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Chemistry - ACIDS AND BASES > Chapter 4.1 - Introducing Acids and Bases > Flashcards

Chapter 4.1 - Introducing Acids and Bases Flashcards

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1
Q

What are ACIDS?

A

According to the Bronstead-Lowry Theory, An Acid is a substance capable of donating a Hydrogen ion/Proton

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2
Q

What is Acidity?

A

The concentration of H3O+ ions in an aqueous solution.

- Measured on a pH scale.

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3
Q

What is a BASE?

A

According to Bronstead-Lowry theory, a substance capable of accepting a proton/Hydrogen ion.

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4
Q

Hydrochloric Acid
Formula
Uses

A

HCl

  • Stomach acid to help breakdown proteins
  • cleaning agent for brickwork
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5
Q

Sulfuric Acid
Formula
Uses

A

H2SO4

  • chemical manufactured for Car batteries, fertilizers, detergents.
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6
Q

Nitric Acid
Formula
Uses

A

HNO3

  • fertilizers, dyes, and explosives
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7
Q

ETHANOIC/ ACETIC ACID
Formula
Uses

A

CH3COOH

  • vinegar, used as a preservative
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8
Q

Carbonic Acid
Formula
Uses

A

H2CO3

-soft drinks and beer

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9
Q

Phosphoric Acid
Formula
Uses

A

H3PO4

  • soft drinks and manufacture of fertilizers
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10
Q

Citric Acid
Formula
Uses

A

C6H8O6

  • found in citrus fruits
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11
Q

Ascorbic Acid
Formula
Uses

A

C6H8O6

  • citrus fruits (VITAMIN C)
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12
Q

What is an ALKALI?

A

A soluble base

  • base definition also
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13
Q

What is a solution?

A

A homogenous mixture of a solute dissolved in a solvent

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14
Q

Sodium hydroxide (Caustic Soda)
Formula
Uses

A

NaOH

Used in drain and oven cleaners,
Soap making

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15
Q

Ammonia
Formula
Uses

A

NH3

Used in Household cleaners, fertilizers and explosives

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16
Q

Calcium Hydroxide
Formula
Uses

A

Ca(OH)2

Found in Cement and mortar
Used in garden lime to adjust soil pH

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17
Q

Magnesium Hydroxide
Formula
Uses

A

Mg(OH)2

Ingredient In ANTACID, EG MILK OF MAGNESIA to overcome indigestion

18
Q

Sodium Carbonate
Formula
Uses

A

Na2CO3

manufacture washing powder and glass

19
Q

What are some common properties of all ACIDS? (6)

A
  1. Turns litmus paper red
  2. Tend to be CORROSIVE
  3. SOUR TASTE
  4. REACTS with BASES: neutralization may occur
  5. Solutions have relatively low pH
  6. Solutions CONDUCT ELECTRIC CURRENT
20
Q

What are some common properties for all BASES?

A
  1. Turns Litmus paper blue
  2. are Caustic and FEEL Slippery
  3. Tastes Bitter
  4. Reacts with Acids
  5. Solutions have relatively high pH
  6. Solutions conduct an electric current
21
Q

Why do bases feel slippery?

A

Bases feel slippery/soapy.

This is because they dissolve the fatty acids and oils from your skin and this cuts down on the friction between your fingers as you rub them together.

Good for cleaning products because they react with fats and oils to produce water-soluble soaps

22
Q

Explain the Bronsted-Lowry theory

A

This theory explains that a substance behaves as an ACID WHEN IT DONATES PROTON (H+) to a base.

A substance behaves like a BASE when it ACCEPTS A PROTON from an Acid.

23
Q

What is an Acid-Base reaction?

A

An acid-base reaction involves an exchange of protons from an acid to a base.

eg. HCl(g) + H2O(l) –> H3O+ (aq) + Cl- (aq)

24
Q

Explain the acid-base reaction.

eg. HCl(g) + H2O(l) –> H3O+ (aq) + Cl- (aq)

ACID? BASE? REACTION EQUATIONS

A
  1. In an Aqueous solution of Hydrogen chloride, nearly all the hydrogen chloride is present as ions – virtually no molecules of hydrogen chloride remain.
    - - This solution is known as Hydrochloric acid.
  2. The HCl molecule has donated a proton to the water molecule, forming the HYDRONIUM ION (H3O+ (aq))
    - HCl has acted as the Acid
    - Water is the base then,
  3. The hydronium ion can be represented as either H3O+ (aq) or H+ (aq).

Therefore can be represented as either a Hydrolysis reaction

HCl(g) + H2O (L) —> H3O+ (aq) + Cl - (aq)

or a DISSOCIATION REACTION.

