Worksheets2nd 5th review
Total questions: 40
Worksheet time: 1hrs 2mins
Name
Class
Date
1.
Which relationship between ion concentrations always exists in an aqueous solution that is basic? [H+] equals zero.[H+] equals [OH–].[H+] is less than [OH–].[H+] is greater than [OH–].
a)
[H+] equals zero.[
b)
[H+] equals [OH–
c)
[H+] is less than [OH–]
d)
.[H+] is greater than [OH–].
2.
The table below contains data for water samples from four sources. Analyziz ot Water Samplez Source ot Water Sample Volume (mL) pH Rain 5 5.7 Creek 20 7.9 Pool 10 7.4 Faucet 20 6.8 Nancy analyzed water samples from several sources: rainfall, a nearby creek, a swimming pool, and her kitchen faucet. She recorded her data in the table. Which sample was most acidic?
a)
Rain
b)
Creek
c)
Pool
d)
Faucet
3.
The pH of a 0.10 M CH3COOH solution is
a)
less than 1
b)
greater than 1 but less than 7
c)
equal to 7
d)
greater than 7 but less than 14
4.
The table below shows pH values of some foods. A patient has chronic indigestion due to an overproduction of stomach acid. Which foods should the patient avoid until the condition is resolved?
a)
Vegetables
b)
Citrus
c)
dairy/egg
d)
Starches
5.
This is a pH chart of common materials. Which substance is the most basic?
a)
Cola
b)
Cheese
c)
Baking soda
d)
Bleach
6.
The table below shows the pH and reaction to litmus of four body fluids. These data indicate that gastric juice is very
a)
Acidic
b)
Very basic
c)
Positively charged
d)
Negatively charged
7.
The diagrams below show a 0.1 M aqueous solution of HCl and a 0.1 M aqueous solution of HF.
a)
HF has less H+ ions in solution making 0.1M HF more acidic than HCl
b)
HCl has more H+ ions in solution making 0.1M HCl more acidic than HF
c)
The pH of 0.1M HCl should be higher than HF because there are more Cl– ions the solution
d)
The pH of 0.1 M HCl should not be lower than 0.1 M HF due to the number of HF particles in the solution
8.
Angie is testing whether ammonia and vinegar are acids or bases. Litmus paper helps determine whether a chemical is an acid or a base. A drop of ammonia turns the litmus paper blue, and a drop of vinegar turns the litmus paper red. .
a)
Both of the chemicals are acids.
b)
Both of the chemicals are bases.
c)
Ammonia is an acid, and vinegar is a base
d)
Ammonia is a base, and vinegar is an acid
9.
Given the balanced equation representing a reaction: NH3(g) + H2O(A) ‹ NH4+(aq) + OH–(aq) According to one acid-base theory, the NH3(g) molecules act as
a)
an acid because they accept H+ ions
b)
an acid because they donate H+
c)
a base because they accept H+
d)
a base because they donate H+ ions
10.
A solution has a hydroxide ion concentration of 2.8 x 10–5M. What is the hydrogen ion concentration of the solution? A. 4.60 x 10–9M B. 3.57 x 10 –10M C. 3.98 x 10–6M D. 2.8 x 10–5M
a)
4.60 x 10-9M
b)
3.57 x 10-10M
c)
3.98 x 10-6M
d)
2.8 x 10-5M
11.
A beaker containing 80 grams of lead(II) nitrate, Pb(NO3)2, in 100 grams of water has a temperature of 30 ºC. Approximately how many grams of the salt are undissolved, on the bottom of the beaker?
a)
20 grams
b)
80 grams
c)
66 grams
d)
14 grams
12.
Which salt is LEAST soluble at 0 ºC?
a)
K2Cr2O7
b)
KNO3
c)
KClO3
d)
Ce2(SO4)3
13.
How many grams of sodium nitrate, NaNO3, are soluble in 100 g of water at 10 ºC?
a)
80 grams
b)
100 grams
c)
40 grams
d)
10 grams
14.
When 50 grams of potassium chloride, KCl, is dissolved in 100 grams of water at 50 ºC, the solution can be correctly described as:
a)
supersaturated
b)
unsaturated
c)
saturated
15.
