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DE_CH_5.3_Acids, Bases, and Salts

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Last updated over 2 years ago
41 questions
Background Knowledge
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3
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Acid-Base Theories (1)
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Precipitation Reactions (2)
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Acid-Base Strength (3-4)
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Acid-Base Reactions and Buffers (5-6)
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pH and pOH (7-8)
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Question 1
1.

What do I already know about acids, bases, and salts?

Question 2
2.

What are ways in which you use acids, bases and salts in your everyday life?

Question 3
3.
Chemists rely on chemical equations that help them analyze the different _______ involved in acid-base reactions. An important aspect of acid-base reactions is the extent to which the compounds _______. These processes are constantly occurring all around you and even within your body. People, as well as most other living things, cannot survive if their bodies become too _______ or too_______.
Question 4
4.
log(0.001) = _______
log 4 + log 3 = log _______
2 = log ________
Other Answer Choices:
100
-3
12
1
7
-1
-2
10
Question 5
5.

Match each acid formula with its name.

Draggable itemarrow_right_altCorresponding Item
HCl
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hydrocloric acid
HClO
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hypoclorous acid
HClO2
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chlorous acid
HClO3
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cloric acid
HClO4
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pechloric acid
Question 6
6.
The original theory of acids and bases was proposed by Svante August Arrhenius around 1884. An Arrhenius __________ is any substance that increases the number of hydrogen ions (H+) in an aqueous solution. An Arrhenius base is any substance that increases the number of __________ in an aqueous solution.
Question 7
7.

What will hydrochloric acid form when added to water?

Question 8
8.

What will sodium hydroxide form when added to water?

Question 9
9.
Not all acids and bases produce hydrogen or hydroxide ions in solutions. The _______ definition of acids and bases was created to solve this issue. It specifically describes the gain or loss of _______ (protons). A Brønsted-Lowry acid is any substance that can _______ a hydrogen ion (proton). Brønsted-Lowry base is any substance that can _______ a hydrogen ion (proton).
Question 10
10.

For the Brønsted-Lowry definition of acids and bases, a donated proton is

Question 11
11.
Gilbert Lewis proposed a different mechanism for acid-base theory, also around 1923. The Lewis theory is based on the _______. A Lewis acid is an electron pair _______. A Lewis base is an electron pair _______. _______ is both a Lewis acid and a Lewis base.
Question 12
12.


The common acids are all formed from a negative ion and a negative hydroxide ion.

Question 13
13.

What is a precipitation reaction?

Question 14
14.
A precipitation reaction can sometimes occur when two __________ are mixed together in an aqueous solution.
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Question 15
15.

These are guidelines that help you to identify insoluble compounds known as

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Question 16
16.
Use the solubility rules and the dropdown menus to indicate whether each compound is aqueous or solid.
Rb2S(__________) + CuI2(__________) -> 2RbI(__________) + CuS(__________)
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3
Question 18
18.

According to the Arrhenius definition of acids and bases, the strength of an acid or base is defined as

Question 19
19.

All acids dissociate, but only some will ionize.

Question 20
20.
Strong acids and bases dissociate _______ in water. Weak acids and bases dissociate _______ in water.
Question 21
21.

Categorize the following statements.

  • HA = H+ + A-
  • Forms a conjugate base
  • B = OH- + BH+
  • Kb
  • Ka
  • Forms a conjugate acid
  • Acid Reactions
  • Base Reactions
Question 22
22.

Which of these compounds is an amphoteric substance?

Question 23
23.

When a water molecule accepts a proton, hydronium is formed. Where does this extra proton come from?

Question 24
24.

Match the correct reaction type to the corresponding chemical equation.

Draggable itemarrow_right_altCorresponding Item
weak acid-strong base
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HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (aq)
weak acid-weak base
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HC2H3O2 (aq) + KOH (aq) → H2O (aq) + KC2H3O (aq)
strong acid-weak base
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HCl (aq) + NH3 (aq) ⇄ NH4Cl (aq)
strong acid-strong base
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NH3 (aq) +H2O (aq) ⇄ NH4+ (aq) + OH- (aq)
Questions 25 & 26 | 01:37
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Questions 25 & 26
01:37
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Question 26
26.

What is the name of the compound that is insoluble in the reaction shown in the video.

Question 27
27.

Consider the following left-hand side of a chemical reaction:

HClO4 + KOH →

Select the correct right hand side from the list below.

Question 28
28.
Complete the following chemical reaction when ammonia acts as a base.

NH3 + H20 → _______ + _______
Question 29
29.

How can chemists maintain a constant concentration of the pH of a solution?

Question 30
30.
Acidic buffer solutions are made from a _______ and one of its salts. This will allow the buffer solution to resist against a higher concentration of _______ being produced in the solution.

Conversely, acid or alkali buffer solutions are made from a _______* and one of its salts. This will allow the buffer solution to resist against a higher concentration of _______ being produced in the solution.

*The text is incorrect for this part.
Question 31
31.

During neutralization, an acid and a base will react to form what?

Question 32
32.

What is the equation for Neutralization?

Question 33
33.

What volume, in milliliters, of a 0.997 M KOH solution is needed to neutralize 30.0 mL of 0.400 M HCL?

Question 34
34.

A student pipets 10.0 mL 0.0500 M H3PO4 into a flask. What volume of 0.0200 M Mg(OH)2 could be added that will completely neutralize the acid?

Question 35
35.

An unknown volume of 0.200 M acetic acid (HC2H3O2) was completely neutralized by 22.0 mL 0.140 M ammonia (NH3) in water. What was the original volume of the acetic acid before neutralization?

Question 36
36.
The term pH is a mathematical way of comparing the strength of acids and bases. A difference of one on the scale will mean a difference in strength of 10.

That means, an acid with a pH of 2 will be _______ times stronger than an acid with a pH of 4
Question 37
37.
pH will describe the quantity of _______ ions in the solution. pOH will describe the quantity of _______ ions in the solution. The pH and pOH of the solution can be calculated from the other and will always total _______.
Question 38
38.

We can use the negative logarithm (pH = -log[molarity]) in order to find the pH of weak acids/bases.

Questions 39 & 40 | 01:07
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Questions 39 & 40
01:07
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Question 39
39.

The method used to determine the unknown concentration of an acid or base by analyzing neutralization during the reaction is known as

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Question 41
41.

Organize the following substances in decreasing order from highest pH to lowest pH.

  1. 5 g of distilled water
  2. Bleach with a pH of 12.6
  3. 1mM of KOH
  4. 4 kg of HCl with a molarity of 1mM
Question 17
17.
This is the ionic equation for question 16.

2Rb+1(aq) + S-2(aq) + Cu+2(aq) + 2I-1(aq) -> 2Rb+1(aq) + 2I-1 (aq) + CuS(s)

Fill in the dropdown menus with the correct net ionic equation by removing the spectator ions.

__________ + __________ = __________
Question 25
25.

Which of these is not a method of salt preparation shown in the video?

Question 40
40.

What is an indicator used for in a titration reaction?