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Solutions and Acid Base Honors Chemistry

Total questions: 74

Worksheet time: 2hrs 34mins

Name
Class
Date
1.

Based on the solubility chart, what is the solubility of KClO3 at 60oC in 100 g of water?

a)

65 g

b)

32 g

c)

50 g

d)

23 g

2.

Properties that only depend on the number of solute particles dissolved and not the identity of the solute are called

a)

cohesive

b)

colligative

c)

collaborative

d)

conductive

3.
According to the pH scale, which of the following would be true?
a)
baking soda is a weak base while drain cleaner is a strong base
b)
lemon is a weaker acid than a banana
c)
tomato and soap are acidic
d)
vinegar is less acidic than an apple
4.
Which of the following would NOT be a way to speed up the rate of solubility of rock salt?
a)
stir it
b)
heat the water
c)
crush the salt
d)
cool the water
5.
Which characteristics describe a base?
a)
sour, indicator turns red, pH less than 7, produces hydrogen ions (H+)
b)
bitter, slippery, indicator turns blue, pH greater than 7, produces hydroxide ions (OH-)
c)
neutral, pH of 7
d)
sour, indicator turns red, pH greater than 7
6.
Which characteristics describe an acid?
a)
sour, indicator turns red, pH less than 7, produces hydrogen ions (H+)
b)
bitter, slippery, indicator turns blue, pH greater than 7, produces hydroxide ions (OH-)
c)
neutral, pH of 7
d)
sour, indicator turns red, pH greater than 7
7.
An extremely strong base would have a pH of...
a)
1
b)
7
c)
9
d)
14
8.
A neutral substance would have pH of...
a)
8
b)
7
c)
6
d)
14
9.
pH less than 7.
a)
Acids
b)
Bases
c)
All
10.
The pH scale is based off of the concentration of _________ ions.
a)
Oxygen
b)
Hydrogen
c)
Nitrogen
d)
None of the others
11.

Arrhenius base

a)

Any compound that produces H+ ions

b)

Any compound that produces OH- ions

c)
Ionic compound formed from a metal and a nonmetal
d)
A charged particle, atom, or ion
12.
Neutralization
a)
Compound formed by a metal and a nonmetal
b)
The reaction between an acid and a base which produces a salt and water
c)
A chemical whose color changes in the presence of acids and bases
d)
To decrease the amount of solute as compared to the amount of solvent in a solution
13.

The substance that does the dissolving

a)

Solute

b)

Solvent

c)

Solution

d)

Miscibility

14.

The substance getting dissolved

a)

Solvent

b)

Solute

c)

Solution

d)

Mixture

15.

If I want more sugar to dissolve in water, I should heat the water

a)

true

b)

false

16.

If I want my salt to dissolve in water faster, I should stir the water

a)

true

b)

false

17.

Molality is defined as ________ divided by _____________

a)

liters solution, mols solute

b)

mols solute, liters solvent

c)

kg solvent, mols solute

d)

mols solute, kg solvent

18.

Molarity concentration is abbreviated as _________

a)

MM.

b)

m.

c)

Mol.

d)

M.

19.

Molarity is defined as _________ divided by ___________

a)

mol, liters

b)

mol, kg

c)

kg, liters

d)

liters, kg

20.

How many mols of HCl are in 3000. mL of 2.0M HCl solution?

a)

2.0

b)

1.5

c)

6.0

d)

0.66

21.

When the theoretical maximum amount of solute has dissolved, the solution is _________

a)

supersaturated

b)

unsaturated

c)

saturated

d)

megasaturated

22.

What does "like dissolves like" mean?

a)

polar solvents dissolve in polar solutes

b)

polar solutes dissolve in polar solvents

c)

non-polar solvents dissolve in polar solutes

d)

non-polar solutes dissolve in polar solvents

23.
An electrolyte is...
a)
The rapid, random movement of particles in colloidal dispersion.
b)
A substance that dissolves in water and conducts electric current.
c)
A substance that dissolves in water and does not conduct electric current.
d)
The solution process when water is the solvent.
24.

Conditions associated with a sucrose (sugar) solution are plotted as point A. This solution would be considered

a)

Unsaturated

b)

Supersaturated

c)

Saturated

d)

Undefined

25.

Conditions associated with a sugar solution are plotted as point C. This graph represents a(n) ___ solution

a)

saturated

b)

supersaturated

c)

unsaturated

d)

undefined

26.

What is the molality of a solution made by dissolving 2 moles of NaOH in 400 grams of water?

a)

5 mol/kg solvent

b)

4 mol/kg solvent

c)

3 mol/kg solvent

d)

0.005 moles/kg solvent

27.
How many moles of NaCl are present in a solution with a molarity of 8.59 M and a volume of 125 mL?
a)
1074 mol
b)
0.069 mol
c)
1.07 mol
d)
62.7 mol
28.

