Acids and Bases Deck 1 Flashcards
Define an acid
Proton Donor
Define a base
Proton Acceptor
Define a strong Acid
An acid (proton donor) which fully dissociates
Define a weak Acid
An acid ( proton donor) which only partially dissociates
Define pH
pH = -Log10[H+]
[H+] =
[H+] = 10-pH
Ionic Product of Water (Kw) =
Kw = [H+][OH-]
When calculating the pH of a strong acid use:
pH = -Log10[H+]
When calculating the pH of a strong base use:
Rearrange Kw = [H+][OH-] to get [OH-] then use pH = -Log10[H+]
When calculating the pH of a weak acid use:
Ka = [H+]2/[HA] and rearrange to get [H+]
then use pH = -Log10[H+]
Chemical equation for Hydrochloric Acid + Sodium
HCl(aq) + Na(s) –> NaCl(aq) + ½ H2(g)
Chemical equation for Nitric Acid + Potassium Oxide
2HNO3 (aq) + K2O(s) –> 2KNO3 (aq) + H2O(l)
Chemical equation for Phosphoric Acid + Sodium Hydroxide
H3PO4(aq) + 3NaOH(s) –> Na3PO4(aq (aq) + 3H2O(l)
Chemical equation for Hydrochloric Acid + Calcium Oxide
2HCl (aq) + CuO(s) –> CuCl2 (aq) + H2O(l)
Chemical equation for Sulfuric Acid + Sodium Carbonate
H2SO4(aq) + Na2CO3(s) –> Na2SO4(aq) + CO2(g) + H2O(l)
A difference of 1 on the pH scale means
a 10x difference in [H+]
pKa =
-Log10Ka
Ka =
10-pKa
The value of Kw will alter with temperature, explain why pure water is always neutral
because [H+] = [-OH] at all times.
Formula for sulphuric acid
H2SO4
Formula for nitric acid
HNO3
Formula for phosphoric acid
H3PO4
Formula for ethanoic acid
CH3COOH
Formula for aluminium phosphate
AlPO4
Formula for sodium ethanoate
CH3COONa
Formula for lead (II) nitrate
Pb(NO3)2
Formula for potassium sulphate
K2SO4
Formula for magnesium chloride
MgCl2
Explain how to chose a suitable indicator for a titration
A SUITABLE INDIATOR CHANGES COLOUR SOMEWHERE ON THE VERTICAL SECTION OF A pH TITRATION CURVE
What does the vertical section of a titration curve show?
This indicates what the average titre would be which can be used in a calculation. The midpoint of this vertical section is the equivalence point.
