H_(2)SO_(4)+NaOH rarr Na_(2)SO_(4)+H_(2)O

H_(2)SO_(4)+2NaOH rarr Na_(2)SO_(4) +2H_(2)O In this equation the equivalent weight of sulphuric acid is..........

Acic base + Redox titration 1^(st) titration : M/10 reacts with oxalic acid as well as H_(2)SO_4 according to equation H_(2)C_(2)O_4 + NaOH rarrNa_(2)C_(2)O_4 + H_(2)O, H_(2)SO_(4) + NaOH rarr Na_(2)SO_(4) + H_(2)O 2^(nd) titration : The mixture solution is titrated with M/10KMnO_4 solution which will reacts with oxalic acid (redox titration) in the presence of H_(2)SO_(4) H_(2)C_(2)O_(4) + underset(("Purple"))(KMnO_4)+H_(2)SO_(4) rarr K_(2)SO_(4) +underset(("Colourless"))( MnSO_4)+H_2O+CO_2 The reactionof oxalic acid with KMnO_4 is very slow therefore the oxalic acid solution is heated to 60-70^@C initially. Once the reation has started, its rate automatically increases. MnO_4^(-) acts as an oxidising agent. MnO_(4)^(-)overset(H^(+))rarrunderset("colourless")(Mn^(++),MnO_(4)^(--) ,MnO_(4) underset(H_2O)rarroverset("Brown ppt")(MnO_2) In the permanganate titration, the solution of reductant is always made acidic by adding H_2SO_4 rather than HCl or HNO_3 because

When 1L of 0.1 M sulphuric acid solution is allowed to react with 1 L of 0.1 M sodium hydroxide then the molarity of sodium sulphate formed is (H_(2)SO_(4) + 2NaOH rarr Na_(2)SO_(4) + 2H_(2)O) :

When 1L of 0.1 M sulphuric acid solution is allowed to react with 1 L of 0.1 M sodium hydroxide then the molarity of sodium sulphate formed is (H_(2)SO_(4) + 2NaOH rarr Na_(2)SO_(4) + 2H_(2)O) :

Acic base + Redox titration 1^(st) titration : M/10 reacts with oxalic acid as well as H_(2)SO_4 according to equation H_(2)C_(2)O_4 + NaOH rarrNa_(2)C_(2)O_4 + H_(2)O, H_(2)SO_(4)) + NaOH rarr Na_(2)SO_(4) + H_(2)O 2^(nd) titration : The mixture solution is titrated with M/10KMnO_4 solution which will reacts with oxalic acid (redox titration) in the presence of H_(2)SO_(4) H_(2)C_(2)O_(4) + underset(("Purple"))(KMnO_4)+H_(2)SO_(4) rarr K_(2)SO_(4) +underset(("Colourless"))( MnSO_4)+H_2O+CO_2 The reactionof oxalic acid with KMnO_4 is very slow therefore the oxalic acid solution is heated to 60-70^@C initially. Once the reation has started, its rate automatically increases. MnO_4^(-) acts as an oxidising agent. MnO_(4)^(-)overset(H^(+))rarrunderset("colourless")(Mn^(++),MnO_(4)^(--) ,MnO_(4) underset(H_2O)rarroverset("Brown ppt")(MnO_2) If 1.34 gm Na_(2)C_2O_4 dissolve in 50 ml of water this solution is titrated with KMnO_4 The volume of KMnO_4 used is

Balance the following chemical equations. (i) HNO_(3) + Ca(OH)_(2) rarr Ca(NO_(3))_(2) + H_(2)O (ii) NaOH + H_(2)SO_(4) rarr Na_(2)SO_(4) + H_(2)O (iii) NaCl + AgNO_(3) rarrAgCl +NaNO_(3) (iv) BaCl_(2)+H_(2)SO_(4) rarr BaSO_(4) + HCl

Balance the follwowing equations. 5) NaOH +H_(2)SO_(4) rarr Na_(2)SO_(4)+H_(2)O

Certain reactions regarding H_(2)SO_(4) are given H_(2)SO_(4)+NaOH to NaHSO_(4)+H_(2)O" "H_(2)SO_(4) +2NaOH to Na_(2)SO_(4) +2H_(2)O C_(12)H_(22)O_(11)+H_(2)SO_(4) to 12C+11H_(2)O These reactions shows that