At approximately what temperature does the solubility of sodium chloride, NaCl, match the solubility of potassium dichromate, K2Cr2O7?
a)
60 ºC
b)
30 ºC
c)
50 ºC
d)
83 ºC
16.
What is the precipitate formed when you mix silver nitrate with copper chloride?
a)
copper nitrate
b)
copper chloride
c)
silver chloride
d)
silver nitrate
17.
When no more sugar will dissolve in a glass of water, the solution is
a)
unsaturated
b)
saturated
c)
supersaturated
d)
suspended
18.
A _______ solution contains more solute than would normally dissolve at a certain temperature.
a)
unsaturated
b)
suspended
c)
saturated
d)
supersaturated
19.
You and your friend have a contest to see who can make iced tea the fastest. Which of the following would NOT help you win?
a)
Cooling the water
b)
Using smaller crystals
c)
Heating the water
d)
Stirring quickly
20.
What is Solubility?
a)
What is dissolved
b)
What does the dissolving
c)
A measure of how much solute can dissolve in solvent
d)
a charged ion
21.
What is the precipitate formed when you mix silver nitrate with copper chloride?
a)
copper nitrate
b)
copper chloride
c)
silver chloride
d)
silver nitrate
22.
Which of these lists contains only soluble substances?
a)
sodium nitrate, potassium chloride, calcium carbonate
b)
lead nitrate, lead chloride, lead sulfate
c)
calcium nitrate, copper chloride, ammonium phosphate
d)
silver nitrate, barium sulfate, copper carbonate
23.
In a beaker of concentrated sugar water, pure water is a...
a)
...solute.
b)
...solvent.
c)
...solution.
d)
...supsension.
24.
What is one way to increase the solubility of sugar in water?
a)
Heat the water.
b)
Chill the water.
c)
Increase the amount of sugar.
d)
Decrease the amount of water.
25.
The pH scale measures...
a)
...the strength of an acid.
b)
...the strength of hydrogen ions.
c)
...the concentration of hydrogen ions.
d)
...the concentration of an acid
26.
Reacts with metals to form H2.
a)
Acids
b)
Bases
c)
All
d)
Salts
27.
Tastes bitter.
a)
Acids
b)
Bases
c)
Salts
d)
All
28.
Electrolyte
a)
Acids
b)
Bases
c)
Salts
d)
All
29.
Feels slippery.
a)
Acids
b)
Bases
c)
All
30.
Which is most acidic?
a)
milk
b)
Lemon Juice
c)
bleach
31.
This image represents
a)
Neutralization reaction
b)
synthesis
c)
decompostion
d)
single displacement
32.
pH greater than 7.
a)
Acids
b)
Bases
c)
All
33.
The difference between a strong and weak acid is:
a)
Strong acids stay intact in water weak acids don't
b)
Strong acids are slippery weak acids aren't
c)
Strong acids break apart in water. Weak acids stay intact
d)
Weak acids break apart in water most of the time, strong acids do all of the time.
34.
What is the conjugate acid in the following equation?
a)
PO43-
b)
HNO3
c)
NO3-
d)
HPO42-
35.
What is the conjugate base of HCO3-?
a)
HCO3-
b)
H2CO3-
c)
H2CO3
d)
CO32-
36.
What is the pH of a solution that has an [H3O+] =1x10-4?
a)
4
b)
-4
c)
2
d)
3
37.
The pH of a solution is 2.0. What is the [OH-] concentration?
a)
1x10-12M
b)
12 M
c)
1x10-2M
d)
2 M
38.
The pH of a 0.001 M solution of HCl is
a)
11
b)
3
c)
-3
d)
-11
39.
Which is most acidic?
a)
pH = 8.5
b)
[H3O+] = 1 x 10-13
c)
[H3O+] = 1 x 10-2
d)
pH = 3
40.
What is the concentration of H3O+ ions in a 0.02M solution of HNO3?
a)
0.02
b)
0.04
c)
10-12
d)
3 x 0.002
100 %
