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molarity, dilution titration

Total questions: 65

Worksheet time: 3hrs 44mins

Name
Class
Date
1.

What is the molarity of a 0.5L sample of a solution that contains 60.0 g of sodium hydroxide (NaOH)

a)

0.8 M

b)

1.5M

c)

3.0M

d)

6.0M

2.

When calculating molality, Kg of the following are included in the calculation?

a)

solvent

b)

solute

c)

none of these

d)

solvent & solute

3.

To calculate molality you only need which of the following?

a)

scale

b)

flask

4.

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

5.

What is the molarity of a solution containing 4 moles of KCl in 2.5 L of solution?

a)

1.6 M

b)

0.63 M

c)

10 M

d)

2.6 M

6.

What volume is needed to make a 2.45 M solution of KCl using 0.50 mol of KCl?

a)

4.9 L

b)

0.20 L

c)

1.2 L

7.

How many moles of NaCl are needed to make 5.25 L of a 0.25 M solution?

a)

1.3 mol

b)

21 mol

c)

0.048 mol

8.

How many grams of KCl would be dissolved in 5.50 L of a 0.250 M solution of KCl? *molar mass of KCl = 74.55 g/mol*

a)

1.48 g

b)

103 g

c)

1640 g

d)

3.39 g

9.

What is the molarity of a solution made by adding 1.565 moles of PbNO3 to 0.5 L?

a)

300. M

b)

31.3 M

c)

3.13 M

d)

1.56 M

10.

Which solution is more diluted?

Solution 1:

1000 mL of water

60g of salt


Solution 2:

500 mL of water

60 g of salt

a)

Not enough information to tell

b)

Solution 1

c)

Solution 2

d)

They are equally diluted

11.
What is the molarity of 4 grams of sodium chloride in 3,800 mL of solution?
a)
0.018 M
b)
0.018 mol
c)
1.052 M
d)
1.052 mol
12.
What is the molarity of a solution which contains 22.41 grams of NaCl in 50.0 mL of solution?
a)
0.488 M
b)
7.67 mol
c)
7.67 M
d)
0.00767 M
13.
How many grams of solute are dissolved in 125.0 mL of 5.00 M NaCl (MM = 58.45)?
a)
0.625 g NaCl
b)
625 g NaCl
c)
36.5 g NaCl
d)
0.04 mol NaCl
14.
What is the molarity of 2.5 mol of NaOH in 12.0 L of solution?
a)
0.21 M
b)
30 M
c)
4.8 M
d)
20.8 M
15.
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
16.
The ___ is the thing being dissolved
a)
solute
b)
solvent
17.
True or false? Insoluble means that two substances can dissolve in one another.
a)
true
b)
false
18.
Which sweet tea would you expect to taste the sweetest?
a)
1M
b)
3M
c)
3.1M
d)
2.5M
19.
If you have 0.045 L of 0.465 M potassium bromide. How many moles of potassium bromide are present?
a)
20.9 mol
b)
0.021 mol
c)
0.02 mol
d)
0.0209 mol
20.
What is the molarity in 650. ml of solution containing 63 grams of sodium chloride?
a)
2.4 M
b)
0.86 M
c)
1.7 M
d)
0.54 M
21.

50 ml of a 1 M solution is diluted until the final volume is 80ml. How much water was added?

a)

50 ml

b)

1.3 ml

c)

30 ml

d)

130 ml

22.
What is the molarity of a solution made by diluting 26.5 mL of 6.00M HNO3 to a volume of 250 mL?
a)
15.9 M
b)
0.636 M
c)
0.642 M
d)
1.59 M
23.
What is the molarity of a solution made by adding 1.565 moles of PbNO3 to 500 mL?
a)
300. M
b)
31.3 M
c)
3.13 M
d)
1.56 M
24.

How many liters would you need to make a 1 M solution if you have 6 moles of Sodium Hydroxide?

a)

2

b)

3

c)

4

d)

6

25.

