All compounds containing Cl^+,K^+, Na^+, NH_4 NO_3CH_2COO^- (ClO)_3are soluble i

Question

All compounds containing Cl^+,K^+, Na^+, NH_4 NO_3CH_2COO^- (ClO)_3are soluble in water. Most of the halide ions (X): Cl^-. Br^-. l^-, are soluble except with Ag^+ Hg_2^-2,. and Pb'^2+ Most of the SO_4^2- are soluble except with Ca^2+ Sr^2+. Ba^2+ and Pb^2+ Most of CO_3^-2', PO_4^-3', and CrO_4^-2 are insoluble except rule 1; Most of S^2- and OH^- are Insoluble except rule 1 and with Ca^2-, Sr^- and Ba^2- are insoluble m water Write a balanced chemical equation for each of the six compounds to be tested (NaCI, NaBr. Nal, Na_2CO_2, Na_2CO_2. Na_3PO_4). with the reagents being used Use the solubility rules to help you determine the products and if a reaction will occur, if no reaction, then indicate "no rxn" at the end of your balanced equation with AgNO_3 with BaCl_2

Explanation / Answer

The only possible net ionic reactions (by applying the solubility rules) are

Ag+   + Cl- (or Br-, I-) = AgCl (pp)

2Ag+   + CO32- = Ag2CO3 (pp)

3Ag+   + PO43- = Ag3PO4 (pp)

The only possible net ionic reactions (by applying the solubility rules) are

Ba2+ + CO32- = BaCO3 (pp)

Ba2+ + SO42- = CaSO4 (pp)

Ba2+ + PO43- =Ba3(PO4)2 (pp)

I see for the first time a question asking to write balanced equations for “no reaction”.

Write the equations… as required!

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