HSO_(4)

The voltage of the cell Pb(s)|PbSO_(4)(s)|NaHSO_(4)(0.600M)||Pb^(2+)(2.50 xx 10^(-5)M)|Pb(s) is E = +0.061V . Calculate K_(2) = [H^(+)] [SO_(4)^(2-)]//[HSO_(4)^(-)] the dissociation constant for HSO_(4)^(-) . Given Pb(s) +SO_(4)^(2-) rarr PbSO_(4) +2e^(-) (E^(@) = 0.356V),E^(@) (Pb^(2+)//Pb) =- 0.126V .

The voltage of the cell Pb(s)|PbSO_(4)(s)|NaHSO_(4)(0.600M)||Pb^(2+)(2.50 xx 10^(-5)M)|Pb(s) is E = +0.061V . Calculate K_(2) = [H^(+)] [SO_(4)^(2-)]//[HSO_(4)^(-)] the dissociation constant for HSO_(4)^(-) . Given Pb(s) +SO_(4)^(2-) rarr PbSO_(4) +2e^(-) (E^(@) = 0.356V),E^(@) (Pb^(2+)//Pb) =- 0.126V .

For the reaction: I^(-)+ClO_(3)^(-)+H_(2)SO_(4)toCl^(-)+HSO_(4)^(-)+I_(2) The correct statement(s) in the balanced equation is/are (1) Stoichiometric coefficient of HSO_(4)^(-) is 6 (2) Iodide is oxidized. (3) Oxidation number of chlorine changes by 5 units (4) H_(2)O is one of the products

For the reaction: I^(-)+ClO_(3)^(-)+H_(2)SO_(4)+Cl^(-)+HSO_(4)^(-)+I_(2) The correct statement(s) in the balanced equation is/are (1) Stoichiometric coefficient of HSO_(4)^(-) is 6 (2) Iodide is oxidized. (3) Oxidation number of chlorine changes by 5 units (4) H_(2)O is one of the products

Write the conjugate acid and conjugate base of each of the following: HSO bar4