Deck 4: Chemical Reactions and Solutions Stoichiometry

Question 1

A 38.1-g sample of SrCl₂ is dissolved in 112.5 mL of solution.Calculate the molarity of this solution.

A)27.0 M
B)2.14 M
C)53.7 M
D)0.339 M
E)none of these

Answer 1

2.14 M

Question 2

Which of the following aqueous solutions contains the greatest number of ions?

A)400.0 mL of 0.10 M NaCl
B)300.0 mL of 0.10 M CaCl₂
C)200.0 mL of 0.10 M FeCl₃
D)200.0 mL of 0.10 M KBr
E)800.0 mL of 0.10 M sucrose

Answer 2

300.0 mL of 0.10 M CaCl₂

Question 3

Polar molecules have an unequal distribution of charge within the molecule.

Answer 3

True

Question 4

How many grams of NaCl are contained in 350.mL of a 0.287 M solution of sodium chloride?

A)16.8 g
B)5.87 g
C)11.74 g
D)100.5 g
E)none of these

Question 5

All of the following are weak acids except

A)HCNO
B)HBr
C)HF
D)HNO₂
E)HCN

Question 6

Consider two organic molecules,ethanol and benzene.One dissolves in water and the other does not.Why?

A)They have different molar masses.
B)One is ionic,the other is not.
C)One is an electrolyte,the other is not.
D)Ethanol contains a polar O-H bond,and benzene does not.
E)Two of these are correct.

Question 7

The man who discovered the essential nature of acids through solution conductivity studies is

A)Priestly
B)Boyle
C)Einstein
D)Mendeleev
E)Arrhenius

Question 8

A solid acid HX is mixed with water.Two possible solutions can be obtained.Which of the following is true? I. II.

A)In case I,HX is acting like a weak acid,and in case II,HX is acting like a strong acid.
B)In case I,HX is acting like a strong acid,and in case II,HX is acting like a weak acid.
C)In both cases,HX is acting like a strong acid.
D)In both cases,HX is acting like a weak acid.
E)HX is not soluble in water.

Question 9

What mass of calcium chloride,CaCl₂,is needed to prepare 3.950 L of a 1.49 M solution?

A)294 g
B)5.89 g
C)41.9 g
D)111 g
E)653 g

Question 10

A 74.28-g sample of Ba(OH)₂ is dissolved in enough water to make 2.450 liters of solution.How many mL of this solution must be diluted with water in order to make 1.000 L of 0.100 M Ba(OH)₂?

A)565 mL
B)177 mL
C)17.7 mL
D)4.34 mL
E)231 mL

Question 11

An unknown substance dissolves readily in water but not in benzene (a nonpolar solvent).Molecules of what type are present in the substance?

A)neither polar nor nonpolar
B)polar
C)either polar or nonpolar
D)nonpolar
E)none of these

Question 12

An acid is a substance that produces OH^- ions in water.

Question 13

How many grams of NaOH are contained in 5.0 $\times$ 10² mL of a 0.74 M sodium hydroxide solution?

A)15 g
B)74 g
C)0.37 g
D)30 g
E)370 g

Question 14

Which of the following is a strong acid?

A)HF
B)KOH
C)HClO₄
D)HClO
E)HBrO

Question 15

A 16.4-g sample of HF is dissolved in water to give 2.0 $\times$ 10² mL of solution.The concentration of the solution is:

A)0.82 M
B)0.16 M
C)0.08 M
D)4.1 M
E)8.2 M

Question 16

What mass of solute is contained in 256 mL of a 0.838 M ammonium chloride solution?

A)11.5 g
B)175 g
C)16.3 g
D)215 g
E)3.27 g

Question 17

Which of the following is not a strong base?

A)Ca(OH)₂
B)KOH
C)NH₃
D)LiOH
E)Sr(OH)₂

Question 18

Which of the following is paired incorrectly?

A)H₂SO₄ - strong acid
B)HNO₃ - weak acid
C)Ba(OH)₂ - strong base
D)HCl - strong acid
E)NH₃ - weak base

Question 19

What volume of 18 M sulfuric acid must be used to prepare 2.30 L of 0.145 M H₂SO₄?

