Deck 4: Solution Chemistry: The Hydrosphere

Question 1

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

Answer 1

4.5 mM

Question 2

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

Answer 2

0.115 M

Question 3

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 3

sulfuric acid.

Question 4

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 5

Lead is the least toxic metal ion 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 6

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 7

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)55.5 moles
D)18.0 moles
E)100 moles

Question 8

What is the concentration, in g/L, of a 0.100 M sodium chloride solution?

A)1.71 g/L
B)5.84 g/L
C)584 g/L
D)11.7 g/L
E)3.42 g/L

Question 9

What are the units of molar concentration, M ?

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

Question 10

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 M
B)2.60 M
C)4.26 M
D)7.85 M
E)7.85 M

Question 11

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 12

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 13

A concentrated aqueous ammonia solution has a density of 0.90 g/mL and is 28.0% ammonia by mass. 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 14

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 M
B)1.99 M
C)2.63 M
D)1.19 M
E)0.263 M

Question 15

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 16

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 17

Mercury is one of the most toxic metal ions to fish, as they can only tolerate a concentration slightly above 1.5 mM. What is the mercury concentration in $\mu$ g/L?

A)6.0 $\mu$ g/L
B)12 $\mu$ g/L
C)30 $\mu$ g/L
D)75 $\mu$ g/L
E)1.5 $\mu$ g/L

Question 18

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 19

Which of the following cartoons depicts a solution?

A)
B)
C)
D)
E)

Question 20

A medical saline solution is prepared by mixing 55 mg of morphine (C₁₇H₁₉NO₃) with water to make 75.0 mL of solution. What is the millimolar concentration of this solution?

A)1.45 mM
B)2.57 mM
C)3.69 mM
D)14.5 mM
E)2.09 mM

Question 21

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 22

What volume of 12 M HCl solution needs to be diluted to produce 275 mL of 2.1 M HCl solution?

A)1.8 mL
B)9.2 mL
C)5.7 mL
D)23 mL
E)48 mL

Question 23

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 24

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 mL
E)83 mL

Question 25

Which of the following compounds is a strong electrolyte?

A)methane, CH₄
B)methanol, CH₃OH
C)ammonia, NH₃
D)hydrofluoric acid, HF
E)potassium chloride, KCl

Question 26

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

A)
B)
C)
D)

Question 27

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 28

What mass of potassium iodide (molar mass = 166.0 g/mol) is needed to produce 325.0 mL of a solution that has a concentration of 0.0150 M ?

A)2.94 g
B)0.809 g
C)809 g
D)7.66 g
E)1.31 g

Question 29

How many moles of ammonium hydroxide are present in 100 mL of a 0.17 M solution?

A)1.7 moles
B)5.8 moles
C)1.7 moles
D)1.7 moles
E)17 moles

Question 30

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 31

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

Question 32

How many moles of magnesium nitrate are present in 75.0 mL of a 0.33 M solution?

A)2.5 moles
B)25 moles
C)4.4 moles
D)2.3 moles
E)4.4 moles

Question 33

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

A)
B)
C)
D)

Question 34

How many grams of magnesium chloride, MgCl₂, are needed to make up 500.0 mL of a solution that is 0.300 M ?

A)14.3 g
B)57.1 g
C)158 g
D)1.58 g
E)1.75 g

Question 35

The World Health Organization recommends that the maximum allowable concentration of lead(II) in drinking water be limited to 0.015 mg/L. If the absorbance of lead(II) at 417 nm is 0.289 at this concentration, what is the molar absorptivity, assuming a 10-cm-long cell was used?'

A)4.0 M^-1
B)1.3 M^-1cm^-1
C)430 M^-1cm^-1
D)2.8 M^-1cm^-1
E)6.1 M^-1cm^-1

Question 36

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 37

Hartmann's solution is used in intravenous therapy to replace lost body fluid and mineral salts. The total ion concentration in Hartmann's solution is 276 mM. It often is prepared from a more concentrated stock solution. How much stock solution is needed to prepare 500 mL of Hartmann's solution? The total ion concentration in the stock solution is 1.38 M.

