M6 Topic 2 Using Bronsted-Lowry Theory Part 1 Flashcards
conduct an investigation to demonstrate the use of pH to indicate the differences between the strength of acids and bases (ACSCH102) ● write ionic equations to represent the dissociation of acids and bases in water, conjugate acid/base pairs in solution and amphiprotic nature of some salts, for example: – sodium hydrogen carbonate – potassium dihydrogen phosphate
What are conjugate Acid/Base pairs
two species that differ by one hydrogen ion
what happens when a strong acid react with a strong base(2)
- they fully dissociate in solution(form into ions)
- give a PH of 7
what happens when a weak base reacts with a weak acid(2)
- They form a equilibrium reaction
- give a PH of 7
what happens when a weak acid reacts with a strong base
-gives a PH of more than 7
what happens when a strong acid reacts with a weak base
- gives a PH of less than 7
How is the strength of a acid or base calculated
through the acid/base dissociation constant (Kₐ, Kb) being put into a logarithmic scale (PKa,PKb)
what is the equation to get the acid/base dissociation constant
Kₐ, Kb = products(ions)/reactant
what is the equation to turn the acid/base dissociation constant into a logarithmic scale
PKa,PKb= -log₁₀[Kₐ,Kb]
examples of strong acids (3)
HCl - Hydrochloric acid
HBr - Hydrobromic acid
HI - Hydroiodic acid
Examples of strong Bases (3)
LiOH - Lithium hydroxide
NaOH - Sodium Hydroxide
KOH - Potassium hydroxide
Examples of weak acids (3)
CH₃COOH - Acetic acid
HF - Hydrofluoric acid
HCOOH - Formic Acid
Examples of weak bases (3)
NH₃ - Ammonia
H₂O - Water
NH₄OH - Ammonium Hydroxide
what are Amphoteric substances
Substance that can act as an acid or a base
examples of amphoteric substances (2)
- Sodium hydrogen carbonate
- Potassium dihydrogen phosphate
What is a polyprotic acid
an acid that contains multiple hydrogens