A)19 mL
B)0.33 mL
C)1.1 $\times$ 10³ mL
D)2.9 mL
E)6.0 mL

Question 20

The interaction between solute particles and water molecules,which tends to cause a salt to fall apart in water,is called

A)hydration
B)polarization
C)dispersion
D)coagulation
E)conductivity

Question 21

You have two solutions of sodium chloride.One is a 2.00 M solution,the other is a 4.00 M solution.You have much more of the 4.00 M solution and you add the solutions together.Which of the following could be the concentration of the final solution?

A)2.70 M
B)3.00 M
C)3.50 M
D)6.00 M
E)8.10 M

Question 22

When NH₃(aq)is added to Cu²⁺(aq),a precipitate initially forms.Its formula is:

A)Cu(NH)₃
B)Cu(NO₃)₂
C)Cu(OH)₂
D)Cu(NH₃)₂²⁺
E)CuO

Question 23

Diabetics often need injections of insulin to help maintain the proper blood glucose levels in their bodies.How many moles of insulin are needed to make up 45 mL of 0.0062 M insulin solution?

A)0.00056 mol
B)0.14 mol
C)7.3 mol
D)0.28 mol
E)0.00028 mol

Question 24

The following reactions
2K(s)+ Br₂(l) $\to$ 2KBr(s)
AgNO₃(aq)+ NaCl(aq) $\to$ AgCl(s)+ NaNO₃(aq)
HCl(aq)+ KOH(aq) $\to$ H₂O(l)+ KCl(aq)
Are examples of

A)precipitation reactions
B)redox,precipitation,and acid-base,respectively
C)precipitation (two)and acid-base reactions,respectively
D)redox reactions
E)none of these

Question 25

All of the following reactions
2Al(s)+ 3Br₂(l) $\to$ 2AlBr₃(s)
2Ag₂O(s) $\to$ 4Ag(s)+ O₂(g)
CH₄(l)+ 2O₂(g) $\to$ CO₂(g)+ 2H₂O(g)
Can be classified as

A)oxidation-reduction reactions
B)combustion reactions
C)precipitation reactions
D)A and B
E)A and C

Question 26

For the reaction 4FeCl₂(aq)+ 3O₂(g) $\to$ 2Fe₂O₃(s)+ 4Cl₂(g),what volume of a 0.760 M solution of FeCl₂ is required to react completely with 6.36 $\times$ 10²¹ molecules of O₂?

A)5.26 $\times$ 10³ mL
B)10.7 mL
C)10.4 mL
D)18.5 mL
E)6.02 mL

Question 27

The following reactions:
Pb²⁺ + 2I^- $\to$ PbI₂
2Ce⁴⁺ + 2I^- $\to$ I₂ + 2Ce³⁺
HOAc + NH₃ $\to$ NH₄⁺ + OAc^-
Are examples of

A)acid-base reactions
B)unbalanced reactions
C)precipitation,acid-base,and redox reactions,respectively
D)redox,acid-base,and precipitation reactions,respectively
E)precipitation,redox,and acid-base reactions,respectively

Question 28

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?

A)Ba(OH)₂
B)NaNO₃
C)K₂SO₄
D)Cu(NO₃)₂
E)none of these

Question 29

How many of the following salts are expected to be insoluble in water? sodium sulfide
Barium nitrate
Ammonium sulfate
Potassium phosphate

A)none
B)1
C)2
D)3
E)4

Question 30

Which of the following do you need to know to be able to calculate the molarity of a salt solution?
I.the mass of salt added
II.the molar mass of the salt
III.the volume of water added
IV.the total volume of the solution

A)I,III
B)I,II,III
C)II,III
D)I,II,IV
E)You need all of the information.

Question 31

Phosphoric acid,H₃PO₄,is a triprotic acid.What is the total number of moles of H⁺ available for reaction in 2.50 L of 0.700 M H₃PO₄?

A)0.233 mole
B)2.10 mole
C)0.583 mole
D)3.00 moles
E)5.25 moles

Question 32

A 230.0-mL sample of a 0.275 M solution is left on a hot plate overnight; the following morning the solution is 1.29 M. What volume of solvent has evaporated from the 0.275 M solution?

A) 49.0 mL
B) 63.3 mL
C) 181.0 mL
D) 230. mL
E) 279.0 mL

Question 33

You have equal masses of different solutes dissolved in equal volumes of solution.Which of the solutes would make the solution having the highest molar concentration?

A)NaOH
B)KCl
C)KOH
D)LiOH
E)all the same

Question 34

Which of the following ions is most likely to form an insoluble sulfate?

