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Analytical Chemistry Midterm

Total questions: 85

Worksheet time: 1hrs 27mins

Name
Class
Date
1.

Molality (m) = moles of solute / _________________________.

a)

kilogram of solvent

b)

kiloliter of solvent

c)

kilometer of solvent

d)

ounces of solvent

2.

Given the following:

Na = 22.98 g/mol

C = 12.01 g/mol

H = 1.01 g/mol

O = 16 g/mol

identify the molar mass of Na2CO3

a)

105.97 grams/mol

b)

52.99 grams/mol

c)

100.45 grams/mol

d)

54 grams/nol

3.

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)

2.5 moles /kg solvent

4.
True or False? The higher the concentration of a solution the less solutes it has in it.
a)
True
b)
False
5.

Molarity is measured in _____.

a)

moles per g.

b)

mols per L.

c)

moles per mm.

d)

moles per mL.

6.

Given the following:

P = 30.97

N = 14.01

H = 1.01 g/mol

O = 16 g/mol

What is the mass of 0.75 moles of (NH4)3PO4?

a)

61.98 g

b)
121.75 g
c)

149.12 g

d)
131.75 g
7.
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
8.

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

9.

Which equation is used to find molarity?

a)

Moles solute/L solution

b)

Moles solute/kg solution

c)

Moles solute/kg solvent

d)

Grams solute/L solution

10.

Which equation is used to find molality?

a)

Moles solute/L solution

b)

Moles solute/kg solution

c)

Moles solute/kg solvent

d)

Grams solute/L solution

11.

What is the molality of a solution in which 3.0 moles of NaCl is dissolved in 1.5 Kg of water?

a)

2.0 M

b)

0.22 m

c)

135 m

d)

2.0m

12.

What is the molarity of 4 grams of sodium chloride in 3,800 mL of solution?

Molar mass of sodium is 22.98 and chloride 35.453.

a)
0.018 M
b)
0.018 mol
c)
1.052 M
d)
1.052 mol
13.
Total number of mol fraction for all component in the solution is equal to
a)
1.0
b)
0.95
c)
0.50
d)
2.0
14.

When KCl (potassium chloride) is dissolved in water, how many particles are in solution?

a)

1

b)

2

c)

3

d)

4

15.

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

a)

1

b)

2

c)

3

d)

4

16.
Colligative properties depend on the _____ of solute particles in solution.
a)
type
b)
number
c)
pH
d)
nature
17.
The freezing point of a solution is ____ the freezing point of the pure solvent.
a)
the same as
b)
lower than
c)
higher than
d)
no relation to
18.
The boiling point of a solution is ______ the boiling point of the pure solvent.
a)
higher than
b)
the same as
c)
lower than
d)
higher or lower than
19.

TRUE or FALSE: On the pH scale, 7 is the neutral value.

a)

True

b)

False

20.

TRUE or FALSE: Molarity is defined as the ratio of the number of moles of solute to the volume of solutions in liters.

a)

False

b)

True

21.

TRUE or FALSE: The solution is a type of mixture that contains more than one phase.

a)

True

b)

False

22.

TRUE or FALSE: There is a concept of “like dissolves like”. Polar Solutes dissolve in Polar Solvents. Nonpolar Solute dissolves in Nonpolar Solvents.

a)

True

b)

False

23.
What is the concentration, in percent by mass, of 0.62 g of solute in 45.0 g of solution?
a)
0.014 %
b)
1.4 %
c)
0.13%
24.
What is the concentration, in percent by volume, of 15.3 mL of solute in 2.65 L of solution?
a)
0.58%
b)
0.0058%
c)
5.8%
25.

What is the molality of a solution in which 3.0 moles of NaCl is dissolved in 1.5 Kg of water?

a)

2.0 M

b)

0.22 m

c)

135 m

d)

2.0m

26.

