WorksheetsNIE Level 2: Spec. ions & NIE's
Total questions: 21
Worksheet time: 24mins
What precipitate forms when you mix lead(II) nitrate, Pb(NO3)2 with sodium chloride, NaCl?
sodium nitrate, NaNO3
lead(II) chloride, PbCl2
sodium lead, NaPb
chloride nitrate, ClNO3
CuCl2(aq) + NaOH(aq) → Cu(OH)2(s) + NaCl(aq)
What is the result of the reaction between solutions of potassium bromide, KBr and ammonium sulfide, (NH4)2S?
potassium sulfide, K2S precipitates
ammonium bromide, NH4Br precipitates
potassium ammonium, KNH4 precipitates
no precipitate is formed
What would happen if solutions of sodium nitrate, NaNO3 and ammonium chloride, NH4Cl were mixed?
A precipitate of sodium chloride, NaCl would form.
A precipitate of ammonium chloride, NH4Cl would form.
Neither sodium nitrate, NaNO3 nor ammonium chloride, NH4Cl would dissolve.
Nothing would happen.
K2SO4(aq) + Ba(C2H3O2)2(aq) -> BaSO4(s) + 2 KC2H3O2(aq)
Which is the correct net ionic equation for the reaction of AgNO3(aq) and CaCl2(aq)?
Ca2+(aq) + 2Cl- (aq) → CaCl(s)
Ag+(aq) + Cl- (aq) → AgCl(s)
Ag + Cl → AgCl
Ag+ + Ca2+ →Ag2Ca (s)
CuCl2(aq) + NaOH(aq) → Cu(OH)2(s) + NaCl(aq)
In this equation,
CuCl2(aq)+ NaOH(aq) → Cu(OH)2 + NaCl
Which product is insoluble?
copper(II) hydroxide
sodium chloride
sodium hydroxide
copper(II) chloride
Which of the following shows the correct net ionic equation for the reaction of the two solutions: Ba(MnO4)2(aq) + (NH4)2SO4(aq)?
Ba2+ + SO42- --> BaSO4
2NH4+ + 2MnO4- --> 2NH4MnO4
Ba + MnO4- --> Ba(MnO4)2
2MnO4- + SO42- --> BaSO4
What is the correct complete ionic equation for the reaction between AgNO3(aq) and KClaq
Ag+ + NO3- + K+ + Cl-→ K+ + NO3- + AgCl(s)
Ag- + NO3+ + K- + Cl+→ K- + NO3+ + AgCl(s)
Ag+ + NO3- + K+ + Cl-→ KNO3(s) + Ag++ Cl-
No reaction
Select the precipitation reaction below
2 Mg(s) + O2(g) -> 2 MgO(s)
Pb2+(aq) + CrO42-(aq) -> PbCrO4(s)
SO3(g) + 2 H2O(l) -> H3O+(aq) + HSO4-(aq)
2 H2O(g) -> 2 H2(g) + O2(g)
Ag+(aq) + 2 NH3(aq) -> [Ag(NH3)2]+(aq)
Addition of sulfurous acid, H2SO3 to barium hydroxide, Ba(OH)2 results in the formation of a precipitate. The net ionic equation for this reaction is
2 H+(aq) + 2 OH-(aq) <-> 2 H2O(l)
H2SO3(aq) + Ba2+(aq) + 2 OH-(aq) <-> BaSO3(s) + 2 H2O(l)
2 H+(aq) + SO32-(aq) + Ba2+(aq) + 2 OH-(aq) <-> BaSO3(s) + 2 H2O(l)
H2SO3(aq) + Ba2+(aq) + 2 OH-(aq) <-> Ba2+(aq) + SO32-(aq) + 2 H2O(l)
H2SO3(aq) + Ba(OH)2(aq) <-> BaSO3(s) + 2 H2O(l)
Ag+(aq) + Cl-(aq) ⇄ AgCl(s)
A student mixes dilute AgNO3(aq) with excess NaCl(aq), as represented by the net ionic equation above. Which of the diagrams below best represents the ions that are present in significant concentrations in the solution?
The diagrams here represent solutes present in two different dilute aqueous solutions before they were mixed. Water molecules are not shown. When the solutions were combined, a precipitation reaction took place. Which of the diagrams below is the best particle representation of the mixture after the precipitation reaction occurred?
M+ is an unknown metal cation with a +1 charge. A student dissolves the chloride of the unknown metal, MCl, in enough water to make 100.0 ml of solution. The student then mixes the solution with excess AgNO3 solution, causing AgCl to precipitate. The student collects the precipitate by filtration, dries it, and records the data shown below. (The molar mass of AgCl is 143 g/mol.)
Mass of unknown chloride, MCl = 0.74 g
Mass of filter paper = 0.80 g
Mass of filter paper plus AgCl precipitate = 2.23 g
During the course of the experiment, which of the following happens to the NO3- ions?
They are oxidized by Cl- ions.
They are reduced to NO2- ions.
They are decomposed by reacting with M+ ions.
They remain dissolved in the filtrate solution.
M+ is an unknown metal cation with a +1 charge. A student dissolves the chloride of the unknown metal, MCl, in enough water to make 100.0 mL of solution. The student then mixes the solution with excess AgNO3 solution, causing AgCl to precipitate. The student collects the precipitate by filtration, dries it, and records the data shown below. (The molar mass of AgCl is 143 g/mol.)
Mass of unknown chloride, MCl = 0.74 g
Mass of filter paper = 0.80 g
Mass of filter paper plus AgCl precipitate = 2.23 g
Which of the following diagrams best represents the AgNO3 solution before the reaction occurs?
Note: water molecules are represented by the symbol.
Which of the following is the net ionic equation for the reaction between aqueous sodium fluoride, NaF and hydrochloric acid, HCl?
NaF(aq) + HCl(aq) →NaCl(aq) + HF(aq)
Na+(aq) + F-(aq) + H+(aq) + Cl-(aq) →Na+(aq) + Cl-(aq) + HF(aq)
Na+(aq) + Cl-(aq) →NaCl(aq)
F-(aq) + H+(aq) →HF(aq)
Equal volumes of 0.2 M solutions of lead(II) nitrate, Pb(NO3)2 and potassium bromide, Kbr are combined to form lead(II) bromide, PbBr2 as a yellow precipitate. Which of the following is the correct net ionic equations for the reaction?
Pb2+(aq) + 2Br-(aq) →PbBr2(s)
K+(aq) + NO3-(aq)→KNO3(aq)
Pb2+(aq) + 2 NO3-(aq) + 2 Br-(aq)→2 K+(aq) + 2 NO3-(aq) + PbBr2(s)
Pb(NO3)2(aq) + 2 KBr(aq) →PrBr2(s) + 2 KNO3(aq)
The reaction between aqueous strontium chloride (SrCl2) and aqueous potassium sulfate (K2SO4) forms a precipitate of strontium sulfate (SrSO4). Which of the following represents the net ionic equation for the reaction?
Cl-(aq) + K+(aq) --> KCl(aq)
Sr2+(aq) + SO42-(aq) --> SrSO4(s)
Sr2+(aq) + 2 Cl-(aq) + SO42-(aq) + 2 K+(aq) --> SrSO4(s) + 2 Cl-(aq) + 2 K+(aq)
SrCl2(aq) + K2SO4(aq) --> SrSO4(s) + 2 KCl(aq)
