Question

What mass of precipitate will form if 1.50 L of highly concentrated Pb ( ClO 3 ) 2 is mixed with 0.700 L 0.280 M NaI ? Assume the reaction goes to completion

Write the balanced equation for the reaction of aqueous Pb(ClO3), with aqueous Nal. Include phases. chemical equation: Pb(ClO3)2 (aq) + 2 Nal(aq) = Pb),(s) + 2 Na(C103)(aq) What mass of precipitate will form if 1.50 L of highly concentrated Pb(ClO3), is mixed with 0.700 L 0.280 M Nal? Assume the reaction goes to completion. mass of precipitate: .130 g

Answer 1

Balance equation - Pb(C103) (aq) + 2 Na I lag) Pb I (s) Slim + 2Nacios (ap) moles of NaI = 0.700x0.280 Top = 0.196 moles in the one so, moles of Pb I Form = xmoles of NaI S = fx0.196 do (de 0.098 moes mans of Pb I = moras & molar may s 0.098 x 461,01 s 45018 g

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