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Chemistry 3AB FO REAL > Chapter 8 Acids and Bases > Flashcards

Chapter 8 Acids and Bases Flashcards

1
Q

Define an Acid and Basic solution in basic terms. (basic lol)

A
  1. Acidic Solution:
    - Typically conduct an electric current, will turn blue litmus red and have a sour taste.
    - Acidic properties occur if its hydrogen ions concentration is greater than its hydroxide ion concentration.
  2. Basic Solution:
    - Also conducts and electric current; however, these solutions will turn red litmus blue, have a bitter taste and a slippery, soapy feel.
    - Basic properties occur if the hydroxide ions concentration exceeds the hydrogen ion concentration.
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2
Q

Acid + Metal ->

A

Salt + H2(g)

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3
Q

Acid + Metal Hydroxide ->

A

Salt + H2O

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4
Q

Acid + Metal oxide ->

A

Salt + H2O

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5
Q

Acid + Carbonate ->

A

Salt + H2O + CO2(g)

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6
Q

Acid + Hydrogencarbonate ->

A

Salt + H2O + CO2(g)

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7
Q

Acid + Metal Sulfite ->

A

Salt + H2O + SO2(g)

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8
Q

Base + Ammonium Salt ->

A

Salt + H2O + NH3(g)

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9
Q

Base + Non Metal Oxide ->

A

Salt + H2O

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10
Q

What does the covalent molecular structure of water means?

A

It consist of molecules of formula H2O where each molecule is a covalently bonded cluster of one oxygen atom and two hydrogen atoms.

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11
Q

How are ions (H+ and OH-) produced from H2O molecules?

A

By the reversible reaction known as autoionisation or simply as self-ionisation.

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12
Q

Why is water said to be Neutral?

A

Because the formation of one hydrogen ion is always accompanied by the formation of one hydroxide ion, then in pure water H+(aq) and OH-(aq) ions have the same concentration.

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13
Q

Why is water said to be a Weak Electrolyte?

A

In pure water, both H+(aq) and OH-(aq) ions have the same extremely low concentration of 1 x 10^-7 mol L-^-1.

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14
Q

What does the Arrhenius Theory state?

A

The theory states that:

  1. An acid is a substance that will ionise in solution producing H+(aq) ions.
  2. A base is a substance that will dissociate in solution releasing OH-(aq) ions.
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15
Q

What is the Arrhenius Theory?

A

-It explains that the change in [H+(aq)] and [OH-(aq)] is caused by solutes that release hydrogen ions by ionisation or hydroxide ions by dissociation. easing OH-(aq) ions.

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16
Q

What does Arrhenius describe a strong acid or weak acid as?

A
  1. Strong Acid: One that undergoes complete ionisation in water.
  2. Weak Acid: By comparison, only undergoes partial ionisation.
    - This different ability to undergo ionisation, explains why a strong acid always produce a higher hydrogen ion concentration than does a weak acid of the same acid concentration.
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17
Q

What does the Bronsted-Lowry theory state?

A
  • An acid is a substance that donates a proton.

- A base is a substance that accepts a proton.

18
Q

What is the Bronsted-Lowry?

A
  • The Bronsted-Lowry theory, first proposed in 1923, explains acid-base behaviour in terms of proton transfer between two species, ie hydrogen ion transfer.
  • This theory has greater application as it can better account for the basic nature of aqueous solutions of species like NH3 and HCO3- which do not themselves contain hydroxide ions.
19
Q

What does the Bronsted-Lowry describe a strong acid or base in aqueous solution as ?

A
  • One that undergoes complete hydrolysis with water, as in reaction.
  • Weak acids or bases only undergo partial hydrolysis with water.
20
Q

List all the common Strong Acids.

A
  • HCl
  • H2SO4
  • HNO3
21
Q

List all the common Weak Acids.

A
  • H2C2O4 (Oxalic Acid)
  • H2SO3 (Sulfurous acid)
  • HSO4- (Hydrogen Sulfate Ion)
  • H3PO4 (Phosphoric Acid)
  • CH3COOH (Ethanoic Acid)
  • H2CO3 (Carbonic Acid)
  • H2PO4- (Dihydrogen phosphate ion)
  • H2S (Hydrogen Sulfide)
  • NH4+ (Ammonium Salt)
22
Q

List all the common Strong Bases.

A
  • Oxide Ion

- Hydroxide Ion

23
Q

List all the common Weak Bases.

A
  • S2-
  • (PO4)3-
  • (CO3)2-
  • NH3
  • HS-
  • (HPO4)2-
  • HCO3-
  • CH3COO-
24
Q

Where does the term Conjugate acid and Conjugate base orginate from?

