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7AE_Unit 3 Lesson 2 Quizizz (Part 2)

Total questions: 50

Worksheet time: 35mins

Name
Class
Date
1.

Khi hòa tan muối ăn vào trong nước thì khẳng định nào sau đây là đúng?

a)

Muối ăn là dung môi, nước là chất tan

b)

Nước là dung dịch

c)

Muối ăn là chất tan, nước là dụng môi

d)

Muối ăn là chất tan, nước muối là dung môi

2.

Trường hợp nào sau đây KHÔNG PHẢI là dung dịch?

a)

Cho thìa cát vào cốc nước và khuấy đều

b)

Cho thìa giấm vào cốc nước và khuấy đều

c)

Cho thìa muối ăn vào cốc nước và khuầy đều

d)

Cho 1 gam CuSO4 vào cốc nước và khuấy đều

3.

Dung dịch bão hòa là gì?

a)

là dung dịch hòa tan thêm được lượng nhỏ chất tan

b)

là dung dịch không thể hòa tan thêm chất tan

c)

là dung dịch chứa nhiều loại chất tan

4.

Dung dịch là hỗn hợp

a)

Chất rắn trong chất lỏng

b)

Chất khí trong chất lỏng

c)

Đồng nhất của chất rắn và dung môi

d)

Đồng nhất của chất tan và dung môi

5.

Cách nào không làm quá trình hòa tan đường vào nước diễn ra nhanh hơn

a)

Khuấy đều

b)

Nghiền mịn đường

c)

Thêm nước nóng

d)

Thêm chanh

6.

Câu nào sau đây đúng khi nói về sự điện li?

a)

Sự điện li là sự hoà tan một chất vào nước thành dung dịch.

b)

Sự điện li là sự phân li một chất dưới tác dụng của dòng điện.

c)

Sự điện li là sự phân li chất thành ion khi trong nước hay khi nóng chảy

d)

Sự điện li là quá trình oxi hoá - khử.

7.

Dung dịch chất điện li dẫn điện được là do

a)

Sự chuyển dịch của các electron

b)

Sự chuyển dịch của các cation

c)

Sự chuyển dịch của các phân tử hòa tan

d)

Sự chuyển dịch của cả cation và anion

8.

Chất nào sau đây không dẫn điện được?

a)

KCl rắn, khan

b)

CaCl2 nóng chảy

c)

NaOH nóng chảy

d)

HBr hòa tan trong nước

9.

Nước đóng vai trò gì trong quá trình điện li các chất trong nước?

a)

Môi trường điện li

b)

Dung môi không phân cực

c)

Tạo liên kết hidro với các chất tan.

d)

Dung môi phân cực

10.

Chất nào sau đây là chất điện li yếu

a)

HCl

b)

H2SO4

c)

HNO3

d)

CH3COOH

11.
What is a "homogeneous mixture of two or more substances in a single phase"?
a)
Solution
b)
Solvent
c)
Solute
d)
Compound
12.
What does it mean to be "Soluble" ?
a)
Capable of being a solid.
b)
To have soul.
c)
Capable of being dissolved.
d)
To sink.
13.
Which of the following are considered to be a homogeneous mixture?
a)
Colloid
b)
Solution
c)
Suspension
d)
All Mixtures
14.
What is the unit for molarity?
a)
mass/liters
b)
moles
c)
liters
d)
moles/liter
15.
A measure of the amount of solute in a given amount of solvent or solution is...
a)
saturated
b)
solubility
c)
concentration
d)
miscible
16.
A saturated solution is one that....
a)
contains the maximum amount of dissolved solute.
b)
contains less solute than a saturated solution.
c)
contains more solute than a saturated solution.
d)
is the amount of a substance required to form a saturated solution.
17.
An unsaturated solution is one that....
a)
contains the maximum amount of dissolved solute.
b)
contains less solute than a saturated solution.
c)
contains more solute than a saturated solution.
d)
is the amount of a substance required to form a saturated solution.
18.
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.
19.
A nonelectrolyte 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.
20.
The dissolving medium in a solution is called ... 
a)
colloid
b)
solution
c)
solute
d)
solvent
21.
The substance dissolved in a solution is called ... 
a)
colloid
b)
solution
c)
solute
d)
solvent
22.
What is the molarity of a 2 liter solution containing 5 moles of NaCl?
a)
2.5
b)
0.4
c)
2.5 moles/liter
d)
10 moles/liter
23.

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

a)

1

b)

2

c)

3

d)

4

e)

6

24.

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

a)

1

b)

2

c)

3

d)

4

e)

5

25.

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

a)

1

b)

3

c)

4

d)

5

e)

6

26.
Colligative properties depend on the _____ of solute particles in solution.
a)
type
b)
number
c)
pH
d)
nature
27.
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
28.
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
29.

