Question

2. How many milliliters of 0.100 M HNO, are needed to neutralize the following solution? Write the balanced molecular equation, complete ionic equation, and net ionic equation. 58.5 mL of 0.0100 M Al(OH)3 HNO₃ + KOH KNO3 + H2O 3. a) Balance the following equations. b) Identify oxidizing and reducing agents. e) Determine the oxidation numbers of the elements involved in the redox reaction. Zn (s) + CuSO4 (aq) - ZnSO4 (aq) + Cu(s) 12 (5) + S20;- (aq) + (aq) + S.O.- (aq) 4. Complete and balance the following equations and write the net ionic equations for each. FeCl2 (aq) + Na2S (aq) → MgSO4 (aq) + BaCl2 (aq) +

Answer 1

The oxidation state of Sulphur in S4O6 ^2- comes out to be 2.5 from hit and trial method. But oxidation state cannot be in fraction. So its its oxidation state is determined by its structure. See images.
eliven: 58.5m of 0.01000 M AOH Chomical hesohan: AllO3 +3H NO 10.01m) 1 mele of Allog tem milanity euatio + (0.1 M) 3 male ot HNo M2V2 3HNO 3xO.100x V 0.01x58.5md 0.0l Mx 58.5ml 1.9S -Zn So4 -+ Culs) nt CuSo4 reduciny agent 2+ 2t Cu + reduced adising agent 21 S40 Reductng agent 2- S40% 2 I 203 1 deduced ielismg gent ootidahion Reducny gat educ tron- aeng frS402- 4004 60-2-2 2.5 Anarease in chaige ce cnease. in charge charge Am 2it-23--2 7

3t (s, ertm ble of daubli dis plucement ncactm des2+21t +2 c1e Macly t BaS04. This is again em Hle of daulle dilacoment Juactiom 24 + Ba+2ce+ So2 Baso4 Ocidatim Nimber of 94 = 20