Which of the following pairs of aqueous solutions ...

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Which of the following pairs of aqueous solutions will form a precipitate when mixed? A. Sr(C2H3O2)2 + Na2SO4B. (NH4)2SO4 + KClC. KNO3 + LiOHD. KOH + Li2S

Jules Bruno · Accepted Answer

We are asked to identify the pairs of aqueous solutions that will form a precipitate when mixed. We will refer to the solubility rules in order to determine if an insoluble product is formed or not.Solubility Rules:•Soluble Ionic Compounds:▪ Group 1A ions (Li+, Na+, K+, etc.) and Ammonium ion (NH4+) are soluble▪ Nitrates (NO3-), Acetates (CH3COO- or C2H3O2-), and most Perchlorates (ClO4-) are soluble▪ Cl-, Br-, and I- are soluble except when paired with Ag+, Pb2+, Cu+, Hg22+▪ Sulfates (SO42-) are soluble except those of Ca2+, Sr2+, Ba2+, Ag+, and Pb2+• Insoluble Ionic Compounds:[readmore]▪ Hydroxides (OH-) and Sulfides (S2-) are insoluble except when with Group 1A ions (Li+, Na+, K+, etc.) and ammonium ion (NH4+) and Ca2+, Sr2+, Ba2+▪ Carbonates (CO32-) and Phosphates (PO43-) are insoluble except when with Group 1A ions (Li+, Na+, K+, etc.) and ammonium ion (NH4+)A. Sr(C2H3O2)2 + Na2SO4Reactants:• Sr(C2H3O2)2(aq)▪ strontium → group 2A → +2 charge → Sr2+ ▪ acetate → polyatomic ion → -1 charge → C2H3O2-• Na2SO4▪ sodium → group 1A → +1 charge → Na+ ▪ sulfate → polyatomic ion → -2 charge → SO42-Reaction:• double displacement reaction → the positive ions (cations) and the negative ions (anions) of the two reactants will swap or switch places*criss cross the charges of the cation and anion and that would be the subscript of each ionProducts:• Sr2+ + SO42- → SrSO­4Sulfates (SO42-) are soluble except those of Ca2+, Sr2+, Ba2+, Ag+, and Pb2+SrSO­4(s) → insoluble• Na+ + C2H3O2- →  NaC2H3O2Acetates (CH3COO- or C2H3O2-) are solubleNaC2H3O2(aq) → solubleOverall Reaction:      Sr(C2H3O2)2(aq) + Na2SO4(aq) → SrSO4(s) + 2 NaC2H3O2(aq)Precipitate formed: SrSO4(s)B. (NH4)2SO4 + KClReactants:• (NH4)2SO4(aq)▪ ammonium → polyatomic ion → +1 charge → NH4+▪ sulfate → polyatomic ion → -2 charge → SO42-• KCl▪ potassium → group 1A → +1 charge → K+ ▪ chloride → group 7A → -1 charge → Cl-Products:• NH4+ + Cl- → NH­4ClCl- are soluble except when paired with Ag+, Pb2+, Cu+, Hg22+NH­4Cl(aq) → soluble• K+ + SO42- →  K2SO4Sulfates (SO42-) are soluble except those of Ca2+, Sr2+, Ba2+, Ag+, and Pb2+K2SO­4(aq) → solubleNo precipitate formed C. KNO3 + LiOHReactants:• KNO3(aq)▪ potassium → group 1A → +1 charge → K+ ▪ nitrate → polyatomic ion → -1 charge → NO3-• LiOH(aq)▪ lithium → group 1A → +1 charge → Li+ ▪ hydroxide → polyatomic ion → -1 charge → OH-Products:• K+ + OH- → KOHHydroxides (OH-) insoluble except when with Group 1A ions (Li+, Na+, K+, etc.) and ammonium ion (NH4+) and Ca2+, Sr2+, Ba2+KOH(aq) → soluble• Li+ + NO3- →  LiNO3Nitrates (NO3-) are solubleLiNO­3(aq) → solubleNo precipitate formed D. KOH + Li2SReactants:• KOH(aq)▪ potassium → group 1A → +1 charge → K+ ▪ hydroxide → polyatomic ion → -1 charge → OH-• Li2S(aq)▪ lithium → group 1A → +1 charge → Li+ ▪ sulfide → group 6A → -2 charge → S2-Products:• K+ + S2- → K2SSulfides (S2-) insoluble except when with Group 1A ions (Li+, Na+, K+, etc.) and ammonium ion (NH4+) and Ca2+, Sr2+, Ba2+K2S(aq) → soluble• Li+ + OH- →  LiOHHydroxides (OH-) insoluble except when with Group 1A ions (Li+, Na+, K+, etc.) and ammonium ion (NH4+) and Ca2+, Sr2+, Ba2+KOH(aq) → solubleNo precipitate formed Only A. Sr(C2H3O2)2 + Na2SO4 will form a precipitate when mixed.

Problem: Which of the following pairs of aqueous solutions will form a precipitate when mixed? A. Sr(C2H3O2)2 + Na2SO4B. (NH4)2SO4 + KClC. KNO3 + LiOHD. KOH + Li2S

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Problem: Which of the following pairs of aqueous solutions will form a precipitate when mixed? A. Sr(C2H3O2)2 + Na2SO4B. (NH4)2SO4 + KClC. KNO3 + LiOHD. KOH + Li2S

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