HCL (g) —> H+ (aq) Cl- (aq)

25
Q

Dissociate vs Ionise?

A
  1. Ionisation is the process that involves the formation of ions
    - Ionisation involves the creation of charges across the participating species
    - become charged
  2. dissociation is the process of breaking up a molecule into its constituent atoms, molecules, and ions.
    - dissociation occurs due to a weak bond between species.
    - breakup
26
Q

What is Hydrolysis?

A

A reaction involving the breaking of a bond in a molecule using water as a reactant.

2 smaller molecules are usually formed

27
Q

What is a Hydrolysis Reaction?

A

A reaction that occurs when a molecule or ion in an aqueous solution reacts with water, either accepting or donating a proton.

28
Q

What are the Advantages of the Bronstead-Lowry model?

A
  1. Acids and bases are not restricted to aqueous solutions.
    eg. a reaction between gases can be an acid-base reaction.
  2. Because it categorized acid-base reactions in the case of proton transfer.
example :
solutions
HCl (aq) +NH3 (aq) ---> NH4+ (aq) + Cl- (aq)
gases
HCl (g) + NH3 (g) ---> NH4Cl (s)
29
Q

What are the limitations of the Bronstead-Lowry Model?

A
  1. It cannot be applied to the reaction between acidic and basic oxides.

under certain conditions solid calcium oxide, a basic oxide reacts with gaseous carbon dioxide, an acidic oxide to produce calcium carbonate salt.

CaO (s) + CO2 (g) —> CaCO3 (s)

30
Q

What are conjugate acid-base pairs?

What are Conjugate acids and bases?

A

Conjugate acid-base pairs are molecules that differ from each other by an H+ ion.

(on other side of the equation)
When a conjugate acid donates a proton, it forms a conjugate base.

When a base accepts a proton, it forms a conjugate acid.

31
Q

How can the proton/hydrogen ion affect acidity of a solution be represented?

A

A proton or hydrogen ion in a solution can be represented by the hydronium ion, H3O+ (aq), or simply as H+ (aq)

32
Q

What are Amphiprotic substances?

Example?

A

They are substances that act as either acids or bases, depending on the substance with which they are reacting.

example WATER - can act as a base or acid depending on the solute present.

  • if the SOLUTE is STRONGER ACID than water, then the WATER will act as a BASE.
  • if the SOLUTE is a STRONGER BASE than Water, then the WATER will act as an ACID.

Although both reactions are possible for all amphiprotic substances in water, generally one reaction dominates.

33
Q

Examples of Amphiprotic substances

A 
H2O 
HCO3-
H2PO4- 
HPO4 (-2)
HSO4 -
34
Q

How to determine the dominant amphiprotic reaction?

A

The dominant reaction can be identified by measuring the pH

  • A measure of the amount of hydronium ion in solution.
35
Q

What are monoprotic acids?

Examples?

A

Acids that can donate ONLY ONE proton per molecule.

  • only the hydrogen part of the highly polar O-H bond is donated
  • The hydrogen atom is called the ACIDIC PROTON

HCl
HF (hydrofluoric acid)
HNO3
CH3COOH

36
Q

What is a polyprotic acid?

A

An acid that can donate more than 1 proton to a base.

  • the number of hydrogen ions an acid can donate depends on the structure of the acid
  • they do not donate all at once but does so in steps when reacting with a base
  • Diprotic donates 2
  • Triprotic donates 3
37
Q

Example of Diprotic acids

A
  1. Sulfuric Acid - H2SO4

2. Carbonic Acid - H2CO4

38
Q

What are the stages a diprotic acid, such as sulfuric acid ionizes?

A

2 stages

stage 1 : H2SO4 (L) + H2O (L) —-> HSO4- (aq) + H3O+ (aq)

Stage 2 : HSO4- (aq) + H2O (L) SO4 (-2) (aq) + H3O+ (aq)

39
Q

Examples of triprotic acids

A
  1. PHOSPHORIC ACID - H3PO4

2. BORIC ACID (H3BO3)

40
Q

How do triprotic acids ionize?

A

3 stages
- the extent of ionization decreases progressively from stages 1 to 3.

stage 1 : H3PO4 (aq) + H2O (L) H2PO4 - (aq) + H3O+ (aq)
stage 2: H2PO4 (-2) - (aq) + H2O (L) HPO4 (-2) (aq) + H3O+ (aq)
stage 3: HPO4 (-3) (aq) + H2O (L) PO4 (-3) + H3O+ (aq)

Chemistry - ACIDS AND BASES (4 decks)

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