A)50 mL
B)10 mL
C)100 mL
D)500 mL
E)200 mL

Question 38

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

A)
B)
C)
D)

Question 39

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 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

What are the spectator ions in the reaction of barium hydroxide and nitric acid?

A)H₃O^- and NO₃^-
B)Ba²⁺ and OH^-
C)H₃O⁺ and OH^-
D)Ba²⁺ and NO₃^-
E)Ba²⁺, NO₃^-, H₃O⁺, and OH^-

Question 42

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

A)H⁺
B)Ca²⁺
C)Cl^-
D)CO₃^2-
E)H₃O⁺

Question 43

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 44

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

A)A weak base ionizes only to a small extent in water.
B)A weak base ionizes in water to produce hydroxide ions.
C)A weak base neutralizes acids.
D)Sodium hydroxide is an example of a weak base.
E)A weak base can also be a weak electrolyte.

Question 45

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 46

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 47

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 48

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 49

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 50

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 51

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 52

Identify the base in the following acid-base reaction. NaNO₂(aq) HI(aq) NaI(aq) HNO₂(aq)

A)Na⁺
B)NO₂^-
C)I^-
D)HI
E)HNO₂

Question 53

Which of the following compounds is a nonelectrolyte?

A)sulfuric acid, H₂SO₄
B)acetic acid, CH₃COOH
C)hexane, C₆H₁₄
D)nitrous acid, HNO₂
E)potassium hydroxide, KOH

Question 54

In the following reaction, H₂O ________ CH₃COOH(aq) H₂O(l) CH₃COO^-(aq) H₃O⁺(aq)

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 55

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

A)H⁺ Br ^- K⁺ OH^- KBr H₂O
B)H⁺ Br ^- K⁺ OH^- K⁺ Br ^- H₂O
C)HBr KOH KBr H₂O
D)K⁺ Br^- KBr
E)H⁺ OH^- H₂O

Question 56

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 57

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 LiCl H₂O
B)H⁺ Cl^- Li⁺ OH^- Li⁺ Cl^- H₂O
C)H⁺ Cl^- Li⁺ OH^- LiCl H₂O
D)Li⁺ Cl^- LiCl
E)H⁺ OH^- H₂O

Question 58

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

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

Question 59

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 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

Which of the following phosphate compounds is soluble in water?

A)Ag₃PO₄
B)Ca₃(PO₄)₂
C)(NH₄)₃PO₄
D)AlPO₄
E)Mg₃(PO₄)₂

Question 62

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 63

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 64

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 65

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) C₆H₆O₆(aq) 2I^-(aq) 2H⁺(aq)

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

Question 66

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

A)AgCl
B)CaCl₂
C)MgCl₂
D)BaCl₂
E)NaCl

Question 67

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 68

Which of the following compounds are soluble in water? PbCO₃ , Fe₂S₃ , AgNO₃, NH₄OH
I II III IV

A)I and II only
B)II and IV only
C)III and IV only
D)I, II, and IV only
E)All compounds are soluble.

Question 69

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 70

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 71

Which of the following ionic compounds is insoluble in water?

A)cesium fluoride
B)cesium chloride
C)cesium bromide
D)cesium iodide
E)All the compounds are soluble in water.

Question 72

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 73

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) 2I^-(aq) S₄O₆^2-(aq)

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

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

Most alkaline earth salts are soluble. Identify an exception to this generalization.

A)MgSO₄
B)CaS
C)Sr(OH)₂
D)BaSO₄
E)Ca(NO₃)₂

Question 76

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 77

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 78

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 79

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 80

In carrying out a titration of a potassium hydroxide solution with a standard hydrochloric acid solution, a student misread the volume on the burette. That is, the actual volume recorded was smaller than the volume required to reach the end point. How will this error affect the calculated concentration of the potassium hydroxide solution?

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 determine how this error will affect the calculation.
E)The calculated concentration will be the actual concentration.