Which of the following solutions will have the lowest freezing point?

a)

1.0 mol/L sucrose (C12H22O11)

b)

1.0 mol/L lithium chloride (LiCl)

c)

1.0 mol/L sodium phosphide (Na3P)

d)

1.0 mol/L magnesium fluoride (MgF2)

30.

Which of the following compounds will be most effective in melting the ice on the roads when the air temperature is below zero?


a)

sodium iodide (NaI)

b)

magnesium sulfate (MgSO4)

c)

potassium bromide (KBr)

d)

all will be equally effective

31.

Which sample, when dissolved in 1.0 liter of water, produces a solution with the lowest freezing point?

a)

0.1 mol of C2H5OH

b)

0.1 mol of LiBr

c)

0.2 mol of C6H12O6

d)

0.2 mol of CaCl2

32.

Compared to the freezing point and boiling point of water at 1 atmosphere, a solution of a salt and water at 1 atmosphere has a

a)

lower freezing point and a lower boiling point

b)

lower freezing point and a higher boiling point

c)

higher freezing point and a lower boiling point

d)

higher freezing point and a higher boiling point

33.
Colligative properties depend on the _________ of the solute but not the __________ of the solute.
a)
 concentration; identity
b)
identity; concentration
c)
reactivity; nature
d)
nature; reactivity
34.

While making homemade ice cream, you add rock salt to the ice. Which choice below provides the best explanation for why this is done?

a)

Adding salt to the ice will lower the freezing point by creating a solution that's freezing point is lower than just the ice.

b)

Adding salt to the ice will lower the freezing point by creating a solution that's freezing point is higher than just the ice.

c)

Adding salt to the ice will raise the freezing point by creating a solution that's freezing point is lower than just the ice.

d)

Adding salt to the ice will raise the freezing point by creating a solution that's freezing point is higher than just the ice.

35.

In the image, which best describes the solvent

a)

The salt

b)

Sodium Chloride

c)

The water

d)

The Chorine

36.

The separation of ions that occurs when an ionic compound dissolves is

a)

ionization

b)

dissociation

c)

electronegativity

d)

spectation

37.

How many moles of ions are produced when 1 mol of magnesium chlorate are dissolved in water?

a)

1 moles of ions

b)

2 moles of ions

c)

3 moles of ions

d)

4 moles of ions

38.

____________ is the process where particles of a solvent completely surround the particles of a solute.

a)

solvation

b)

immisciblation

c)

dissolution

d)

saturation

39.

Which of these would be most likely to decrease the rate of solvation?

a)

stirring or shaking

b)

breaking the solute into smaller pieces

c)

lowering the temperature

d)

increasing the temperature

40.

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

41.
Which of the following is LEAST likely to dissolve in water?
a)
nonpolar fats and oils
b)
polar sugar molecules
c)
salt made of a positive sodium ion and a negative chloride ion
d)
all of the substances will dissolve easily in water
42.

In general, which types of compounds dissolve easily in water?

a)
Polar and Nonpolar
b)
Polar and Ionic
c)
Nonpolar and Ionic
d)
Covalent and Nonpolar
43.
A supersaturated solution is one that....
a)
contains the maximum amount of dissolved solute.
b)
contains less solute than a saturated solution.
c)
contains more solute than a saturated solution.
d)
is the amount of a substance required to form a saturated solution.
44.

The formula M1V1 = M2V2 is used when:

a)

dissolving a solute in a solvent

b)

diluting a solution

c)

reacting an acid with a base

d)

determining the pH of an acid

45.

How does a solution become supersaturated?

a)

Vigorous stirring to dissolve more solute than usual.

b)

Heat the solution to increase the solute then let it cool.

c)

Add more solvent to lower the concentration.

d)

Keep pouring solute in the solvent until it goes in.

46.

Why is salad not a solution?

a)

because it's an element

b)

because it's a compound

c)

because it's a heterogeneous mixture

d)

because it's a homogeneous mixture

47.

This is a mixture that will settle over time if you let it sit.

a)

Suspension

b)

Colloid

c)

Mix - Mix a lot

48.
According to Mr. Edmonds aqueous solutions are __________. 
a)
explosive 
b)
heterogeneous 
c)
squishy 
d)
transparent 
49.
What is it about the water molecule that makes it a great solvent?
a)
water demonstrates polarity; a partial charge on each side of the molecule
b)
due to its molecular formula
c)
it has a liner molecular shape
d)
due to it's non-polar molecular structure
50.
What is the correct formula to solve for the Molarity of a solution that has .4 moles of HCl in 9.5 L of solution?
a)
M = 9.5 L / .4 mol
b)
M1V1=M2V2
c)
M = .4 mol / 9.5 L
d)
none of the other choices

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