Acids and Base

Question 1

Bronsted lowry acid

Answer 1

Proton donor

Question 2

Bronsted lowry base

Answer 2

Proton acceptor

Question 3

Alkali

Answer 3

A type of base which releases OH- ions into a solution

Question 4

Conjugate base pair

Answer 4

Species formed when an acid donates a proton and can then accept a proton and act a base (vice versa)

Question 5

Example of monobasic acid

Answer 5

HCl

Question 6

Example of tribasic acid

Answer 6

H3PO4

Question 7

Example of dibasic acid

Answer 7

H2SO4

Question 8

Weak acids examples

Answer 8

CH3COOH, Citric acid

Question 9

Strong acid examples

Answer 9

HCl, H2SO4, H3PO4, HNO3

Question 10

Equation for pH

Answer 10

-log[H+] (2dp)

Question 11

Equation for H+

Answer 11

10-pH

Question 12

Equation for acid dissociation constant/ Ka for a weak acid

Answer 12

([base] x [H+]) / [acid]

Question 13

What does a large Ka value indicate?

Answer 13

Stronger acid

Question 14

Equation for pKA

Answer 14

-log(Ka)

Question 15

Inverse of kPA

Answer 15

10^-pKA

Question 16

Approximations for weak acids

Answer 16

• At equilibrium the concentration of acid is much greater than H+
• Concentration of H+ and A- is the same at equilibrium
• The dissociation of water is negligible

Question 17

Limitations for approximation of weak acid

Answer 17

• Doesn’t apply to a equilibrium dissociation of 5% because the equilibrium value of acid is too different compared to the start
  -[Acid]eq > [H+]eq does not apply to strong weak acids

Question 18

Ionic product of water

Answer 18

Kw (1.00x10^-14) = [H+aq] x [OH-] at 298K

Question 19

What does the ionic product of water assume?

Answer 19

The dissociation of water is negligible