A 0.573 M Pb(NO3)2(aq) solution has a density of 1.17 g/mL. Calculate the % mass of...

A 0.573 M Pb(NO₃)_2(aq) solution has a density of 1.17 g/mL. Calculate the % mass of this solution to three significant figures. The molar mass of lead(II) nitrate is 331.2 g/mole.

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queen_honey_blossom answered 2 years ago

Reaction is: Pb(NO3)2(aq) + 2KI(aq) ---> PbI2(s) + 2KNO3(aq) 2.0 ml of 0.250M Pb(NO3)2 and 7.0...

Reaction is: Pb(NO3)2(aq) + 2KI(aq) ---> PbI2(s) + 2KNO3(aq) 2.0 ml of 0.250M Pb(NO3)2 and 7.0 ml of 0.250M KI A) In your experiment, one of the reagents was limiting and the other was in excess. Therefore after the lead(II)iodide precipitated from the solution, there were spectator ions left in the solution, and also the unreacted excess reagent. Assuming complete precipitation of lead (II) iodide, calculate the concentrations of each type of ion (Pb2+, K+, NO3-, I-) present in the...

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1. a.) A student mixes 47.0 mL of 3.30 M Pb(NO3)2(aq) with 20.0 mL of 0.00183...

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