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

27.
Hydrogen bonding occurs when hydrogen is bonded to N, O, or F.  Which of the following has hydrogen bonding?
a)
CBr4
b)
NO2
c)
H2S
d)
NH3
28.
Does H2O have hydrogen bonding?
a)
yes
b)
no
29.

Intermolecular forces for: NH3

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

30.
What word describes when water is attracted to other substances?
a)
cohesion
b)
adhesion
c)
capillary action
d)
surface tension
31.

When water and other liquids stick together to form drops or thin films called ________________.

a)

adhesion

b)

capillary action

c)

cohesion

d)

surface tension

32.
molecule in which opposite ends have opposite electric charges
a)
cohesion
b)
polar molecule
c)
hydrogen bond
d)
solution
33.
Which term refers to water having partial positive and a partial negative charge?
a)
cohesion
b)
surface tension
c)
polarity
d)
adhesion
34.

Capillary Action

a)

The property of water that allows ice to float on the surface of liquid water

b)

The property of water that allows it to dissolve polar substances

c)

When water molecules stick to other surfaces

d)

The property of water that allows water to move up a thin tube (or the stem of a plant) by itself

35.
What is viscosity?
a)
A liquid's resistance to flow.
b)
a liquids flow.
c)
a liquid
d)
gas to solid.
36.

High viscosity is when particles are closer together and the cohesive force is stronger.

a)

True

b)

False

c)

I don't know

37.

The temperature at which its vapor pressure equals atmospheric pressure.

a)

specific heat

b)

vapor pressure

c)

molar heat of fusion

d)

boiling point

38.

Which of the following has the strongest IMF?

a)

dipole-induced dipole

b)

dipole-dipole

c)

ion-dipole

d)

London Dispersion

39.

A force that exist between polar and non-polar molecule.

a)

ion dipole

b)

hydrogen bonding

c)

London dispersion

d)

dipole-induced dipole

40.

In ion-dipole forces the cation forms an attractive force with the negative end of the molecule.

a)

true

b)

false

41.

The weaker the intermolecular forces of a substance the _____________ the boiling point

a)

higher

b)

lower

42.

45.13 g of sodium chloride is added to 0.318 kg of water. Determine the boiling point elevation.

Constant:

Molar mass of sodium chloride = 58.44 g/mol

Kb = molal boiling point elevation water = 0.512 °C kg/mol

van't Hoff factor of NaCl = 2

Given:

Solute = 45.13 g

Solvent =0.318 kg

NOTE: write numerical answer only (2 decimal places only.), do not indicate the unit of measurement anymore! 

(a)  

43.

What is the equation of boiling point elevation when solute is non-electrolyte?

a)

△T = Kbm

b)

△T = iKbm

c)

△T = iKfm

d)

△T = Kfm

44.

What happens to the solution when solute is added?

a)

freezing point will be elevated

b)

boiling point will be lowered

c)

vapor pressure will be lowered

d)

all of the above

45.

The equation called Raoult's Law would look like this

a)

Posolvent = Xsolvent Psolvent

b)

Psolvent = Posolvent + Xsolvent

c)

Psolvent = Xsolvent Posolvent

d)

Posolvent = Xsolvent + Psolvent

46.

Which of the following is NOT correct?

a)

boiling point of solution will rise when solute is removed

b)

freezing point of solution will be lowered when solute is added

c)

vapor pressure of solute and solvent depends on the number of solute in the solution.

d)

all are correct

47.

Determine the boiling point elevation if 56.03 g of Calcium Chloride is added to 436g of chloroform.

molar mass of CaCl2 = 110.98 g/mol

Kb of chloroform = 3.80 oC kg/mol

van't Hoff factor = 3

NOTE: write numerical answer only (2 decimal places only.), do not indicate the unit of measurement anymore! 

(a)  

48.

71.05 g of sucrose is added to 0.850 kg of water. Determine the freezing point depression. (answer should be in 3 decimal places)

molar mass of sucrose = 342.3 g/mol

Kf of water = -1.86oC kg/mol

van't Hoff factor of sucrose

NOTE: write numerical answer only (2 decimal places only.), do not indicate the unit of measurement anymore! 

