Table of Reactions for Experiment 7: (1) Na 3 PO 4 + AgNO 3 Molecular: Na 3 PO 4
ID: 505417 • Letter: T
Question
Table of Reactions for Experiment 7:
(1) Na3PO4 + AgNO3
Molecular: Na3PO4 (aq.) + 3 AgNO3 (aq.) ® 3 NaNO3 (aq.) + Ag3PO4 (s)
Total Ionic: 3 Na+1 (aq.) + PO4-3 (aq.) + 3 Ag+1 (aq.) + 3 NO3-1 (aq.) ® 3 Na+1 (aq.) + 3 NO3-1 (aq.) + Ag3PO4 (s)
Net Ionic: 3 Ag+1 (aq.) + PO4-3 (aq.) ® Ag3PO4 (s)
(2) Na3PO4 + Cr(NO3)3
Molecular: Na3PO4 (aq.) + Cr(NO3)3 (aq.) ® 3 NaNO3 (aq.) + CrPO4 (s)
Total Ionic: 3 Na+1 (aq.) + PO4-3 (aq.) + Cr+3 (aq.) + 3 NO3-1 (aq.) ® 3 Na+1 (aq.) + 3 NO3-1 (aq.) + CrPO4 (s)
Net Ionic: PO4-3 (aq.) + Cr+3 (aq.) ® CrPO4 (s)
(3) Na3PO4 + Pb(NO3)2
Molecular: 2 Na3PO4 (aq.) + 3 Pb(NO3)2 (aq.) ® 6 NaNO3 (aq.) + Pb3(PO4)2 (s)
Total Ionic: 6 Na+1 (aq.) + 2 PO4-3 (aq.) + 3 Pb+2 (aq.) + 6 NO3-1 (aq.) ® 6 Na+1 (aq.) + 6 NO3-1 (aq.) + Pb3(PO4)2 (s)
Net Ionic: 2 PO4-3 (aq.) + 3 Pb+2 (aq.) ® Pb3(PO4)2 (s)
(4) NaI + AgNO3
Molecular: NaI (aq.) + AgNO3 (aq.) ® Na+1 (aq.) + I-1 (aq.) + AgI (s)
Total Ionic: Na+1 (aq.) + I-1 (aq.) + Ag+1(aq.) + NO3-1 (aq.) ® Na+1 (aq.) + NO3-1 (aq.) + AgI (s)
Net Ionic: I-1 (aq.) + Ag+1(aq.) ® AgI (s)
(5) NaI + Cr(NO3)3
Molecular: 3 NaI (aq.) + Cr(NO3)3 (aq.) ® 3 NaNO3 (aq.) + CrI3 (aq.)
Total Ionic: 3 Na+1 (aq.) +3 I-1 (aq.) + Cr+3 (aq.) + 3 NO3-1 (aq.) ® 3 Na+1 (aq.) +3 I-1 (aq.) + Cr+3 (aq.) + 3 NO3-1 (aq.)
Not net ionic because all ions are soluble
(6) NaI + Pb(NO3)2
Molecular: 2 NaI (aq.) + Pb(NO3)2 (aq.) ® 2 NaNO3 (aq.) + PbI2 (s)
Total Ionic: 2 Na+1 (aq.) +2 I-1 (aq.) + Pb+2 (aq.) + 2 NO3-1 (aq.) ® 2 Na+1 (aq.) + 2 NO3-1 (aq.) + PbI2 (s)
Net Ionic: 2 I-1 (aq.) + Pb+2 (aq.) ® PbI2 (s)
(7) Na2Cr2O4 + AgNO3
Molecular: Na2Cr2O4 (aq.) + 2AgNO3 (aq). ® 2 NaNO3 (aq). + Ag2Cr2O4 (s)
Total Ionic: 2 Na+1 (aq.) + Cr2O4-2 (aq.) + 2 Ag+1 (aq.) + 2 NO3-1 (aq.) ® 2 Na+1 (aq.) +2 NO3-1 (aq.) + Ag2Cr2O4 (s)
Net Ionic: Cr2O4-2 (aq.) + 2 Ag+1 (aq.) ® Ag2Cr2O4 (s)
(8) Na2Cr2O4 + Cr(NO3)3
Molecular: 3 Na2Cr2O4 (aq.)+ 2 Cr(NO3)3 (aq.) ® 6 NaNO3 (aq.) + Cr2(Cr2O4)3 (s)
Total Ionic: 6 Na+1 (aq.) + 3 Cr2O4-2 (aq.) + 2 Cr+3 (aq.) + 6 NO3-1 (aq.) ® 6 Na+1 (aq.) + 6 NO3-1 (aq.) + Cr2(Cr2O4)3 (s)
Net Ionic: 3 Cr2O4-2 (aq.) + 2 Cr+3 (aq.) ® Cr2(Cr2O4)3 (s)
EXPERIMENT 7: CHEMICAL REACTIONS;
QUESTION (1) WHICH OF THE REACTION IN PART 1 ABOVE MAY BE CALLED PRICIPITATION REACTIONS? GIVE REASONS FOR CALLING THEM SUCH.
(2) WHICH OF THE PRICIPITATION IN PART 1 MAY BE CALLED A DECOMPOSITION REACTION? GIVE REASONS FOR CALLING THE REACTION SUCH.
(3). SUPPOSE YOU MIX A SOLUTION OF SODIUM NITRATE AND A SOLUTION OF BARIUM CHLORIDE TOGETHER, DO YOU EXPECT A PRICIPITATE TO FORM? EXPLAIN.
Explanation / Answer
1) All the reaction except reaction 5 are called precipitation reactions because one of the products of the reaction is insoluble in the reaction medium (water) and separates out from the medium in the form of a solid. Since all the reaction except 5 produce a solid product, all these reactions are precipitation reactions.
2) The precipitation reactions cannot be called as decomposition reactions. However, reaction 5 produces no solid product and all the ions are soluble in water. Therefore, reaction 5 is a decomposition reaction since we are breaking up the electrolyte into the constituent ions.
3) A mixture of sodium nitrate and barium chloride will not produce a precipitate. The reason is there will be simply a displacement of cations and anions producing barium nitrate and sodium chloride. All sodium and nitrate salts are water soluble, hence no precipitate will form.
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