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H Chem Molarity, solubility and stoic

Total questions: 44

Worksheet time: 6hrs 33mins

Name
Class
Date
1.

How do chemists describe the "strength" or concentration of a solution?

a)

molarity

b)

concentrated

c)

diluted

d)

strong

2.

How do chemists calculate molarity?

a)

grams/mole

b)

moles/Liter

c)

ounces/container

3.

What is the molarity of 0.50 moles of NaCl in 0.25 L of solution?

a)

1.0 M

b)

0.5 M

c)

2.0 M

d)

1.5 M

4.

Determine the molarity of 2.25 moles of sulfuric acid, H2SO4, dissolved in 725 mL of solution.

a)

322 M

b)

3.10 M

c)

0.325 M

d)

2.25 M

5.
How many moles of NaCl are present in a solution with a molarity of 8.59 M and a volume of 125 mL?
a)

10.74 mol

b)

0.0695 mol

c)

1.07 mol

d)

62.7 mol

6.
How many moles are needed to make 2.5 L of a 3.8 M solution? 
a)

9.5 mol

b)

0.66 mol

c)

1.5 mol

d)

15 mol

7.

If 20.0 mL of a 3.80 M solution is diluted to 50.0 mL, what is the ending molarity?

a)

1.52

b)

2.67

c)

2.95

d)

5.62

8.

If 50.0 mL of a 0.78 M solution is diluted to 90.0 mL, what is the ending molarity?

a)

.14

b)

.43

c)

14.2

d)

43.3

9.

If 30.0 mL of a solution that has a 1.82 M is diluted to 1.14 M, what is the VOLUME of my ending solution?

a)

.07mL

b)

19mL

c)

47.9mL

d)

63.8mL

10.

What is the molarity of 4.00 grams of KNO3 in 3.80 L of solution?

a)

0.0104 M

b)

0.0207 M

c)

1.05 M

d)

1.08 M

11.

Calculate the molarity of the following solution:  400.0 g of CuSO4 (molar mass = 159.60 g/mol) in 4.00 L solution.

a)

100. M

b)

251 M

c)

0.627 M

d)

1.60 M

12.
What is the volume (in liters) of a 0.20 M solution that contains 0.30 moles of Na2SO4 dissolved in it?
a)

1.5 L

b)

0.060 L

c)

0.67 L

d)

2.3 L

13.
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

14.

What are [C] and [D]?

a)

concentration of reactants

b)

concentration of products

c)

energy of reactants

d)

energy of products

15.
What is the equilibrium-constant expression for 
CO2(g) + H2(g) ↔ CO(g) + H2O(l)
a)
Kc= [CO][H2O] / [CO2][H2]  
b)
Kc= [CO2][H2] / [CO]
c)
Kc= [CO2][H2] / [CO][H2O]
d)
Kc= [CO] / [CO2][H2]  
16.

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 [CH4]4

17.
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
18.
What are [A] and [B]?
a)
concentration of reactants
b)
concentration of products
c)
energy of reactants
d)
energy of products
19.

What is the reaction/equation for this Kc expression

a)

2N2 + O2 ⇌ 2NO

b)

N2 + O2 ⇌ NO

c)

NO ⇌ 2NO

d)

N2 + O2 ⇌ 2NO

20.

70 grams of CaCl2 dissolved in 100 grams of water at 30°C would make what type of solution?

a)

unsaturated

b)

saturated

c)

supersaturated

21.

30 grams of KCl dissolved in 100 grams of water at 10°C would make what type of solution?

a)

unsaturated

b)

saturated

c)

supersaturated

22.

20 grams of K2Cr2O7 dissolved in 100 grams of water at 20°C would make what type of solution?

a)

Unsaturated

b)

Supersaturated

c)

Saturated

d)

Undefined

23.

What type of a solution is 60g NaNO3 at 40ºC in 100g H2O?

a)

Saturated

b)

Unsaturated

c)

Supersaturated

24.

What type of a solution is 100g KNO3 at 40ºC in 100g H2O?

a)

Saturated

b)

Unsaturated

c)

Supersaturated

25.

What type of a solution is 260g sugar at 50ºC in 100g H2O?

a)

Saturated

b)

Unsaturated

c)

Supersaturated

26.

How much KNO3 solute is saturated at 40 degrees?

a)

75

b)

55

c)

65

d)

85

27.

How much C12H22O11 solute is saturated at 40 degrees?

a)

240

b)

220

c)

230

d)

250

28.

How much Ce2(SO4)3 solute is saturated at 80 degrees?

a)

20

b)

15

c)

30

d)

2

29.

At what temperature can you fully dissolve 60g of KNO3?

a)

27

b)

30

c)

37

d)

You cannot determine this

30.

At which temperature do KBr and KNO3 have the same solubility?

a)

60°C

b)

55°C

c)

50°C

d)

Never

31.

What is the maximum temperature where at least 60 g of HCl can dissolve?

a)

35 ⁰C

b)

45 ⁰C

c)

55 ⁰C

d)

65 ⁰C

32.

Which solute is MOST likely a gas?

a)

KNO3

b)

NaNO3

c)

KCl

d)

Ce2(SO4)3

33.
For the Balanced Reaction: 3 Mg + 1 Fe2O3 → 3 MgO + 2 Fe; What is the Ratio of moles of Mg to moles Fe?
a)
3mol Mg / 2 mol Fe
b)
2 mol Mg/ 3 mol Fe
c)
1 mol Fe/ 2 mol Fe
d)
3 mol MgO / 2 mol Fe
34.
2 KClO3 → 2 KCl + 3 O2
How many moles of oxygen are produced when 6.7 moles of KClO3 decompose completely?
a)
6.7 mol
b)
1.0 mol
c)
10.1 mol
d)
4.5 mol
35.
2Na + 2H2O → 2NaOH+ H2
How many grams of hydrogen are produced if 120 g of Na are available?
a)
5.2 g
b)
2.6 g
c)
690 g
d)
45 g
36.
CH4 + 2 O2 → CO2 + 2 H2O
How many moles of carbon dioxide are produced from the combustion of 110 g of CH4?
a)
13.7 mol
b)
2.75 mol
c)
6.11 mol
d)
6.85 mol
37.
Mole ratios are obtained from the
a)
balanced chemical equation
b)
periodic table
c)
molar mass
38.

How many moles of water could form from 5.00 moles of hydrogen?

a)

5.00 moles

b)

10.00 moles

c)

2.50 moles

d)

No Reaction

39.

What numbers in a balanced equation do we use to determine mole ratios?

a)

Subscripts

b)

Superscripts

c)

Coefficients

40.
Balance this reaction: ____ RbNO3 + ____ BeF2 ----> ____ Be(NO3)2 + ____ RbF
a)
1,1,1,1
b)
1,2,1,1
c)
2,1,1,2
d)
2,1,2,1
41.
Using the following equation:
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from  6 moles H2? 
a)
4 moles Fe
b)
6 moles Fe
c)
9 moles Fe
d)
2 moles Fe
42.
What is the molar mass of (NH4)2CO3 ?
a)
144 g
b)
138 g
c)
96 g
d)
78 g
43.

Mg(s) + 2 HCl(aq) → MgCl₂(aq) + H₂(g)

How many moles of HCl are consumed in the production of 7.5 moles of MgCl₂?

a)

3.8 moles

b)

15 moles

c)

7.5 moles

d)

23 moles

44.
2Na + 2H2O → 2NaOH+ H2
How many grams of hydrogen are produced if 120 g of Na are available?
a)
5.2 g
b)
2.6 g
c)
690 g
d)
45 g

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