The total should equal when you add all oxidation numbers: Pb + (-2) = 0 ----> Pb = +2. Therefore oxidation number of Pb in PbSO 4 ⦠Identify which reactants are being oxidized (the oxidation number increases when it reacts) and which are being reduced (the oxidation number goes down). PbSO4 --> Pb2+ + SO4 2- (A net dissociation reaction of the salt) SO4 has an oxidation number of -2. PbSO 4 salt does not have an overall charge. ... Pb PbO2 PbSO4 H2O H2SO4. In order to make the compound neutral, Pb must be +2. Therefore oxidation number of Pb is +2. Sulfide ion is at -2 oxidation state. It is suggested that a precipitation mechanism to form PbSO 4 occurs under some conditions prior to the solid state ⦠Check to see if the oxidation numbers show oxidation or reduction. Could you tell me how you went about getting the oxidation number for Pb in PbSO4? So, Pb is at +2 oxidation state. what is the oxidation number of pb in pbso4. Oxidation number of O=-2. Therefore x+6-8=0. Pb. The rates of PbSO4 formation on the Pbâ0.08 mass% CaâSn alloys, which are the choice materials for grids in the valve-regulated leadâacid battery (VRLA), were inhibited by the presence of Sn. To neutral that -2 charge, +2 charge should be there and it is given by Pb 2+ ion. How to calculate oxidation number of Pb in PbSO4?And Explain? Also, the answer would not be +10 if what you had said was correct (about the sulfur ion). Expert Answer: Let the oxidation number of Pb=x. You are correct that oxidation is the loss of electrons and reduction is the gaining of electrons. H2O2 + PbS --> PbSO4 + H2O. H in H2 : 0. It can only be +2, or +4. Oxidation number of Pb is +2 But Sulfate ion has -2 charge. pb +2 s-2 + h +1 2 o-1 2 â pb +2 s +6 o-2 4 + h +1 2 o-2 b) Identify and write out all redox couples in reaction. Identify the products and the reactants, and then their oxidation numbers. Pb in PbSO4 : +2. +1 +3 0-1 +2 +1. Figuring out why these numbers are the way they are takes a fair amount of work. The system is compared with measurements on Pb(Hg) in H 2 SO 4 and with Pb(Hg), Hg, solid Pb in HClO 4 solution. If you consider oxidation as the loss of electrons and gain of oxidation number, and reduction as the gain of electrons and decrease in oxidation number, the oxidation states are as follows: Pb : 0 (Elementary state) H in H2SO4 : +2. I went by the rule of the most electronegative atom getting their typical oxidation state (so O was assigned -2 (total -8)...then S was assigned -2...and finally Pb was given +10 to balance the molecule). Sum of all oxidation number =0. Lead, being a metal, has very set oxidation numbers. SO4 has charge of -2. Oxidation = number goes down Reduction = number goes up. What is the oxidation number of phosphorous in the H3PO2 molecule? Asked by | 25th Mar, 2009, 06:56: PM. Oxidation number of S=+6. 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