(a)  

49.

Calculate the vapor pressure of solution made by dissolving 67.37 g of glucose, in 8.24g of water. The vapor pressure of pure water at 37oC is 47.1 torr.

molar mass of glucose = 180.156 g/mol

molar mass of water = 18.015 g/mol

NOTE: write numerical answer only (3 DECIMAL PLACES), do not indicate the unit of measurement anymore! 

(a)  

50.

The substance that gets dissolved in a solution is generally called_______.

a)

electrolyte

b)

nonelectrolyte

c)

solute

d)

solvent

51.
For the reaction...
SO2 + O2  <−>  SO3
If the concentration of SO2 is increased, the equilibrium of the reaction will shift ___________.
a)
left
b)
right
c)
left and right 
d)
neither left nor right
52.
What is the Kc expression for this reaction?
   2 NO(g)  +  O2(g) ⇌  2 NO2(g)
a)
Kc = [NO2]2 / [NO]2 [O2]
b)
Kc =  [NO]2 [O2] / [NO2]2
c)
Kc = [NO]2 [O2] [NO2]2
d)
Kc = [NO2]2 / [NO]2 +  [O2]
53.
What are [A] and [B]?
a)
concentration of reactants
b)
concentration of products
c)
energy of reactants
d)
energy of products
54.
The following reaction :    
SO2 (g) +  NO2 (g) <=> SO3 (g) + NO (g)  
had reached a state of equilibrium, was found to contain  
0.40 mol L-1 SO3 , and 0.30 mol L-1 NO,
0.15 mol L-1NO2 , and 0.20 mol L-1 SO2.
Calculate the equilibrium constant  for this reaction. 
a)
4
b)
.42
c)
.25
d)
1
55.
N2O4(g) ↔ 2 NO2(g)
What is the concentration equilibrium constant expression?
a)
Kc = [NO2]2/[N2O4]
b)
Kc = [N2O4]/[NO2]2
c)
Kc = [N2O4]2/[NO2]
d)
Kc = [NO2]/[N2O4]2
56.
Consider the following reaction. What would be the equilibrium constant expression?
4Br2(g) + CH4(g) ↔  4HBr(g) + CBr4(g)
a)
[Br2]4  [CH4]/ [HBr]4  [CBr4]
b)
[HBr]4 [CBr4]/ [Br2]4 [CH4]
c)
[HBr ]/ [Br2]4 [CH4]
d)
[HBr]4 [CBr4]/ [Br2]4 [CH]4
57.

Kc = ?

a)

products / reactants

b)

reactants /products

58.
For the equilibrium
2SO3(g) ↔ 2SO2(g) + O2(g)
Kc = 4.08x10-3 at 1000K
What is Kp?
a)
3.45 x 105
b)
2.99
c)
0.335
d)
3.4 x 10-5
59.

At the start of a reaction, there are 0.490 mol N2, 5.861X10-2 mol H2, and 9.84X10-4 mol NH3 in a 6.00L reaction vessel at 386 °C. If the equilibrium constant (Kc) for the reaction

N2(g) + 3H2(g) ⇌ 2NH3 (g)

Is 1.2 at this temperature. Predict which way the net reaction will proceed.

a)

left to right

b)

right to left

c)

no movement

60.

Which of the following doesn't affect chemical equilbrium

a)

temperature

b)

volume

c)

mass

d)

concentration

61.

According to _______ acids are compound that increases concentration of H+.

a)

Svante Arrhenius

b)

Bronsted- Lowry

c)

Gilbert Lewis

62.

According to Lewis Bases are __________.

a)

molecule that donates an electron pair to form a covalent bond

b)

molecule that accepts an protons

c)

molecule that donates cations to ionic compounds

d)

none of the above

63.

What is the conjugate acid in this example?