What is the molarity of 122.5 g of AlCl3 in 1.0 L of solution? (MM = 133 g/mol)

a)

1.225 M

b)

0.92 M

c)

0.1225 M

26.
How many moles of NaCl are present in a solution with a molarity of 8.59M and 125 mL of solution?
a)
1.07 gram
b)
62.7 mol
c)
1.07 mol
d)
62.7 grams
27.

How many grams of AgNO3 are needed to prepare 0.125M solution in 250 mL of water? (MM 169.87g/mol)

a)

.03g

b)

0.5g

c)

5.3g

d)

84.9g

28.

If I have 340 mL of a 0.5 M NaBr solution, what will the concentration be if I add 560 mL more water to it?

a)

.188 M

b)

3.78 M

c)

.389 M

d)

1.76 M

29.
How many mL of 10.8M HCl are required to make 100.0 mL of 3.00M acid?
a)
27.8 mL
b)
27.78 mL
c)
2.8 mL
d)
278 mL
30.

What mass of Iodine, (molar mass= 253.80 g/mol), must be used to prepare a .960m solution if 100.0g of ethanol, CH3CH2OH, is used? molality= moles of solutekg solventmolality=\ \frac{moles\ of\ solute}{kg\ solvent}  

a)

50.0 g

b)

96.0 g

c)

2.54 g

d)

24.4 g

31.

What is the molarity of a solution composed of 8.210 g of potassium chromate, (molar mass= 194.20g/mol), dissolved in enough water to make .500L of solution?

​
   Molarity= molesofsoluteL of solutionMolarity=\ \frac{molesofsolute}{L\ of\ solution}  

a)

.0423 M

b)

.0846 M

c)

16.4 M

d)

.172 M

32.
HCl + NaOH → 
a)
NaH + ClOH
b)
NaCl + H2
c)
NaCl + H2O
d)
NaCl + Cl2
33.
What is the endpoint of a titration
a)
Where the amount of acid and base are balanced according to the equation
b)
Where there is no base
c)
At the end
34.
I am titrating 1M HCl with 1M NaOH.  I have 25mL of HCl. How much NaOH will I need?
a)
2.5mL
b)
5mL
c)
25mL
d)
50mL
35.
I have 25mL of 1M HCl which neutralises 20mL of NaOH. What is the concentration of the NaOH?
a)
0.8 M
b)
1 M
c)
1.25 M
36.
A 50.0 mL sample of Ca(OH)2 is neutralized by 300.0 mL of HCl solution with a pH of 1.3. Calculate the molarity of the Ca(OH)2 solution.
a)
1.0 M
b)
0.50 M
c)
0.15 M 
d)
0.30 M
37.
How many moles of Ca(OH)2 are needed to neutralize three moles of HCl? 
a)
8
b)
1.5
c)
6
d)
3
38.

In a titration, the solution changes color at the

a)

end point

b)

equivalence point

39.

A titration can be used to determine the _______________ of a solution

a)

molarity

b)

density

c)

boiling point

d)

reactivity

40.

A 25.00 mL sample of HCl was titrated to the end point with 15.00 mL of 2.00 M NaOH. The following neutralization reaction occured: HCl  +  NaOH  →  NaCl  +  H2OHCl\ \ +\ \ NaOH\ \ \rightarrow\ \ NaCl\ \ +\ \ H_2O  
What is the molarity of the HCl? 

a)

0.650 M

b)

1.05 M

c)

1.20 M

d)

1.50 M

41.

A 10.00 mL sample of H2SO4 was neutralized by 13.5 mL of 1.00 M KOH by the following reaction: H2SO4 +  2KOH  →  K2SO4  +  2H2OH_2SO_4\ +\ \ 2KOH\ \ \rightarrow\ \ K_2SO_4\ \ +\ \ 2H_2O  
What is the molarity of H2SO4?

a)

0.675 M

b)

0.910 M

c)

1.05 M

d)

1.20 M

42.

