $\rightarrow$ PbSO₄(s) + CO₂(g) + H₂O(l )

A) PbCO₃(s)
B) CO₂(g)
C) PbSO₄(s)
D) H₂O(l )
E) H₂SO₄(aq)

Question 55

A cross section of a Mad-Dawg gumball shows an outer layer of citric acid and malonic acid, beneath that a layer of food coloring, sugar, and flavoring, beneath that a layer of sodium bicarbonate (NaHCO₃), and finally in the middle-gum! A 12-year-old puts one in his mouth and immediately puckers, smiles, and then foams at the mouth before chewing. Where did the foam come from?

A) Twelve-year-olds naturally foam at the mouth.
B) The sodium bicarbonate explodes when exposed to moisture.
C) The acids react with the sodium bicarbonate, making unstable carbonic acid.
D) The foam must have been packed in the gum somewhere.
E) The acids react with the sugar, making a carbon volcano.

Question 56

Which one of the following reaction equations is the net ionic equation for the reaction of hydrochloric acid with lithium hydroxide? All species are in aqueous solution.

A) HCl + LiOH $\rightarrow$ LiCl + H₂O
B) H⁺ + Cl^- + Li⁺ + OH^- $\rightarrow$ Li⁺ + Cl^- + H₂O
C) H⁺ + Cl^- + Li⁺ + OH^- $\rightarrow$ LiCl + H₂O
D) Li⁺ + Cl^- $\rightarrow$ LiCl
E) H⁺ + OH^- $\rightarrow$ H₂O

Question 57

Which one of the following reaction equations is the molecular equation for the reaction of hydrochloric acid with sodium hydroxide? All species are in aqueous solution.

A) HCl + NaOH $\rightarrow$ NaCl + H₂O
B) H⁺ + Cl^- + Na⁺ + OH^- $\rightarrow$ Na⁺ + Cl^- + H₂O
C) H⁺ + Cl^- + Na⁺ + OH^- $\rightarrow$ NaCl + H₂O
D) Na⁺ + Cl^- $\rightarrow$ NaCl
E) H⁺ + OH^- $\rightarrow$ H₂O

Question 58

Identify a spectator ion in the following acid-base reaction.
Ca(CO₃)(s) + 2HCl(aq) $\rightarrow$ CaCl₂(aq) + 2H₂O(l ) + CO₂(g)

A) H⁺
B) Ca²⁺
C) Cl^-
D) CO₃^2-
E) H₃O⁺

Question 59

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 60

Chalk contains calcium carbonate. What would be the best solution for cleaning a sidewalk that a preschool class covered with smiling suns, flowers, birds, rainbows, and houses using sidewalk chalk?

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

Question 61

Ammonia (NH₃) is a weak base that reacts with a strong acid to form the ammonium ion, NH₄⁺. If 5.00 mL of a solution of an ammonia cleaner is titrated directly with 42.6 mL of 0.5000 M HCl, what is the concentration of the NH₃ in solution? (Assume that the ammonia is the only solute that reacts with the acid.)

A) 0.0587 M
B) 0.107 M
C) 4.26 M
D) 1.07 M
E) 5.87 M

Question 62

In carrying out a titration of a hydrochloric acid solution with a standard sodium hydroxide solution, a student went beyond the end point before reading the volume on the burette. That is, the volume used was larger than the volume required to reach the end point. How will this error affect the calculated concentration of the hydrochloric acid?

A) The calculated concentration will be larger than the actual concentration.
B) The calculated concentration will be smaller than the actual concentration.
C) The calculated concentration will be the correct concentration.
D) There is no way to tell how this error will affect the calculation.
E) The calculated concentration will be the actual concentration.

Question 63

Water-soluble toxic chromium compounds are waste products of electroplating operations, but the chromium can be precipitated as Cr(OH)₃ to remediate the water. How much 1.0 M NaOH solution is needed to remove the chromium from 100 L of a solution that is 0.001 M in Cr³⁺?

A) 100 mL
B) 300 mL
C) 10 L
D) 30 L
E) 33 L

Question 64

A 125 mL sample of orange juice was titrated using a redox reaction to the equivalence point with the addition of 7.6 mL of a 0.0025M iodine (I₂) solution. What is the concentration of vitamin C (C₆H₈O₆) in this sample?
C₆H₈O₆(aq) + I₂(aq) $\rightarrow$ C₆H₆O₆(aq) + 2I^-(aq) + 2H⁺(aq)

A) 30 mM
B) 15 mM
C) 19 mM
D) 0.30 mM
E) 0.15 mM

Question 65

Most chloride salts are soluble. Identify an exception to this generalization.

A) AgCl
B) CaCl₂
C) MgCl₂
D) BaCl₂
E) NaCl

Question 66

What mass of lead(II) chloride is produced when 200.0 mL of a 0.250 M solution of sodium chloride is mixed with 200.0 mL of a 0.250 M solution of lead(II) nitrate.

