Acids and Bases
No description yet. This curated deck is ready for daily study.
Card preview (24)
Define a Brønsted-Lowry Acid?
A proton Donor
Define Brønsted-Lowry Base
Proton Acceptor
What ion causes a solution to be acidic
The oxonium ion H3O+ Protons react with H2O to form it
What ion causes a solution to be alkaline
-OH Hydroxide ion
Write the equation for the ionisation of water
Derive the Kw Equation using the ionisation of water
Ka = [H3O+][OH-] / [H2O] [H2O] Kw = [H3O+][OH-] [H2O] is so large in comparison to [H3O+] and [OH-] That it is considered to remain constant Kw = [H3O+][OH-]
State the value of kw at 298k
10^-14
What physical factors affect the value of Kw and explain why
Temperature only If temperature is increased the eqm moves in the endothermic direction (right) Kw therefore increases and the Ph of pure water decreases
Why is pure water still neutral even if the ph doesn’t equal 7?
[H3O+] = [OH-]
What is the equation for Ph? What bace is the logarithm to
Ph = -log(H3O+) Base 10
A lower ph has a _____________________________
Higher concentration of [H+] present
A Ph difference of 1 is a ______________ difference in [H+]
A factor of 10
How do you find [OH-] From ph
1) PH —-> [H3O+] 2) Kw = [H3O+][OH-] 3) Kw at 298k = 10^-14
Explain the difference between monoprotic, diperotic and triprotic acids?
Produce different amounts of Protons per mol of acid Monoprotic —> 1 Mol of [H+] from 1 mol of acid DiProtic ——> 2 Mol of [H+] from 1 mol of acid Triprotic ——> 3 Mol of [H+] from 1 mol of acid
How do you calculate the PH of a strong alkaline solution?
1) Kw = [H+][OH-] 2) ph = -log([H+])
Define the term strong acid?
An acid which dissociates fully into their ions within aqueous conditions
Define the term strong bace
A bace which fully dissociates into their ions in water
What is the difference between a strong acid and a concentrated one?
Concentrated acids have many moles per unit volume Strong acids dissociate fully in water
What is a weak acid and bace
Acids and braces which only dissociate partially into their ions in aqueous conditions
Name some strong acid examples
H2SO4 - Diprotic HCl - Monoprotic H3PO4 - Triprotic
Give some examples of strong bases?
NaOH CaCO3 Na2CO3
Give an example of a weak acid
Ethanoic acid - CH3COOH Any organic acid
Give an example of a weak Base?
NH3 Ammonia
Write the expression for Ka
Ka = [H+][A-] / [HA] Where HA (reversible) [H+][A-]