H2O   +      H2SO4      ⟶\longrightarrow        HSO4- +     H3O+

a)

H2O

b)

H2SO4

c)

HSO4

d)

H3O

64.

Which of the following indicates basic aqueous solution

a)

[H+] > [OH-]

b)

[H+] < [OH-]

c)

[H+] = [OH-]

65.

Determine wether the solution that contains 0.50 M OH is acidic, basic or neutral

a)

acidic

b)

basic

c)

neutral

66.

Which of the following is mismatched?

a)

acidic : blue litmus paper - turns red

b)

neutral : blue litmus paper - remains blue

c)

neutral : red litmus paper - turns blue

d)

basic : red litmus paper - turns blue

67.
A(n) ______ is a substance with a pH less than 7
a)
Acid
b)
Alkaline
c)
Base
d)
Buffer
68.
On the pH scale higher numbers indicate
a)
acids
b)
bases
69.
A solution has a pH of 7.0.  What would happen to the pH if H ions were added?
a)
pH would go up
b)
pH would go down
c)
pH would stay the same
d)
None of these
70.
Feels slippery.
a)
Acids
b)
Bases
c)
All
71.

Substances like dark chocolate that have a bitter taste, usually indicates that it would be classified as a

a)

Acids

b)

Bases

c)

Salts

d)

All

72.

What does pH measure?

a)

the amount of hydrogen (H+) ions

b)

the amount of hydroxide (OH-) ions

c)

amount of water

d)

all of the above

73.
A solution with a pH of 3.6 would be...
a)
Acid
b)
Base
c)
Neutral
d)
Acid and Base
74.

What is the pH of a solution that has a [H+] of 2.5 x 10-5?

4.605.02.57

a)

4.6

b)

5.0

c)

2.5

d)

7.0

75.

What is the [OH-] if the [H+] is 1.0 x 10-3 M?

a)

1.0 x 10-3 M

b)

6.02 x 10-23 M

c)

1.0 x 10-14 M

d)

1.0 x 10-11 M

76.

CO32-(aq) + H2O(l) → HCO3-(aq)+OH-(aq)

Using the above reaction, which compound is the conjugate base?

a)

CO32-

b)

H2O

c)

HCO3-

d)

OH-

77.

An Arrhenius acid:

a)

donates H+ to another substance

b)

accepts H+ from another substance

c)

produces H+

d)

produces OH-

78.

A Bronsted Lowry base:

a)

donates H+ to another substance

b)

accepts H+ from another substance

c)

produces H+

d)

produces OH-

79.

For a solution, pH + pOH =

a)

7

b)

14

c)

1.0 x 10-14

d)

-log (1.0 x 10 -14)

80.

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

a)

10.44

b)

1.00

c)

3.57

d)

-4.43

81.
Acidic buffer is made up of
a)
weak acid and weak base
b)
weak acid and its conjugate salt
c)
weak acid and its conjugate base
d)
strong acid and its conjugate base
82.

Which of the following statements ARE TRUE about buffer solution?


(you may choose more than one answer)

a)

pH of buffer solution will never change despite addition of small amount of base or acid

b)

Buffer can be made by mixing weak acid and salt of its conjugate base or by mixing weak base with salt of its conjugate acid

c)

Buffer has acid and base components that can work specifically to resist pH change

d)

the closer the ratio of concentration weak acid/base to the concentration of salt of its conjugate base/acid, the less effective the buffer to resist pH change

83.

a buffer solution is made by mixing HA, a weak acid, with salts containing A- ions.


HA ↔ H+ + A-


a formula that can be used for the calculation of the pH of this buffer solution is

a)
b)
c)
d)
84.
Pure water has a pH of 7. Pure water _______.
a)
is a base
b)
is a neutral substance
c)
could be either an acid or a base
d)
is an acid
85.
Which is the stronger acid?
a)
pH 1
b)
pH 4
c)
pH 8
d)
pH 13

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