A) 13.9 g
B) 27.8 g
C) 3.48 g
D) 6.95 g
E) 1.39 g

Question 67

How many liters of 0.200 M NaOH solution are required to completely react with 1.00 L of
0)100 M HCN solution to produce sodium cyanide and water?

A) 0.25 L
B) 0.50 L
C) 1.00 L
D) 1.50 L
E) 2.00 L

Question 68

Which of the following compounds is most soluble in water?

A) AgCl
B) CaCO₃
C) Al(OH)₃
D) K₂SO₄
E) MgS

Question 69

Magnesium hydroxide is insoluble. Write the net ionic equation for the reaction that takes place between a solution of magnesium chloride and a solution of sodium hydroxide.

A) MgCl₂(aq) + NaOH(aq) $\rightarrow$ MgOH(s) + NaCl₂(aq)
B) MgCl₂(aq) + 2NaOH(aq) $\rightarrow$ Mg(OH)₂(s) + 2NaCl(aq)
C) Mg²⁺(aq) + 2OH^-(aq) $\rightarrow$ Mg(OH)₂(s)
D) Mg²⁺(aq) + 2Cl^- (aq) + 2Na⁺(aq) + 2OH^-(aq) $\rightarrow$ Mg(OH)₂(s) + 2NaCl(s)
E) Mg²⁺(aq) + OH^-(aq) $\rightarrow$ MgOH(s)

Question 70

Which one of the following water solubility guidelines A-D is not valid?

A) Salts with an alkali metal cation are soluble.
B) Salts with a nitrate anion are soluble.
C) Most ionic compounds with chloride and bromide anions are soluble.
D) Salts with the ammonium ion are soluble.
E) The guidelines A-D all are valid.

Question 71

Hard water contains Mg²⁺ and Ca²⁺ ions and 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 bathochromic shift.
E) bad housekeeping.

Question 72

Silver salts are used in black-and-white photography. Owing to the value of silver, the ions left in developing solutions are often collected by precipitation reactions for recycling. A 4.5 L jug of a developing solution was treated with an excess of sodium chloride, and a precipitate containing 2.86 g of dry silver chloride was collected. What was the molar concentration of the silver ions in the developing solution? The net ionic equation is
Ag⁺(aq) + Cl^-(aq) $\rightarrow$ AgCl(s)

A) 2.9 M
B) 5.9 *10^-3 M
C) 2.9 *10^-3 M
D) 4.4 * 10^-3 M
E) 4.4 M

Question 73

What mass of barium sulfate (233 g/mol) is produced when 125 mL of a 0.150 M solution of barium chloride is mixed with 125 mL of a 0.150 M solution of iron(III) sulfate?

A) 7.59 g
B) 3.65 g
C) 13.1 g
D) 18.8 g
E) 4.37 g

Question 74

Which of the following ionic compounds is insoluble in water?

A) BaCl₂
B) BaSO₄
C) NaOH
D) Ba(NO₃)₂
E) MgCl₂

Question 75

What mass of silver chloride will be recovered if excess sodium chloride is added to 500 mL of solution containing 10.79 g of Ag⁺?

A) 10.8 g
B) 21.6 g
C) 28.6 g
D) 7.2 g
E) 14.3 g

Question 76

In a titration, the solution of known concentration delivered by the burette is called the titrant, and the solution being titrated is called the analyte. To carry out a calculation to determine an unknown concentration of a sample from titration data, one would need all of the following data except __________

A) the volume of the titrant delivered.
B) the volume of the analyte.
C) the stoichiometry of the reaction between the titrant and the analyte.
D) the concentration of the analyte.
E) the concentration of the titrant.

Question 77

What mass of barium sulfate (233 g/mol) is produced when 125 mL of a 0.150 M solution of barium chloride is mixed with 25 mL of a 0.175 M solution of iron(III) sulfate?

A) 3.06 g
B) 1.02 g
C) 13.1 g
D) 18.8 g
E) 4.37 g

Question 78

A 500 mg dietary supplement of L-lysine (an amino acid, 146.2 g/mol) required 68.4 mL of
0)100 M NaOH to reach the end point. How many protons were removed for each L-lysine molecule in this titration?

A) 1
B) 2
C) 3
D) 0.500
E) 2.5

Question 79

Sodium thiosulfate (Na₂S₂O₃, molar mass = 158.2 g/mol) is used in the development of photographic film. Your summer job is at a photography lab and you need to check the purity of an outdated supply. You react 40.21 mL of 0.246 M iodine solution with a 3.232 g sample. What is the percent purity of the sodium thiosulfate that you report to your boss?
I₂(aq) + 2S₂O₃^2-(aq) $\rightarrow$ 2I^-(aq) + S₄O₆^2-(aq)

A) 100%
B) 48.4%
C) 96.8%
D) 98.6%
E) 84.4%

Question 80

A reaction that takes place between dissolved barium nitrate and dissolved sodium sulfate results in formation of solid barium sulfate. Which equation describes this reaction?

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