What do molarity and molality have in common?

a)

Both have "moles solute" in the numerator

b)

Both have "kg solvent" in the denominator

c)

Both have "L solution" in the denominator

d)

Both have "moles solution" in the denominator

29.

What is the molality of a solution in which 3.0 moles of NaCl is dissolved in 1.5 Kg of water? (Careful of the unit!)

a)

2.0 M

b)

0.22 m

c)

140 m

d)

2.0 m

30.

How many mL of stock solution of 2.00 M NaCl do you need to prepare 100.0 mL of 0.150 M NaCl?

a)

7.50 mL

b)

15.0 mL

c)

1330 mL

d)

200. mL

31.

How many grams of solute are dissolved in 125.0 mL of 5.00 M NaCl (MM = 58.45 g/mol)?

a)

0.625 g NaCl

b)

625 g NaCl

c)

36.5 g NaCl

d)

0.04 mol NaCl

32.

How many mL of 1.00 M KBr solution would you need to prepare 250. mL of a 0.200 M dilution?

a)

175 mL

b)

250. mL

c)

50.0 mL

d)

5.00 mL

33.

When CH3OH is dissolved in water, how many particles are in solution for each unit?

a)

1

b)

3

c)

4

d)

5

e)

6

34.

When CaBr2 is dissolved in water, how many particles will be in solution for each unit?

a)

1

b)

2

c)

3

d)

4

e)

5

35.

Adding a nonvolatile solute to a liquid will ___.

a)

depress both the freezing point and the boiling point

b)

elevate both the freezing point and the boiling point

c)

depress the freezing point and elevate the boiling point

d)

elevate the freezing point and depress the boiling point

36.

If the [H+] of a solution is 1 x 10-2 M the pH is

a)

2

b)

12

c)

-2

d)

1

37.
If the pH of a solution is 5 the [H+] is
a)
1.0 x 105  M
b)
1.0 x 109  M
c)
5.0 x 101  M
d)
1.0 x 10-5  M
38.
If the pH of a solution is 5.6 the pOH is
a)
6.5
b)
12.4
c)
8.4
d)
5.6
39.
A  pH and a pOH will add up to:
a)
0
b)
7
c)
14
d)
1.0 x 10-14
40.

If the [OH-] of a solution is 2.7 x 10-4 M the pOH of the solution is

a)

10.44

b)

3.56

c)

1.00

d)

-4.43

41.

A solution of NaCl has a molality of 1.0 m and a solution of CaCl2 has a molality of 1.0 m, which solution has the lower freezing point?

a)

NaCl

b)

CaCl2

c)

they are the same

d)

the freezing point is higher, not lower.

42.

If colligative properties don't depend on the identity of the solute, what is a reasonable explanation for why we don't spread sugar (C12H22O11) all over the roads in the winter instead of a salt like CaCl2.

a)

calcium chloride breaks up into 3 particles, but sugar only has 1.

b)

calcium chloride breaks up into 3 particles, but sugar breaks up into 45, making it very difficult to dissolve.

c)

sugar is more damaging to the environment than CaCl2

d)

sugar is less acidic than salt.

43.

The boiling point of a saltwater solution would likely be

a)

90 oC

b)

101 oC

c)

100 oC

d)

50oC

44.

HSO4-+ H2O ,<--> SO42- + H3O+

which statement is not true

a)

HSO4- is the acid

b)

H2O is the base

c)

SO42- is the conjugate base

d)

H3O+ is the conjugate base

45.

Which of the following substances would be considered a weak electrolyte?

a)

ethanol

b)

potassium chloride

c)

acetic acid

d)

all of the above

46.

A Bronsted Lowry base is also known as

a)

a proton acceptor

b)

a proton donor

c)

a substance that gives away its H+

d)

an Arrhenius acid

47.

Brine (salt water) is sometimes put on roads in the winter. Why?

a)

to lower the freezing point of water in the hope that the air temperature won't get cold enough for precipitation to form ice.

b)

to create an endothermic reaction to melt any ice that forms

c)

to act as a catalyst to lower the activation energy

d)

to increase the freezing point of water so ice doesn't form if the air temperature gets really cold.

48.

What is the pH of a 2.5 x 10-4 M Mg(OH)2 solution?

a)

5.0 x 10-4

b)

3.30

c)

10.70

d)

-10.70

49.

Check all that are true!! This is a picture of oil and water.

a)

oil is nonpolar

b)

oil is polar

c)

oil is more dense than water

d)

oil is less dense than water

50.

Which substance turned the pH paper red?

a)

bleach

b)

coke

c)

tums

d)

baking soda

51.

