The total should equal when you add all oxidation numbers: Pb + (-2) = 0 ----> Pb = +2. Check to see if the oxidation numbers show oxidation or reduction. It is suggested that a precipitation mechanism to form PbSO 4 occurs under some conditions prior to the solid state … Figuring out why these numbers are the way they are takes a fair amount of work. Lead, being a metal, has very set oxidation numbers. Oxidation = number goes down Reduction = number goes up. PbSO4 --> Pb2+ + SO4 2- (A net dissociation reaction of the salt) SO4 has an oxidation number of -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) Therefore x+6-8=0. To neutral that -2 charge, +2 charge should be there and it is given by Pb 2+ ion. So, Pb is at +2 oxidation state. But Sulfate ion has -2 charge. +1 +3 0-1 +2 +1. SO4 has charge of -2. Also, the answer would not be +10 if what you had said was correct (about the sulfur ion). 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. H2O2 + PbS --> PbSO4 + H2O. 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. Therefore oxidation number of Pb in PbSO 4 … Pb in PbSO4 : +2. Pb. Therefore oxidation number of Pb is +2. In order to make the compound neutral, Pb must be +2. Identify the products and the reactants, and then their oxidation numbers. PbSO 4 salt does not have an overall charge. 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). Asked by | 25th Mar, 2009, 06:56: PM. Identify which reactants are being oxidized (the oxidation number increases when it reacts) and which are being reduced (the oxidation number goes down). 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. Sulfide ion is at -2 oxidation state. How to calculate oxidation number of Pb in PbSO4?And Explain? You are correct that oxidation is the loss of electrons and reduction is the gaining of electrons. H in H2 : 0. Expert Answer: Let the oxidation number of Pb=x. ... Pb PbO2 PbSO4 H2O H2SO4. 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. Could you tell me how you went about getting the oxidation number for Pb in PbSO4? What is the oxidation number of phosphorous in the H3PO2 molecule? It can only be +2, or +4. 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