A)K⁺
B)Li⁺
C)Ca²⁺
D)S^2-
E)Cl^-

Question 35

Which of the following salts is insoluble in water?

A)Na₂S
B)K₂CO₃
C)Pb(NO₃)₂
D)CaCl₂
E)All of these are soluble in water.

Question 36

The concentration of a salt water solution that sits in an open beaker decreases over time.

Question 37

The following reactions
ZnBr₂(aq)+ 2AgNO₃(aq) $\to$ Zn(NO₃)₂(aq)+ 2AgBr(s)
KBr(aq)+ AgNO₃(aq) $\to$ AgBr(s) + KNO₃(aq)
Are examples of

A)oxidation-reduction reactions
B)acid-base reactions
C)precipitation reactions
D)A and C
E)none of these

Question 38

An analytical procedure requires a solution of chloride ions.How many grams of NaCl must be dissolved to make 1.95 L of 0.0561 M Cl^-?

A)3.28 g
B)0.595 g
C)6.39 g
D)1.64 g
E)12.8 g

Question 39

Aqueous solutions of sodium sulfide and copper(II)chloride are mixed together.Which statement is correct?

A)Both NaCl and CuS precipitate from solution.
B)No reaction will occur.
C)CuS will precipitate from solution.
D)NaCl will precipitate from solution.
E)A gas is released.

Question 40

Aqueous solutions of potassium sulfate and ammonium nitrate are mixed together.Which statement is correct?

A)Both KNO₃ and NH₄SO₄ precipitate from solution.
B)A gas is released.
C)NH₄SO₄ will precipitate from solution.
D)KNO₃ will precipitate from solution.
E)No reaction will occur.

Question 41

You mix 275.0 mL of 1.20 M lead(II)nitrate with 300.0 mL of 1.85 M potassium iodide.The lead(II)iodide is insoluble.Which of the following is false?

A)The final concentration of Pb²⁺ ions is 0.0913 M.
B)You form 128 g of lead(II)iodide.
C)The final concentration of K⁺ is 0.965 M.
D)The final concentration of NO₃^- is 0.965 M.
E)All are true.

Question 42

The filtrate is the solid formed when two solutions are mixed.

Question 43

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?

A)AgCl (s)
B)2AgCl (s)
C)2Ba(NO₃)₂ (aq)
D)BaNO₃ (aq)
E)3AgCl (aq)

Question 44

If all of the chloride in a 3.734-g sample of an unknown metal chloride is precipitated as AgCl with 70.90 mL of 0.2010 M AgNO₃,what is the percentage of chloride in the sample?

A)50.52%
B)13.53%
C)1.425%
D)7.391%
E)none of the above

Question 45

When sodium chloride and lead(II)nitrate react in an aqueous solution,which of the following terms will be present in the balanced molecular equation?

A)PbCl(s)
B)Pb₂Cl(s)
C)NaNO₃(aq)
D)2NaNO₃(aq)
E)2PbCl₂(s)

Question 46

Aqueous solutions of barium chloride and silver nitrate are mixed to form solid silver chloride and aqueous barium nitrate.
The balanced complete ionic equation contains which of the following terms?

A)2Ba²⁺(aq)
B)Cl^-(aq)
C)2Ag⁺(aq)
D)NO₃^- (aq)
E)AgCl(aq)

Question 47

The net ionic equation for the reaction of calcium bromide and sodium phosphate contains which of the following species?

A)2Br^-(aq)
B)PO₄^3-(aq)
C)2Ca₃(PO₄)₂(s)
D)6NaBr(aq)
E)3Ca²⁺(aq)

Question 48

Consider an aqueous solution of calcium nitrate added to an aqueous solution of sodium phosphate.Write and balance the equation for this reaction to answer the following question.What is the sum of the coefficients when the molecular equation is balanced in standard form?

A)4
B)5
C)7
D)11
E)12

Question 49

Which of the following compounds is soluble in water?

A)Ni(OH)₂
B)K₃PO₄
C)BaSO₄
D)CoCO₃
E)PbCl₂

Question 50

A mixture of BaCl₂ and NaCl is analyzed by precipitating all the barium as BaSO₄.After addition of an excess of Na₂SO₄ to a 3.725-g sample of the mixture,the mass of precipitate collected is 2.734 g.What is the mass percentage of barium chloride in the mixture?

A)82.28%
B)73.40%
C)43.18%
D)65.47%
E)19.60%

Question 51

When solutions of cobalt(II)chloride and carbonic acid react,which of the following terms will be present in the net ionic equation?

