Question

1. when the following solutions are mixed together, what precipitate (if any) will form?

a. feso₄(aq) + kcl(aq)
b. al(no₃)₃(aq) + ba(oh)₂(aq)
c. cacl₂(aq) + na₂so₄(aq)
d. k₂s(aq) + ni(no₃)₂(aq)

Explanation:

Step1: Analyze reaction a

For \(FeSO_{4}(aq)+KCl(aq)\), the possible products are \(FeCl_{2}\) and \(K_{2}SO_{4}\). According to solubility rules, \(FeCl_{2}\) is soluble (most chloride salts are soluble, and \(Fe^{2 +}\) does not form an insoluble chloride) and \(K_{2}SO_{4}\) is soluble (all potassium salts and most sulfate salts are soluble). So no precipitate forms.

Step2: Analyze reaction b

For \(Al(NO_{3})_{3}(aq)+Ba(OH)_{2}(aq)\), the possible products are \(Al(OH)_{3}\) and \(Ba(NO_{3})_{2}\). \(Ba(NO_{3})_{2}\) is soluble (all nitrate salts are soluble). \(Al(OH)_{3}\) is insoluble (hydroxide salts of \(Al^{3+}\) are insoluble). So \(Al(OH)_{3}\) precipitates.

Step3: Analyze reaction c

For \(CaCl_{2}(aq)+Na_{2}SO_{4}(aq)\), the possible products are \(CaSO_{4}\) and \(NaCl\). \(NaCl\) is soluble (all sodium salts and most chloride salts are soluble). \(CaSO_{4}\) is slightly soluble. In the context of precipitation reactions (where we consider significant precipitation), \(CaSO_{4}\) will precipitate.

Step4: Analyze reaction d

For \(K_{2}S(aq)+Ni(NO_{3})_{2}(aq)\), the possible products are \(KNO_{3}\) and \(NiS\). \(KNO_{3}\) is soluble (all potassium and nitrate salts are soluble). \(NiS\) is insoluble (sulfide salts of transition metals like \(Ni^{2+}\) are insoluble). So \(NiS\) precipitates.

Answer:

a. No precipitate forms.
b. \(Al(OH)_{3}\) precipitates.
c. \(CaSO_{4}\) precipitates.
d. \(NiS\) precipitates.