Acids and Bases EQUATIONS Flashcards
What is the equation for pH
pH = -log[H⁺]
What is the equation for [H⁺]
[H⁺] = 10⁻ᵖᴴ
What is the equation for K꜀ for H2O
K꜀ = [H⁺] [OH⁻] / [H2O]
What is the equation for Kᵥᵥ
Kᵥᵥ = [H⁺]²
What is the equation for Kₐ
Kₐ = [H⁺] [A⁻]/[HA]
Since [H⁺] = [A⁻] in the equation HA ⇌ H⁺ + A⁻
Kₐ = [H⁺]²/[HA]
What is Ka
A weak acid approximation
What is the equation for pKa
pKa = -logka
How do we get Ka from pKa
Ka = 10⁻ᵖᴷᵃ
What is the equation for the dissociation of a weak acid
HA ⇌ H⁺ + A⁻
If Ka is small what does this mean about the strength of an acid
If Ka is small - means a weaker acid (weaker, weak acid since Ka is for weak acids)
If Ka is large what does this mean about the strength of an acid
If Ka is large - means a stronger acid (stronger, weak acid since Ka is for weak acids)
If pKa is small what does this mean about the strength of an acid
If pKa is small - means a stronger acid (stronger, weak acid since Ka is for weak acids)
If pKa is large what does this mean about the strength of an acid
If pKa is large- means a weak acid (weak, weak acid since Ka is for weak acids)
What is the equation for the dissociation of H2O
H2O ⇌ H⁺ + OH⁻
Is the dissociation of water exothermic or endothermic
Endothermic, +ΔH
What is a buffer solution
A solution which resists changes in pH on addition of a small amount of acid, base or on dilution with water
What the dissociation equation for making a buffer solution by adding a salt to a weak acid
HA ⇌ H⁺ + A⁻
(A- from salt)
What is the equation for calculating [H+] of a buffer solution
[H+] = Ka x nHA/nA⁻
What is the moles of A⁻ equal too when making a buffer by adding a base to an acid
nA⁻ = nOH⁻
What is the dissociation equation when making a buffer by adding a base to an acid
HA + OH⁻ ⇌ A⁻ + H2O
What is the equation to calculate the new [H+] of a buffer solution when we add an acid to it
nH+ = mol of H+ added
What is the equation to calculate the new [H+] of a buffer solution when we add a base to it
nOH- = mol of OH- added
