Chem Unit Test 4 Flashcards
What factors determine which ionic compounds will be soluble in water?
The amount of charge on each ion and the size of the ion.
What trend does atomic and ionic radius follow?
To the left and down.
The greater the ionic radius…
The greater the solubility
The greater the charge on each ion…
The less soluble the compound will be.
Why is AgNO3 soluble when AgCl is not?
Both anions have a single charge but the NO3- ion is much larger than the Cl- ion. Therefore the attraction between Ag and NO3 is weaker and it is more soluble in water.
What kind of compound can you predict will form a soluble ionic compound?
Small charge and a large radius.
Which cations form soluble compounds with nearly all anions?
H+, NH4+, group 1 metals.
Which anions form soluble compounds with nearly all cations?
Nitrate and acetate.
Gases become more soluble in liquids with…
Lower temperatures and higher pressure
What does a net ionic equation do?
Omits the spectator ions and shows only the ions that react and the products of the reaction.
What is the rate of dissolving affected by?
Agitation, surface area and temperature
Solubility is affected by…
Pressure and temperature.
Add solvent to solute or vice versa?
ALWAYS ADD SOLUTE TO SOLVENT. Add solute to water like you oughter
Add acid to water
All aqueous thing dissociate unless they are…
A weak acid.
What is the net ionic equation for a strong acid+strong base?
H+(aq) + OH-(aq) -> H2O(l)
