Gen 6 - Acids and Bases Flashcards Preview

GAMSAT March 2016 > Gen 6 - Acids and Bases > Flashcards

Flashcards in Gen 6 - Acids and Bases Deck (45)
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1

What is a Bronsted Acid ?

An acid is a proton (ie. H+) donor

2

HA + H2O ⇔ ? + ? 

H3O+ + A-

3

What is the equation for the equilibrium constant Ka ? 

4

Name the two catergories of Acids in general chemistry ? 

  • Binary Acids 
  • Oxy Acids 

5

Describe binary acids ? 

Acids composed of hydrogen and a non-metal e.g. HCl

6

Describe the trend displayed by halogen containing binary acids ? 

As halogen size increases, acid strength also increases. 

Bond length also increases, which means bond strength decreases, leading to increased acidity. 

7

What are Oxyacids ? 

Anions containing a non-metal oxygen such as hydroxide or nitrate ions. They contain:
H - O - X

8

Describe the acidity of Oxyacids ? 

The more oxygen atoms bound to the central atom, the more acidic the oxyacid. 

9

What are diprotic acids ? 

Acids with two protons e.g. H2SO4

10

Describe the equilibrium constant Ka for diprotic or polyprotic acids ? 

The acids would have Ka values for each of its protons, e.g. Ka1 for the first, Ka2 for the second. 

The acids ionise in successive steps with their own Ka's. 

Ka1 is typically > Ka2

11

Give 8 examples of strong acids 

  1. Perchloric HClO4
  2. Chloric HClO3
  3. Nitric HNO3
  4. Hydrochloric HCl
  5. Sulfuric H2SO4
  6. Hydrobromic HBr
  7. Hydroiodic HI
  8. Hydronium ion H3O+

12

What is a base ? 

A proton accepter 

13

B + H2O ⇔ ? + ? 

HB+ + OH-

14

What is the equilibrium constant for a base ? 

15

Give examples of strong and weak acids ? 

Strong bases include any hydroxide of the Group 1A metals e.g. Na, K, Li etc...

The most common weak bases are ammonia and any organic amine. 

16

Why is water amphoteric ? 

It can act as an acid and a base 

17

How does Ka relate to relative acid strength 

The greater the magnitude of Ka, the stronger the acid (the more the reaction proceeds to the right). 

18

What is a conjugate acid-base pair ? 

The acid [HA] and the base produced when it ionises [A-]. 

E.g. HCN and CN-

19

Describe relative strength in conjugate acid-base pairs ? 

If the main acid or base is strong, the conjugate acid or base will be weak, and vice versa. 

20

Explain why an amino acid is an example of a conjugate acid-base ?

It has two groups, the acidic carbonyl group, and the base amine group. 

21

Give a biological example of a Zwitterion ? 

In blood plasma (pH 7.4) the predominant form of amino acids is COO-, NH3+

22

What is the ion product constant for water at STP ? 

Kw = [H+] [OH-] = 1.0 x 10 -14

 

This is the equilibrium constant for the reaction in which water undergoes an acid-base reaction with itself. 

23

What is the pH of a solution ?

An expression of the concentration of hydrogen ions in a solution. 

pH = -log10[H+]

24

If the [H+] of solution of pure water is [H+] = 10-7, what is the pH ? 

7.0

25

If pH is > 7, how is the solution described ? 

Alkaline (basic)

26

If the pH is < 7, how is the solution described ? 

Acidic 

27

How can pH be measured quantitatively and qualitatively ? 

Quantitative = pH meter 

Qualitative - indicator 

28

What is the most commonly encountered weak acid ? 

Acetic acid HOAc 

29

If the Ka of an acid is 1.75 x 10 -15, what is the relative strength of the acid ? 

Weak 

N.B. Log 10=1, Log 1=0)

30

What is a salt ? 

An ionic compound in which the anion is not OH-, or O2-, and the cation is not H+