It takes 126.5 minutes using a current of 5.15 A to deposit all of the nickel from 225mL of a solution contaiing `Ni^(2+)`. What was the original concentration of `Ni^(2+)` in the solution?

10 mL of 2(M) NaOH solution is added to 200 mL of 0.5 (M) of NaOH solution. What is the final concentration of the resultant solution?

A current of 3.7 A is passed for 6h between nickel electrodes in 0.5 L of a 2M solution of Ni(NO_(3))_(2) . What will be the molarity of solution at the end of electrolysis ?

A current of 2.0A is used to plate Ni(s) from 500mL of a 1.0M Ni^(2+) (aq) solution. What is the [Ni^(2+)] after 3.0 hours?

A current of 3.7 A is passed for 6hrs. Between Ni electrodes in 0.5 L of 2 M solution of Ni(NO_(3))_(2) . What will be the molarity of solution at the end of electrolysis?

Aqueous solution of Nickel sulphate contains Ni^(2+) and SO_(4)^(2-) ions. What is the product at the anode ?

The formation constant of Ni(NH_3)_6^(2+) is 6xx10^8 at 25^@C .If 50 ml of 2.0 M NH_3 is added to 50 ml of 0.20 M solution of Ni^(2+) , the concentration of Ni^(2+) ion will be nearly equal to :

A current of 3.6A is a passed for 6 hrs between Pt electrodes in 0.5L of 2M solution of Ni(NO_(3))_(2) . What will be the molarity of solution at the end of electrolysis?