1) A sample of a complex salt, with ideal composition Ni(NH3)6(NO3)2, was analyzed for nickel by dissolution in slightly acidic solution and precipitation as the dimethylglyoximate, Ni(DMG)2.
A crucible of mass 14.1663 g was used to filter off the precipitate. The dried crucible and precipitate had a combined mass of 14.2633 g.
Theoretically calculated mass of Ni(NH3)6(NO3) = 0.0954g
-If the actual mass of the original sample in this experiment was 0.0836 g (instead of the theoretically calculated mass) -- indicating that the original Ni(NH3)6(NO3)2 complex had lost some ammonia -- what would be the corresponding value of n in the revised formula Ni(NH3)n(NO3)2.
-Calculate the percent loss of ammonia which accounts for the difference in the theoretical and actual mass of the initial sample.
2 ) A 6.80-g sample containing only Mn2(SO4)3(s) and Al2(SO4)3(s) is dissolved in aqueous solution. The metal ions are precipitated as hydroxides, which are pyrolyzed in air to produce 2.39 g of a mixture of Mn2O3(s) and Al2O3(s).
Molar mass of Mn2(SO4)3 is 398.1 g/mol.
Molar mass of Al2(SO4)3 is 342.1527 g/mol
What was the percent Mn in the original sample?
What was the percent Al in the original sample?