Aqueous Solutions Flashcards
Hydrochloric Acid
HCl
strong monoprotic acid
Hydrofluoric Acid
HF
weak monoprotic acid
Hydrobromic Acid
HBr
strong monoprotic acid
Hydroiodic Acid
HI
strong monoprotic acid
Hydrocyanic Acid
HCN
Hydrosulfuric Acid
H2S
Oxoacids
Acids that contain hydrogen, oxygen, and another element (the central element)
Carbonic Acid
H2CO3
weak diprotic acid
Chloric Acid
HClO3
Nitric Acid
HNO3
strong monoprotic acid
Sulfuric Acid
H2SO4
strong diprotic acid
Soluble Cations
Group I cations
Li+, Na+, K+, Rb+, Cs+
Soluble Anions
nitrates: NO3(-)
acetates: CH3COO(-)
chlorates: ClO3(-)
Acetic Acid
vinegar or ethanoic acid
CH3COOH (weak monoprotic acid)
a.k.a. CH3CO2H or C2H4O2
Sodium hydroxide
lye or caustic soda
NaOH
strong base
Potassium hydroxide
caustic potash
KOH
strong base
Barium hydroxide
Ba(OH)2
strong base
Ammonia
NH3
weak base
Phosphoric Acid
H3PO4
weak triprotic acid
RICE
Reaction: write the equation
Initial number of moles of each reactant and product
Change: molar change for each reactant and product
End: add or subtract initial amounts to the changes
Aliquot
comprising a known fraction of a whole and constituting a sample
Titrant
known substance in a titration
Analyte
unknown substance in a titration
What is the difference between a complete ionic equation and a net ionic equation?
For a complete ionic equation, separate into ions: all (aq) ionic substances; all (aq) strong acids (i.e. HCl, HBr, HI, HNO3, HClO4 and H2SO4, which should be separated into H+ and HSO4–)
Cancel out any ions that appear the same on both sides of the complete ionic equation from in order to obtain the net-ionic equation.
