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Acid/Base Test Review Flashcards | StudBud
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Acid/Base Test Review
Acid/Base Test Review
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Review of basic solution chemistry: molarity, dilution, pH, and strong and weak acids/bases.
Flashcards
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Answers
1
You have 432 m L of a 1.85 M NaOH solution and dilute it to a volume of 900 mL, what is M
f
?
1.64 M
0.88 M
719820 M
1.85 M
2
Which of the following is a strong base:
HOH
KCl
Ba(OH)2
NH3
3
What is the molar mass of H
2
SO
3
and the name of the compound?
Hyposulfurous Acid: 50 g/mol
Sulfurous Acid: 82 g/mol
Hydrosulfuric Acid: 98 g/mol
Sulfuric Acid: 82g/mol
4
Which of the following formulas is not correctly paired with its name?
H2SO4: Sulfuric Acid
HClO4--Perchloric Acid
H2NO3--Nitrous Acid
HClO3: Chloric Acid
5
What part of the molarity equation cannot be changed when diluting a solution?
Number of moles
Molarity
Volume
Concentration
6
You have 75 mL of 0.5 M KOH and use it to neutralize 43 mL of HCl, what is the molarity of HCl?
Cannot be determined from the information given.
1.69 M HCl
1.15 M HCl
0.88 M HCl
7
You have 25.2 mL of H
3
PO
4
and it is neutralized by 100 ml of 7.3 M Ca(OH)
2
, what is M
A
?
75.6M
108,562 M
9.65M
19.3 M
8
Which of the following is NOT a polyprotic acid?
Ca(OH)2
H2SO4
H2CO3
H3PO4
9
Which of the following is
not
an acid/base theory?
Aristotelian
Bronsted-Lowry
Arrehenius
Lewis
10
Given 12.3 mol of HBr and 4.8 L of liquid, what is the molarity of the solution?
59.04 M
2.56 M
0.39 M
0.032 M
11
The difference between a polyprotic acid and a monoprotic acid is:
The number of OH- (hydroxide) ions in an acid.
The way that one must neutralize the acid.
The number of H+ (hydronium) ions in an acid.
The number of pH degrees lost during titration.
12
What happens to the molarity of a solution when its volume is decreased?
It decreases.
It increases.
It remains the same.
It forms a precipitate.
13
When a compound is acting as an electron donor, it is acting as a:
Lewis Base
Bronsted Lowry Base
Lewis Acid
Bronsted Lowry Acid
14
Given the following Hydronium concentration 1 x 10
-4
, what is the substance?
A base with a pH of .0000001
A base with a pH of 10
An acid with a pH of .00004
An acid with a pH of 4
15
If you add 50 mL of water to 100 mL of a 0.15 M NaOH solution, what will the final molarity be?
0.1 M
0.18 M
0.75 M
0.25 M
16
Select the correct statement about H
2
SO
4
:
It is a strong acid named sulfurous acid.
It is a strong acid named sulfuric acid.
It is a weak acid named hydrosulfuric acid.
It is a weak acid named sulfurous acid.
17
Given the following hydronium ion concentration: 1 x 10
-13
, what is the substance?
An acid with a pH of 0.00000000000013
An acid with a pH of 1.
A base with a pH of 0.0000000000013
A base with a pH of 13.
18
A solution can be diluted by:
By doing all of these.
By changing the number of moles in the solution.
By altering its pH
By altering its volume
19
What mass of magnesium chloride is needed to produce a 3M solution in 782 mL?
0.79 g
74.1g
120.2g
1.27g
20
Molarity compares:
number of moles of solvent per liter of solute
concentration to pH level.
number of moles of solute per liter of solven
hydronium ion ratio to the hydroxide ion concentration
21
When a compound is a proton donor, it is acting as a:
Bronsted Lowry Acid
Lewis Base
Lewis Acid
Bronsted Lowry Base
22
What is the number of moles required to produce a 12M HCl solution in 634 mL of water?
18.9 mol
7609 mol
0.019 mol
7.6 mol
23
Which of the following best describes the process of titration?
When you see the base turn pink and the acid remains clear.
Using an indicator to identify a base or an acid.
Using an indicator to find where H+ ions equal OH- ions
To finding unequivalence where acids and bases are equal.
24
What difference is there between strong acids and strong bases?
Acids combine with water and bases dissociate in water.
Strong acids and bases DO NOT fully ionize in solution.
Acids ionize H+ ions and bases OH- ions
Acids ionize OH- ions and bases H+ ions.
25
Which part of a solution is present in the smallest amount?
Solution
Solute
Precipitate
Solvent
