Solubility & Precipitation
Which of the following compounds is insoluble in water and would form a precipitate?
K2SO4
PbBr2
LiNO3
PbBr2
Write the net ionic equation for the reaction between HCl and NaOH
H+ (aq) + OH- (aq) -> H2O (l)
What is the molarity of a solution made by dissolving 2.0 moles of NaCl in enough water to make 4.0 L of solution.
0.5 M
Which of the following is strong electrolyte?
- CH3OH
- KNO3
- HF
- C12H22O11
KNO3
A student mixes a solution of sodium chloride with a solution of potassium nitrate. based on the solubility rules, what is the most likely outcome.
No precipitate forms
When aqueous BaCl2, is mixed with aqueous Na2SO4, a white precipitate forms. What are the spectator ions in this reaction?
Na+ and Cl-
How many grams of NaOH are required to prepare 500 mL of a 0.20 M solution?
4.0 grams
How many moles of total ion are present in 1 L of 0.5 M CaCl2?
1.5 moles
Which of the following compounds is insoluble in water:
- Na2CO3
- AgNO3
- BaSO4
- NH4Cl
BaSO4
What is the net ionic equation for the reaction between aqueous calcium chloride and aqueous sodium carbonate?
Ca2+ (aq) + CO2- 3 (aq) -> CaCO3 (s)
You need to prepare 100 mL of 0.5 M HCL from a 12.0 M NaCl, how many moles of AgCl precipitate are formed?
4.17 mL
What is the concentration of hydroxide ions in a 0.05 M Sr(OH)2 solution?
0.10 M
You have a solution containing Ag+ Pb2+ Na+ ions. Which single reagent could you add to precipitate two of these ions simultaneously.
Cl- to form AgCl and PbCl2
Nickel (II) chloride is added to sodium phosphate. Write the net ionic equation.
3Ni2+ (aq) + 2PO3- 4 (aq) -> Ni3(PO4)2 (s)
If 25.0 mL of 0.10 M AgNO3 is mixed with 15.0 mL of 0.20 M NaCl, how many moles of AgCl precipitate are formed?
0.0025 moles
A solution of a weak acid and a solution of a strong acid have the same molar concentration. Which solution has a higher electrical conductivity?
The strong acid, they produce more ions
Identify which of these combinations will NOT produce a precipitate:
- Pb(NO3)2 + Na2SO4
- AgNO3 + KCl
- Na2CO3 + CaCl2
- K2SO4 + NaNO3
K2SO4 + NaNO3
Write the net ionic equation for the reaction between weak acid nitrous acid (HNO2) and KOH.
HNO2 (aq) + OH- (aq) -> NO-2 (aq) + H2O (l)
A 50.0 mL sample of unknown HCl is titrated with 0.150 M NaOH. If 32.5 mL of NaOH is required to reach the equivalence point, what is the molarity of the HCl?
0.0975 M
What is the final concentration of nitrate ions when 50.0 mL of 0.10 M KNO3 is mixed with 100.0 mL of 0.20 M Ca(NO3)2?
0.30 M