What is the name of H2SO4?

a)

sulfuric acid

b)

hydrosulfuric acid

c)

sulfurous acid

d)

hydrosulfurous acid

52.

What is the name of Mg(OH)2?

a)

magnesium dihydroxide

b)

magnesium hydroxide

c)

magnesium hydride

d)

magnesium dihydride

53.
PV=nRT
a)
Charles Law
b)
Boyle's Law
c)
Combined Gas Law
d)
Ideal Gas Law
54.
Calculate the volume that a 0.323-mol sample of a gas will occupy at 265 K and a pressure of 0.900 atm.
a)
7.18 L 
b)
7.81 L
c)
4.63 L
d)
4.36 L
55.
Determine the Kelvin temperature required for 0.0470 mol of gas to fill a balloon to 1.20 L under .998 atm pressure. 
a)
0 K 
b)
107 K 
c)
207 K 
d)
307 K 
56.

What does R stand for

a)

Ideal gas constant

b)

Real gas constant

c)

Temperature constant

d)

Ideal gas law

57.

Which is a correct unit for R?

a)

L.atm/mol.k

b)

L.atm

c)

mmHg/mol.K

d)

L.atom/mol

58.
Determine the Celsius temperature of 2.49 moles of gas contained in a 1.00-L vessel at a pressure of 143 kPa. 
a)
-266 degrees C
b)
-622 degrees C
c)
622 degrees C 
d)
266 degrees C
59.
What pressure, in atm, is exerted by 2.50 L of gas containing 1.35 mol at 320 K?
PV=nRT
a)
14.19 atm
b)
16.53 atm
c)
18.42 atm
d)
22.54 atm
60.

If a hairspray can is heated, what can be expected of the pressure of the gas inside the can?

a)

The pressure will increase

b)

The pressure will decrease

c)

The pressure will remain constant

d)

The pressure will equalize

61.
Which of the following would increase the (gas) pressure of a system?
a)
Increase the Temperature
b)
Pump in more gas
c)
Decrease the volume
d)
All of these
62.
In order to convert to Kelvin, you add ______ to the Celsius measurement.
a)
372
b)
273
c)
237
d)
732
63.
Charles' Law States...
a)
As Pressure goes up volume goes down
b)
As Pressure goes up temperature goes up
c)
As Volume goes up temperature goes up 
d)
As Pressure goes down volume goes down 
64.

Absolute zero is

a)

0 K

b)

where there is no molecular movement

c)

the coldest temperature possible

d)

all of these

65.
Whose law states that as pressure goes up, volume goes down?
a)
Charles 
b)
Boyle
c)
Aglow
d)
Mazias 
66.
A balloon will pop in the atmosphere because..
a)
Pressure goes down volume goes up
b)
Pressure goes up volume goes down
c)
temperature goes down volume goes up
d)
volume goes down temperature goes down
67.

What type of relationship is shown between these two variables

a)

A logarithmic relationship

b)

A direct relationship

c)

An indirect relationship

d)

There is no relationship

68.

If I initially have 4.0 L of a gas at a pressure of 1.1 atm, what will the volume be if I increase the pressure to 3.4 atm?

a)

1.29 L

b)

12.36 L

c)

1.29 atm

d)

12.36 atm

69.

A sample of nitrogen occupies a volume of 250 mL at 25oC. What volume will it occupy at 95oC?

a)

308.70 mL

b)

456.1 mL

c)

308.70oC

d)

456.1oC

70.

Oxygen gas is at a temperature of 40oC when it occupies a volume of 2.3 liters. To what temperature should it be raised to occupy a volume of 6.5 liters?

a)

611.84oC

b)

611.84 K

c)

880.33 K

d)

880.33oC

71.
Which equation represents Dalton's Law?
a)
e=mc2
b)
PV=nRT
c)
P1/T1=P2/T2
d)
Ptotal=P1, P2, P3...
72.
Three gases, Ar, N2 and H2 are mixed in a 500L container. Ar has a pressure of 255 torr, N2 has a pressure of 228torr and H2 has pressure of 752torr. What is the total pressure in the container?
a)
483torr
b)
270torr
c)
1235torr
73.
A mixture of hydrogen, nitrogen, and water vapor has a total pressure of 864 mmHg. The partial pressure of hydrogen is 220 mmHg and that of nitrogen is 410 mmHg. What is the partial pressure of water vapor?
a)
234 mmHg
b)
1.37 mmHg
c)
2.64 mmHg
d)
1, 494 mmHg
74.

What can be concluded about NH3, HCl, and SO3 based on their behavior when dissolved in water?

a)

They are solids

b)

They are covalent

c)

They are gases

d)

When heated, more of each can be dissolved in water.

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