A)CoCO₃(s)
B)H⁺(aq)
C)2CoCO₃(s)
D)2Cl^-(aq)
E)two of these

Question 52

Which pair of ions would not be expected to form a precipitate when dilute solutions of each are mixed?

A)Al³⁺,S^2-
B)Pb²⁺,Cl^-
C)Ba²⁺,PO₄^3-
D)Pb²⁺,OH^-
E)Mg²⁺,SO₄^2-

Question 53

A solution contains the ions Ag⁺,Pb²⁺,and Ni²⁺.Dilute solutions of NaCl,Na₂SO₄,and Na₂S are available to separate the positive ions from each other.In order to effect separation,the solutions should be added in which order?

A)Na₂SO₄,NaCl,Na₂S
B)Na₂SO₄,Na₂S,NaCl
C)Na₂S,NaCl,Na₂SO₄
D)NaCl,Na₂S,Na₂SO₄
E)NaCl,Na₂SO₄,Na₂S

Question 54

In writing the complete ionic equation for the reaction (if any)that occurs when aqueous solutions of KOH and Mg(NO₃)₂ are mixed,which of the following would not be written as ionic species?

A)KOH
B)Mg(NO₃)₂
C)Mg(OH)₂
D)KNO₃
E)All of the above would be written as ionic species.

Question 55

When solutions of phosphoric acid and iron(III)nitrate react,which of the following terms will be present in the balanced molecular equation?

A)HNO₃(aq)
B)3HNO₃(aq)
C)2FePO₄(s)
D)3FePO₄(s)
E)2HNO₃(aq)

Question 56

When solutions of strontium chloride and sodium sulfate react,which of the following is a spectator ion?

A)strontium ion
B)chloride ion
C)sodium ion
D)sulfate ion
E)two of these

Question 57

The net ionic equation for the reaction of aluminum sulfate and sodium hydroxide contains which of the following species?

A)3Al³⁺(aq)
B)OH^-(aq)
C)3OH^-(aq)
D)2Al³⁺(aq)
E)2Al(OH)₃(s)

Question 58

Consider the reaction between 15.0 mL of a 1.00 M aqueous solution of AgNO₃ and 10.0 mL of a 1.00 M aqueous solution of K₂CrO₄.When these react,a precipitate is observed.What is present in solution after the reaction is complete? Note: the solid is not considered to be in solution.

A)Ag⁺,NO₃^-,K⁺,CrO₄^2-,water
B)Ag⁺,NO₃^-,K⁺,water
C)K⁺,CrO₄^2-,water
D)NO₃^-,K⁺,CrO₄^2-,water
E)water

Question 59

Consider an aqueous solution of calcium nitrate added to an aqueous solution of sodium phosphate.What is the formula of the solid formed in the reaction?

A)Ca(PO₄)₂
B)CaPO₄
C)Ca₃(PO₄)₂
D)Ca₃(PO₃)₂
E)none of these

Question 60

The net ionic equation contains which of the following terms?

A)Ag⁺(aq)
B)Ba²⁺(aq)
C)NO₃^- (aq)
D)H⁺ (aq)
E)AgCl(aq)

Question 61

A student weighs out 0.512 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.

A)0.00251 M
B)0.092 M
C)0.0139 M
D)0.0682 M
E)none of these

Question 62

You mix 55 mL of 1.00 M silver nitrate with 25 mL of 0.84 M sodium chloride.What mass of silver chloride should you form?

A)3.0 g
B)6.0 g
C)3.3 g
D)6.6
E)none of these

Question 63

An unknown diprotic acid requires 44.39 mL of 0.111 M NaOH to completely neutralize a 0.580-g sample.Calculate the approximate molar mass of the acid.

A)406 g/mol
B)235 g/mol
C)118 g/mol
D)59 g/mol
E)203 g/mol

Question 64

When solutions of carbonic acid and aluminum hydroxide react,which of the following are NOT present in the net ionic equation? I.
Hydrogen ion
II.
Carbonate ion
III.
Aluminum ion
IV.
Hydroxide ion

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

Question 65

When solutions of carbonic acid and potassium hydroxide react,which of the following are NOT present in the complete ionic equation?

A)hydrogen ion
B)carbonate ion
C)potassium ion
D)hydroxide ion
E)water

Question 66

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.

