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DE_CH_5.3_Acids, Bases, and Salts

Last updated almost 3 years ago

41 questions

Background Knowledge

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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.

Other Answer Choices:

100

-3

12

1

7

-1

-2

10

Question 5

5.

Draggable item		Corresponding Item

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.

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.

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.

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2

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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.

Question 20

20.

Strong acids and bases dissociate _______ in water. Weak acids and bases dissociate _______ in water.

Question 21

21.

Question 22

22.

Question 23

23.

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

Question 24

24.

Draggable item		Corresponding Item

Questions 25 & 26

01:37

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1

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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.

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.

Question 32

32.

What is the equation for Neutralization?

Question 33

33.

Question 34

34.

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.

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.

log(0.001) = _______ 
log 4 + log 3 = log _______ 
2 = log ________ 

Match each acid formula with its name.

HClO4

hydrocloric acid

HClO2

hypoclorous acid

HCl

chlorous acid

HClO

cloric acid

HClO3

pechloric acid

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

lost from a nucleus

an unbonded hydrogen ion

an unbonded hydroxide ion

gained in the nuclus

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

True

False

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

Question 16

16.

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

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.

__________ + __________ = __________

All acids dissociate, but only some will ionize.

True

False

Categorize the following statements.

HA = H+ + A-

B = OH- + BH+

Forms a conjugate acid

Ka

Kb

Forms a conjugate base

Acid Reactions

Base Reactions

Which of these compounds is an amphoteric substance?

HCL

H2SO4

H2O

NaOH

Match the correct reaction type to the corresponding chemical equation.

strong acid-weak base

HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (aq)

strong acid-strong base

HC2H3O2 (aq) + KOH (aq) → H2O (aq) + KC2H3O (aq)

weak acid-weak base

HCl (aq) + NH3 (aq) ⇄ NH4Cl (aq)

weak acid-strong base

NH3 (aq) +H2O (aq) ⇄ NH4+ (aq) + OH- (aq)

Question 25

25.

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

HClO4 + KOH →

Select the correct right hand side from the list below.

H204 + KClO

H2O3 + KClO2

H2O2 + KClO3

H2O + KClO4

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

water and a salt

water and sugar

a weak acid

a strong base

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

1.20 mL

30 mL

748 mL

1330 mL

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?

2.67

10 mL

37.5 mL

600 mL

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

True

False

Question 40

40.

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

Bleach with a pH of 12.6

1mM of KOH

5 g of distilled water

4 kg of HCl with a molarity of 1mM

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

Oxidation of metals

Reactions between acids and insoluble bases or metals

Titration

Precipitation

What is an indicator used for in a titration reaction?

Indicators will change an acid into a base.

Indicators will change color when a precipitate is formed.

Indicators will dissolve an acid or base until it is neutralized.

Indicators will change color when exposed to an acid or a base of a certain strength.