Basic Definitions

Question 1

When acid is added to water, what ion is released in the solution?

Answer 1

Hydrogen ion, H+

Question 2

Define Bronsted-Lowry acid

Answer 2

Proton donor

Question 3

Describe the dissociation of a strong acid

Answer 3

Full dissociation

Question 4

Define Bronsted-Lowry base

Answer 4

Proton acceptor

Question 5

monobasic acids

Answer 5

Acids such as HCl, HNO3, and HCN that contain one ionisable hydrogen atom in each molecule

Question 6

Dibasic acids

Answer 6

Contains two ionisable hydrogen atoms per molecule, for example H2SO4

Question 7

Tribasic acids

Answer 7

Acids that contain three ionisable hydrogen atoms per molecule, for example H3PO4

Question 8

Definition of pH

Answer 8

-log10[H+]

Question 9

Weak acid dissociation

Answer 9

Weak acids only barely dissociate in solution.

Question 10

Acid dissociation constant

Answer 10

Ka= [H+][A-]/[HA]

Question 11

Units of the acid dissociation constant

Answer 11

mol dm-3

Question 12

What does the value of Ka mean

Answer 12

*The higher the value of Ka the more dissociated the acid and the stronger it is
*The lower the value of Ka the weaker the acid

Question 13

pKa and what it means

Answer 13

*The range of values of Ka is very large and for weak acids, the values themselves are very small numbers

Question 14

What does Kw mean

Answer 14

‘The ionic product of water’

Question 15

Concentration of [H+]

Answer 15

[H+]= 10*-pH

Question 16

ionic equation to show the dissociation of water

Answer 16

H2O= H+ = OH-