Hi, Can someone please explain how you would do the followingproblem: An analyti

Question

Hi,

Can someone please explain how you would do the followingproblem:

An analytical chemist added 1.2g of dimethylglyoxime (DMG) reagentto a 10-mL 0.01 nickel (II) solution resulting in the formation ofa rose red precipitate. Calculate the mass in grams of theprecipitate produced.

Molar masses (g mol-1): Ni =60, DMG=120

Thanks!

Explanation / Answer

moles of Ni =10*0.001*0.01=0.0001 moles of DMG = 1.2/120=0.01 so Nickel(II) is the Limiting reagent Reaction is: Ni2+ +2DMG-   --> Ni(DMG)2 0.0001 0.01          0   intially 0.0001-x 0.01-2x     x at timet 0            0.0098       0.0001   atequilibrium so 0.0001 moles of precipitate is formed Since molecular weight of Ni(DMG)2 (precipitate) = 60 +2*120=300 => 0.0001 moles of precipitate = 0.03 gm so 30mg of precipitate is formed

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