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DE_CH_5.3_Acids, Bases, and Salts

Last updated over 2 years ago
41 questions
Background Knowledge
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1

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

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3

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

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2
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_______.
Required
1
log(0.001) = _______
log 4 + log 3 = log _______
2 = log ________
Other Answer Choices:
100
-3
12
1
7
-1
-2
10
Required
2

Match each acid formula with its name.

Draggable itemCorresponding Item
HCl
hydrocloric acid
HClO3
hypoclorous acid
HClO
chlorous acid
HClO2
cloric acid
HClO4
pechloric acid
Acid-Base Theories (1)
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2
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.
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1

What will hydrochloric acid form when added to water?

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1

What will sodium hydroxide form when added to water?

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2
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).
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1

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

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2
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.
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1


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

Precipitation Reactions (2)
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1

What is a precipitation reaction?

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1
A precipitation reaction can sometimes occur when two __________ are mixed together in an aqueous solution.
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1

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

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2
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
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.

__________ + __________ = __________
Acid-Base Strength (3-4)
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1

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

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1

All acids dissociate, but only some will ionize.

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1
Strong acids and bases dissociate _______ in water. Weak acids and bases dissociate _______ in water.
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2

Categorize the following statements.

  • Forms a conjugate base
  • Ka
  • B = OH- + BH+
  • HA = H+ + A-
  • Kb
  • Forms a conjugate acid
  • Acid Reactions
  • Base Reactions
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1

Which of these compounds is an amphoteric substance?

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1

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

Acid-Base Reactions and Buffers (5-6)
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1

Match the correct reaction type to the corresponding chemical equation.

Draggable itemCorresponding Item
weak acid-strong base
HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (aq)
weak acid-weak base
HC2H3O2 (aq) + KOH (aq) → H2O (aq) + KC2H3O (aq)
strong acid-weak base
HCl (aq) + NH3 (aq) ⇄ NH4Cl (aq)
strong acid-strong base
NH3 (aq) +H2O (aq) ⇄ NH4+ (aq) + OH- (aq)
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1

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

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1

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

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1

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

HClO4 + KOH →

Select the correct right hand side from the list below.

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2
Complete the following chemical reaction when ammonia acts as a base.

NH3 + H20 → _______ + _______
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1

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

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2
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.
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1

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

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1

What is the equation for Neutralization?

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1

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

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1

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?

Required
2

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?

pH and pOH (7-8)
Required
1
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
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1
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 _______.
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1

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

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1

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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1

What is an indicator used for in a titration reaction?

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1

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