Figuring out why these numbers are the way they are takes a fair amount of work. Asked by | 25th Mar, 2009, 06:56: PM. Expert Answer: Let the oxidation number of Pb=x. Oxidation = number goes down Reduction = number goes up. The anodic oxidation of solid Pb in H 2 SO 4 to form PbSO 4 has been investigated by rotating disc, potentiostatic pulse and ac impedance measurements. Therefore x+6-8=0. So, Pb is at +2 oxidation state. PbSO 4 salt does not have an overall charge. Pb. The rates of PbSO4 formation on the Pb–0.08 mass% Ca–Sn alloys, which are the choice materials for grids in the valve-regulated lead–acid battery (VRLA), were inhibited by the presence of Sn. Sulfide ion is at -2 oxidation state. Oxidation number of Pb is +2 You are correct that oxidation is the loss of electrons and reduction is the gaining of electrons. Identify which reactants are being oxidized (the oxidation number increases when it reacts) and which are being reduced (the oxidation number goes down). In order to make the compound neutral, Pb must be +2. what is the oxidation number of pb in pbso4. 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? Oxidation number of S=+6. Also, the answer would not be +10 if what you had said was correct (about the sulfur ion). It can only be +2, or +4. 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). Therefore oxidation number of Pb in PbSO 4 … 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. Identify the substance oxidised, reduced, oxidising agent and reducing agent for each of the following reactions: Pb(s) + PbO 2 (s) + 2H 2 SO 4 (aq) → 2PbSO 4 (s) + 2H 2 O(l) ... Pb PbO2 PbSO4 H2O H2SO4. The total should equal when you add all oxidation numbers: Pb + (-2) = 0 ----> Pb = +2. Oxidation number of O=-2. Pb in PbSO4 : +2. But Sulfate ion has -2 charge. +1 +3 0-1 +2 +1. Check to see if the oxidation numbers show oxidation or reduction. H in H2 : 0. Therefore oxidation number of Pb is +2. 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. pb +2 s-2 + h +1 2 o-1 2 → pb +2 s +6 o-2 4 + h +1 2 o-2 b) Identify and write out all redox couples in reaction. Lead, being a metal, has very set oxidation numbers. SO4 has charge of -2. Identify the products and the reactants, and then their oxidation numbers. PbSO4 --> Pb2+ + SO4 2- (A net dissociation reaction of the salt) SO4 has an oxidation number of -2. 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