Part I Observations: CationInitial xs OH- NH40H xs NH40H Precipitate Observati o

Question

Part I Observations: CationInitial xs OH- NH40H xs NH40H Precipitate Observati on Mg2+ Clear liquid Clear Slight liquid Clear cloudynes liquid Faint cloudynes s with faint blue tinted liquid No Ni2+ Tint of green liquid Milky light blue liquid, blue liquid, transparan blue tinted NaOH and with solid with solidt liquid liquid particles particles Milky light Blue/green Vibrant Yes, with xs NaOH Tint of Transpara Transpara Light purple, nt, liquid Cr3+ Light Cloudy aqua gree liquid with No nt, bluelnt, bluelgreen green green milky liquid, flaky tiny clear particles particles Clearliquidlight milky Clear liquid Clear liquid Zn2+ Clear Flaky clear Clear particles, liquid No liquid Ag+ Clear liquid Milky MilkyNon- Faint Yes, with brown solid particlesparticles brown with brown with transparan cloudy NaOH and solid brownbrown white liquid liquid t Milky/tinted xs NaOH Clear withBold white Yes, with solid white liquid with NH40H particles white film settled at floating on bottom top Pb2 Clear liquid Bold/Clear cloudy liquid white liquid

Explanation / Answer

Part I

For all the reactions with no precipitation there will be no net ionic balanced equations, because in solution they will dissociate as ions. The ions on both sides will cancel and the net ionic balanced equation will be zero. For the ions which formed precipitates are: Ni2+, Ag+ and Pb2+.

Ni2+ with OH-:

Ni2+ (aq) + 2NaOH (aq) ----> Ni(OH)2 (s) + 2Na+ (aq)

Ionic equation:

Ni2+ (aq) + 2Na+ (aq) + 2OH- (aq) --------> Ni(OH)2 (s) + 2Na+ (aq)

Net ionic balanced equation:

Ni2+ (aq) + 2OH- (aq) -----> Ni(OH)2 (s)

Ni(OH)2 with excess of OH-

Ni(OH)2 (s) + 2NaOH (aq) -------> NiO(OH) (s) + H2O (l) + 2Na+ (aq)

Ionic equation:

Ni(OH)2 (s) + 2Na+ (aq) + 2OH- (aq) -------> NiO(OH) (s) + H2O (l) + 2Na+ (aq)

Net ionic balanced equation:

Ni(OH)2 (s) + 2OH- (aq) -------> NiO(OH) (s) + H2O (l)

Ag+ with NaOH:

Ag+ (aq) + NaOH (aq) ----> AgOH (s) + Na+ (aq)

Ionic equation:

Ag+ (aq) + Na+ (aq) + OH- (aq) --------> AgOH (s) + Na+ (aq)

Net ionic balanced equation:

Ag+ (aq) + OH- (aq) -----> AgOH (s)

AgOH with excess of OH-

AgOH (s) + NaOH (aq) -------> Ag2O (s) + H2O (l) + Na+ (aq)

Ionic equation:

AgOH (s) + Na+ (aq) + OH- (aq) -------> Ag2O (s) + H2O (l) + Na+ (aq)

Net ionic balanced equation:

AgOH (s) + OH- (aq) -------> Ag2O (s) + H2O (l)

Pb2+ with NH4OH:

Pb2+ (aq) + 2NH4OH (aq) ------> Pb(OH)2 (s) + 2NH4+ (aq)

Ionic equation:

Pb2+ (aq) + 2NH4+ (aq) + 2OH- (aq) --------> Pb(OH)2 (s) + 2NH4+ (aq)

Net ionic balanced equation:

Pb2+ (aq) + 2OH- (aq) --------> Pb(OH)2 (s)

Part (III)

only Cl- and I- are making precipitates with Ag+ ion.

Ag+ (aq) + Cl-(aq) ----> AgCl (s)

Ag+ (aq) + I-(aq) ----> AgI (s)

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