A

The Bronsted-Lowry theory also recognises the potential for proton transfer to be reversed.

25
Q

What is a Conjugate Acid and Base?

A

Conjugate Acid: When a base has gained a proton. It could potentially donate this gained proton, thus act as an acid.

Conjugate Base: When the product of an acid that has donated a proton, called the conjugate base of that acid, could potentially acs as a base by regaining a proton.

26
Q

How can the acid-base properties of salts be understood in terms of the Bronsted-Lowry theory?

A

-If one of the ions present in a salt, reacts with water acting
as a proton donor (acid), then its solutions will be acidic.

  • Some salts contain an ion that reacts with water acting as a proton acceptor (base). These salts produce a basic solution.
  • Some salts contain both an acidic and a basic ion. In this situation the salt may be neutral or its acidity is governed by the ion with the strongest acid or base characteristics.
27
Q

What is Kw?

A

With reference to the equilibrium expression for the autoionisation (self-ionisation) of water, known as Kw.

28
Q

What are some important points to understand about the Kw expression?

A
  • It confirms the concentration of H+ and OH- are inversely related. Hence any increase in the H+ concentration causes a corresponding decrease in the OH- concentration and vice versa.
  • Its extremely small value (1x10^-14) is a reminder of the strong tendency for water to remain in the unionised, molecular form, as H2O molecules, rather than the ionised H+ and OH- form.
  • Although Kw has a constant value for most conditions, it does change value with temperature. As the autoionisation of water is endothermic then by Le Chatelier’s principle, higher temperatures will favour the formation of products. This means the concentration of both H+ and OH- rise with increasing temperature. FOr this reason Kw will be higher at higher temperatures.
29
Q

What does a solution’s acidity depend on?

A

It depends upon its H+ concentration.

30
Q

How can the pH of a strong acid or strong base solution of a known concentration be determined?

A

Through the relationship of the pH equation and Kw.

31
Q

In a mixture of two or more strong acid solutions the mole of hydrogen ion present in the mixture is additive. Explain what this means.

A
  • This means the concentration of hydrogen ions in a mixture of strong acids is equal to the total moles of hydrogen ions from both solutions divided by the total volume of the two solutions.
  • Similarly in a mixture of two or more strong base solutions the moles of hydroxide ion present is additive.
  • Thus the concentration of hydroxide ions in a mixture of strong bases is equal to the total moles of hydroxide ions from both solutions divided by the total volume of the two solutions.
32
Q

What are Buffers?

A

Buffers are solutions that have the ability to resist pH change when either acids or bases are added to them.

33
Q

What is a Buffer in general?

A
  • Generally, a buffer solution is one that contains a weak acid-base conjugate pair.
  • This means a buffer solution may contain a weak acid and its conjugate base or it may contain a weak base and its conjugate acid.
34
Q

What is buffering capacity?

A
  • It is the ability of a buffer solution to neutralise excess acid or base without appreciable change in its pH.
  • It can be defined as the amount of acid or base the buffer can neutralise before the pH begins to change appreciably.
35
Q

What can be done for the buffer to be most effective?

A
  • It should contain a relatively large amount of both the weak acid and weak base.
  • This ensure neither the weak acid or its weak conjugate base will be significantly depleted or reduced in concentration on the addition of either excess OH- or H3O+.
36
Q

What are monoprotic acids?

A

Acids such as hydrochloric acid and nitric acid that only donate one hydrogen ion (a proton) in an acid-base reaction are called monoprotic acids.

37
Q

What are multiprotic acids?

A

Acids that can donate more than one hydrogen ion.

38
Q

What is a hydrolysis reaction?

A

When the substance donates a hydrogen ion to, or accepts a hydrogen ion from, water.

39
Q

What is a salt?

A
  • A salt is an ionic compound that contains a negative ion (an anion) other than the oxide ion, O2-, or the hydroxide ion, OH-.
  • A salt can be thought of as a compound whose positive ions (cations) are derived from a base and negative ions from an acid.
    e. g. Sodium fluoride, Calcium Carbonate, Irone (III) sulfate and ammonium nitrate.
40
Q

What happens when a salt dissolves in water?

A
  • It dissociates completely into ions.

- Salts are strong electrolytes.

41
Q

Give an example of a hydrolysis reaction.

A

Since it is possible that one or both of the ions produced in the dissociation reaction can undergo further reaction with water.

Chemistry 3AB FO REAL (11 decks)

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