Azusa Pacific University

CHEM 101

week 4 review

1)The greater the hydronium ion concentration, the higher the pH. Select one:

True

False

2. A sample of orange juice has a pH of 3.44. Its [H3O+] is                . Select one:

a. 5.4 x 10-1 M

b. 3.6 x 10-4 M

c. 1.8 x 10-5

d. 2.7 x 10-3

3. Which of the following is the conjugate acid of the bicarbonate ion, HCO3-? Select one:

1. 1. H2CO3
   2. CO32-
   3. CO2
   4. H3O+

4. When stress is applied to a system at equilibrium such that the equilibrium is disturbed, the reaction proceeds in the direction that counteracts the disturbance. This explanation best describes      .

Select one:

1. Brønsted-Lowry concept
2. Ion-Ion attraction
3. Conjugate pair analysis
4. Le Châtelier’s principle

5. The equilibrium constant, Keq, for the ammonia synthesis below is found to be 6.0 x 10-2 at 500°C. Which of the following statements is true at equilibrium?

Select one:

1. Product concentration is greater than reactant concentration.
2. Reactant concentration is greater than product concentration.
3. Reactant concentration is the same as product concentration.
4. Relative concentrations of reactants and products cannot be predicted.

6. What volume of 0.200 M HCl is required to completely neutralize 50.00 mL of 0.150 M KOH? Select one:

1. 7.50 mL
2. 50.0 mL
3. 66.7 mL
4. 37.5 mL

7. Which of the following is the conjugate base of the bicarbonate ion, HCO3-? Select one:

1. H2CO3
2. CO32-
3. CO2
4. H3O+

8. Hydrogen sulfide ion, HS–, can react differently depending on the acidity of the solution in which it is present.

These two solutions show that the Select one:

1. hydrogen sulfide ion is an acid.
2. hydrogen sulfide ion is a base.
3. hydrogen sulfide ion is amphoteri
4. hydrogen sulfide ion can only react with water.

9. Excessive use of antacids can lead to Select one:

1. an increase in blood pH known as acidosis.
2. an increase in blood pH known as alkalosis.
3. a decrease in blood pH know as acidosis.
4. a decrease in blood pH known as alkylosis.

10. Which of the following is not a common characteristic of an acid? Select one:

1. it turns litmus pink/red
2. it tastes bitter
3. it dissolves common metals
4. all of these choices are common characteristics of acids Check

11. The higher the numerical value of an equilibrium constant (Keq), the further to the right the reaction will proceed.

Select one:

True

False

12. A solution in which the concentration of H+ is greater than the concentration of OH- will Select one:

1. have a pH greater than 7.0 and be basic.
2. have a pH less than 7.0 and be basic.
3. have a pH greater than 7.0 and be acidic.
4. have a pH less than 7.0 and be acidic.

13. The pH of blood is held reasonably stable by which buffer system? Select one:

1. H3PO4/H2PO4–

2. NaCl/Cl–
3. H2CO3/HCO3–
4. HCl/Cl–

14. You produce 500 mL of a 0.001 M HClO4, which ionizes completely in water. What is the pH you should expect?

Select one:

1. pH = 0.5
2. pH = 3.0
3. pH = 2.7
4. pH = 500

15. A catalyst lowers the activation energy for a chemical reaction. This increases the rate of the forward reaction and drives an equilibrium to the right.

Select one:

True

False

16. A common feature of carboxylic acids and phenols is that they contain an O-H group. Select one:

True

False

17. Amine salts formed from amines are mainly used in the drug industry because Select one:

1. they are acidic and react with bases.
2. they do not have a strong, unpleasant odor as do amines.
3. they are weak acids.
4. they are more soluble in water and blood fluids than the amine

18. The smell of rancid butter is due to the presence of butanoic acid. Select one:

True

False

19. The forces that hold one ester molecule to another are predominantly Select one:

1. hydrogen bonding.
2. dipole-dipole interactions and London forces.
3. ionic.
4. covalent.