A 5.00 mL sample of household ammonia was analyzed by titration with hydrochloric acid according to the following reaction:   HCl  +  NH3  →  NH4 +   +  Cl −HCl\ \ +\ \ NH_3\ \ \rightarrow\ \ NH_4^{\ +}\ \ \ +\ \ Cl^{\ -}  
This titration required 19.5 mL of 0.750 M HCl. What is the molarity of the ammonia sample? 

a)

1.97 M

b)

2.19 M

c)

2.44 M

d)

2.92 M

43.

What is the role of an indicator in a reaction?

a)

To help reactants react successfully.

b)

To bind to the analyte to form a products.

c)

To show when the reaction has reached or past the equivalence point.

d)

To provide a surface for the reaction to occur.

44.

What is an equivalence point?

a)

It is the point when enough analyte has been added.

b)

It is the point when the amount of added titrant is equal to the amount of analyte in the solution.

c)

It is the point when the volume of titrant is equivalent the volume of analyte.

d)

It is the point when the concentration of titrant added is equivalent to the volume of analyte.

45.

Equal moles of the indicated acids are dissolved in the amounts of water shown in the beakers below. In which solution will the percent ionization of the acid be the lowest?

a)

Beaker 1

b)

Beaker 2

c)

Beaker 3

d)

Beaker 4

46.

When should you stop a titration?

a)

When you have added equal volumes

b)

When the indicator changes colour

c)

When you run out of solution

d)

When the solution is no longer acidic

47.
Which of the following is NOT a strong base?
a)
Ca(OH)2
b)
KOH
c)
NH3
d)
Sr(OH)2
48.

Acid + Base ₋-->

a)

salt + hydrogen

b)

salt + carbon dioxide + water

c)

salt

d)

salt + water

49.
I have 25mL of 1M HCl which neutralizes 20mL of NaOH. What is the concentration of the NaOH?
a)
0.8 M
b)
1 M
c)
1.25 M
50.
If 100 mL of 0.1 M solution is diluted to 550 mL what is the concentration?
a)
0.02 M 
b)
0.04 M
c)
0.1 M
d)
0.003 M
51.

If it takes 50 mL of 0.5 M Ca(OH)2 to neutralize 125 mL of hydrochloric acid (HCl), what is the concentration of the acid?

a)

0.2 M

b)

5 M

c)

0.5 M

d)

0.4 M

52.

A titration can be used to determine the _______________ of a solution.

a)

Molarity

b)

Density

c)

Boiling point

d)

Reactivity

53.

What is the method used to determine the concentration of an unknown acid or base through a neutralization reaction based on a color change within a certain pH range called?

a)

Analyte

b)

Titrant

c)

Indicator

d)

Titration

54.
a)

a

b)

b

c)

c

d)

d

55.
a)

a

b)

b

c)

c

d)

d

56.
a)

a

b)

b

c)

c

d)

d

57.
a)

a

b)

b

c)

c

d)

d

58.

If I have 18 M H2SO4 and I want to make 500 mL of a 1 M H2SO4 solution, what do I do?

4 lines
59.

If there is 0.09 mol NaCl dissolved in 0.80 L of solution, what is the molarity?

(round the answer to two decimal places)

(a)  

60.

What would be the Molarity of a glass of salt water if 14 g of NaCl is dissolved to form a solution that has a volume of 500 mL? The molar mass of NaCl is 58.44 g/mol. Round to nearest hundredth.

(a)  

61.

What volume must 108 grams of NaCl be watered down to so that the molarity of the solution is 0.80 M? Round to nearest tenth.

(a)  

62.
When a Koolaid mix in water is dark in color and very sweet it is a __________ solution.
a)
concentrated 
b)
Diluted
63.
To prepare 1M of NaOH, you will need a mass of ______g NaOH
a)
23g
b)
40g
c)
4g
d)
39g
64.
Solutions are composed of __________ .
a)
salts and solutes
b)
solvents and salts
c)
solutes and alloys
d)
solutes and solvents
65.
What is the molarity of a solution made by diluting 26.5 mL of 6.00M HNO3 to a volume of 250. mL?
a)
15.9 M
b)
0.636 M
c)
0.642 M
d)
1.59 M

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