1. Lead hydrogen arsenate, PbHAsO4, is an insoluble insecticide used against thepotato beetle. PbHAsO4 is produced industrially by reacting weak acidH3ASO4 with aqueous Pb(NO3)2 as shown in the following (unbalanced) molecularequation:H3ASO4(aq) + Pb(NO3)2(aq)PbHAsO4(s) + HNO3(aq)--->Which of the following equations represents the balanced net ionic equation for thisreaction?O H;ASO4(aq) + Pb(NO3)2(aq)PBHASO4(s) + 2 HNO3(aq)--->O H3ASO4(aq) + Pb2*(aq)-PbHAsOg(s) + 2 H*(aq)--->O H*(aq) + AsO4³-(aq) + Pb2*(aq) --PBHASO4(s)->O HASO4 (aq) + Pb2*(aq)PbHAsO4(s)--->

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1. Lead hydrogen arsenate, PbHAsO4, is an insoluble insecticide used against the potato beetle. PbHAsO4 is produced industrially by reacting weak acid H3ASO4 with aqueous Pb(NO3)2 as shown in the following (unbalanced) molecular equation: H3AsOq(aq) + Pb(NO3)2(aq) ---> PbHAsO4(s) + HNO3(aq) Which of the following equations represents the balanced net ionic equation for this reaction? O H;ASO4(aq) + Pb(NO3)2(aq) - PbHAsO4(s) + 2 HNO3(aq) ---> O H3AsOg(aq) + Pb2*(aq) ---> PBHASO4(s) + 2 H*(aq) O H (aq) + AsO43-(aq) + Pb2*(aq) -- PbHAsO4(s) ---> O HASO4 (aq) + Pb2*(aq) - PbHAsO4(s) --->

1. Lead hydrogen arsenate, PbHAsO4, is an insoluble insecticide used against the potato beetle. PbHAsO4 is produced industrially by reacting weak acid H3ASO4 with aqueous Pb(NO3)2 as shown in the following (unbalanced) molecular equation: H3AsOq(aq) + Pb(NO3)2(aq) ---> PbHAsO4(s) + HNO3(aq) Which of the following equations represents the balanced net ionic equation for this reaction? O H;ASO4(aq) + Pb(NO3)2(aq) - PbHAsO4(s) + 2 HNO3(aq) ---> O H3AsOg(aq) + Pb2(aq) ---> PBHASO4(s) + 2 H(aq) O H (aq) + AsO43-(aq) + Pb2(aq) -- PbHAsO4(s) ---> O HASO4 (aq) + Pb2(aq) - PbHAsO4(s) --->

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter4: Reactions In Aqueous Solution

Section: Chapter Questions

Problem 62QAP: Ten mL of concentrated H3PO4 (91.7% by mass, d=1.69g/mL) was accidentally poured into a beaker...

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