20. Which of the following cannot participate in hydrogen bonding? Select one:

1. phenols
2. primary amines
3. secondary amines
4. tertiary amines

21. Salts of quaternary (4º) ammonium salts Select one:

1. have low boiling points.
2. have high melting points.
3. have weak covalent bonds.
4. are liquids at room temperature.

22. Carboxylic acids and alcohols can react under acidic conditions Select one:

1. to produce compounds that exist only under acidic conditions.
2. to produce esters with water being formed.
3. to produce phenols, if the appropriate hydrolyzing agents are present.
4. only if the carboxylic acid is an extremely strong acid.

23. The amide containing anti-flea drug Lufenuron is hydrophobic, therefore it dissolves easily in

        . Select one:

1. fatty tissue
2. aqueous solutions
3. hair
4. water

24. To which class of compounds would a physiological stimulant most likely belong? Select one:

1. carboxylic acids
2. phenols
3. alcohols
4. amines

25. The structure of amphetamine is shown.

Amphetamine is a              amine. Select one:

1. 1o
2. 2o
3. 3o
4. 4o

26. Rank butane (CH3CH2CH2CH3), butanoic acid (CH3CH2CH2COOH), and pentane (CH3CH2CH2CH2CH3) in order of increasing boiling point. (From lowest to highest.) Select one:

1. butane < butanoic acid < pentane
2. butane < pentane < butanoic acid
3. butanoic acid < pentane < butane
4. pentane < butanoic acid < butane

27. Carboxylic acids have lower boiling points than esters of similar size.

Select one:

True

False

28. Which of the following statements is true about nonane? Select one:

1. It is a polar molecule.
2. It dissolves in water.
3. It is a liquid at room temperature.
4. It contains one double bond.

29. Phenol and toluene (structures shown below) have similar molecular weights.

Which of the following statements accounts for the higher boiling point of phenol (182°C) than that of toluene (111°C)?

Select one:

1. Toluene is more soluble in water than phenol.
2. Phenol molecules are primarily attracted to one another by London forces.
3. Toluene has greater hydrogen bonding interactions than phenol.
4. Phenol molecules are primarily attracted to one another by hydrogen bonds.

30. Which of the following can participate in hydrogen bonding? Select one:

1. alcohols
2. carboxylic acids
3. primary amines
4. all of these choices

31. What is the molar concentration of hydronium ions in a sample of a soft drink that has a pH of 4?

Select one:

1. 1/4 M
2. 4 M
3. 1 x 104 M

d. 1 x 10-4 M

32. Which of the following structures is a constitutional isomer of 2-Methylheptane? The name of the following compound is

Select one:

1. 2,2,4-trimethylpentane.
2. 1,1,1,3-tetramethylbutane.
3. 1,1,1,3,3-pentamethylpropane.
4. Both 1,1,1,3-tetramethylbutane and 1,1,1,3,3-pentamethylpropane are correct names.

33. The ethylammonium ion, CH3CH2NH3+ has a pKa of 10.81. It reacts with water to form ethylamine, CH3CH2NH2

and H3O+ as shown below.

Which of the following statements is true at pH 7? Select one:

1. ethylammonium ion predominates
2. ethylamine predominates
3. the concentration of ethylamine equals that of ethylammonium ion
4. the pH is higher than pKa of the ethylammonium ion

34. The organic product of the reaction between NaOH and 3-methylbutanoic acid is named Select one:

1. 3-methylbutane sodium.
2. 3-methylbutanoate.
3. methylbutanoate.
4. sodium 3-methylbutanoate.

35. When a carboxylic acid or phenol reacts with a strong base, one of the products is the conjugate base of the carboxylic acid or the phenol.

Select one:

True

False

36. The equation:has the following equilibrium constant expression: Select one:

a.

b.

c.

d.

37. Provide IUPAC name for the following molecule. Select one:

1. 3-methyl-5-Hexene
2. 4-ethyl-1-pentene
3. 3-methyl-5-heptene
4. 4-methyl-1-hexene