A)247 g/mol
B)171 g/mol
C)165 g/mol
D)151 g/mol
E)82.7 g/mol

Question 67

Sulfamic acid,HSO₃NH₂ (molar mass = 97.1 g/mol),is a strong monoprotic acid that can be used to standardize a strong base: A 0.165-g sample of HSO₃NH₂ required 19.4 mL of an aqueous solution of KOH for a complete reaction.What is the molarity of the KOH solution?

A)0.00170 M
B)8.76 M
C)0.0876 M
D)0.0330 M
E)none of these

Question 68

When solutions of carbonic acid and copper(II)hydroxide react,which of the following are spectator ions?

A)hydrogen ion
B)carbonate ion
C)copper(II)ion
D)hydroxide ion
E)none of these

Question 69

With what volume of 5.00 M HF will 4.72 g of calcium hydroxide react completely,according to the following reaction?

A)12.7 mL
B)127 mL
C)637 mL
D)25.5 mL
E)39.2 mL

Question 70

You have 88.6 mL of a 2.50 M solution of Na₂CrO₄(aq).You also have 125 mL of a 2.50 M solution of AgNO₃(aq).Calculate the concentration of Na⁺ after the two solutions are mixed together.

A)0.00 M
B)1.04 M
C)2.07 M
D)5.00 M
E)0.443 M

Question 71

What mass of NaOH is required to react exactly with 25.0 mL of 2.7 M H₂SO₄?

A)2.7 g
B)0.7 g
C)5.4 g
D)135 g
E)none of these

Question 72

A 3.00-g sample of an alloy (containing only Pb and Sn)was dissolved in nitric acid (HNO₃).Sulfuric acid was added to this solution,which precipitated 2.37 g of PbSO₄.Assuming that all of the lead was precipitated,what is the percentage of Sn in the sample? (molar mass of PbSO₄ = 303.3 g/mol)

A)46.0% Sn
B)0.781% Sn
C)79.0% Sn
D)54.0% Sn
E)1.62% Sn

Question 73

You have 75.0 mL of a 2.50 M solution of Na₂CrO₄(aq).You also have 125 mL of a 2.01 M solution of AgNO₃(aq).Calculate the concentration of CrO₄^2- after the two solutions are mixed together.

A)0.00 M
B)0.309 M
C)0.938 M
D)0.251 M
E)2.50 M

Question 74

You have 75.0 mL of a 2.50 M solution of Na₂CrO₄(aq).You also have 125 mL of a 1.88 M solution of AgNO₃(aq).Calculate the concentration of NO₃^- after the two solutions are mixed together.

A)0.00 M
B)0.588 M
C)1.18 M
D)2.35 M
E)4.50 M

Question 75

A mixture contained no fluorine compound except methyl fluoroacetate,FCH₂COOCH₃ (molar mass = 92.07 g/mol).When chemically treated,all the fluorine was converted to CaF₂ (molar mass = 78.08 g/mol).The mass of CaF₂ obtained was 35.8 g.Find the mass of methyl fluoroacetate in the original mixture.

A)60.7 g
B)84.4 g
C)30.4 g
D)42.2 g
E)21.1 g

Question 76

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?

A)The HCl solution.
B)The H₂SO₄ solution.
C)You need to know the acid concentrations to answer this question.
D)You need to know the volume and concentration of the NaOH solution to answer this question.
E)C and D

Question 77

A 1.59-g sample of a metal chloride,MCl₂,is dissolved in water and treated with excess aqueous silver nitrate.The silver chloride that formed weighed 3.60 g.Calculate the molar mass of M.

A)70.9 g/mol
B)28 g/mol
C)55.9 g/mol
D)63 g/mol
E)72.4 g/mol

Question 78

In the balanced molecular equation for the neutralization of sodium hydroxide with sulfuric acid,the products are:

A)NaSO₄ + H₂O
B)NaSO₃ + 2H₂O
C)2NaSO₄ + H₂O
D)Na₂S + 2H₂O
E)Na₂SO₄ + 2H₂O

Question 79

You have 75.0 mL of a 2.50 M solution of Na₂CrO₄(aq).You also have 125 mL of a 1.72 M solution of AgNO₃(aq).Calculate the concentration of Ag⁺ after the two solutions are mixed together.

A)0.00 M
B)0.538 M
C)1.08 M
D)0.088 M
E)0.215 M

Question 80

A chemical that changes color at the endpoint of a reaction is called a colorimeter.