1Write balanced chemical equations for each of the following reactionsDon’t forget to indicate phaseIf a precipitate forms, circle itIf all “products” are predicted to be soluble, indicate that there is no reaction by writing “NR”aAqueous sodium iodide is mixed with aqueous silver nitratebAqueous potassium hydroxide is mixed with lead(II) nitratecAqueous magnesium nitrate is mixed with aqueous sodium phosphatedAqueous barium nitrate is mixed with sulfuric acideAqueous aluminum nitrate is mixed with aqueous ammonium sulfidefAqueous lead(II) nitrate is mixed with sodium sulfate.
You get a definitive reaction if a portion of the reactants leave the solution, either by becoming a gas or by becoming a precipitateThat being said: a) Silver iodide precipitates so there is a reaction b) lead hydroxide will tend to precipitate so there is a reaction c) Magnesium phosphate will tend to precipitate so there is a reactiond) Barium sulphate is not very soluble so there is a reaction e) Aluminum sulphide will tend to precipitate so there is a reaction f) Lead sulphate should tend to precipitate so there is a reaction You do the balanced equations.
