Can we store :
(i) Copper sulfate solution in zinc vessel ?
(ii) `FeSO_(4)` solution in silver vessel ?
(iii) Copper sulfate solution in iron vessel?
(iv) 1 M `CuSO_(4)` solution in Ni container ?
Give suitable explanation in support of your answer.

Can we store Copper sulphate solution in iron vessel?

Is it safe to stir 1M AgNO_(3) solution with a copper spoon? Give suitable explanation in support of your answer ?

Is it possible to store: (i) Copper sulphate solution in a zinc vessel? (ii) Copper sulphate solution in a silver vessel? (iii) Copper sulphate solution in a gold vessel? Given: E_(Cu^(2+)| Cu )^(0) = + 0.34 volt and E_(Ag^(2+)| Ag )^(0) = 0.80 volt and E_(Au^(2+)| Au )^(0) = +1.50 volt

Assertion : Copper sulphate solution is not stored in zinc vessel. Reason : Zinc forms complex with CuSO_(4) .

Why cannot we store AgNO_3 solution in copper vessel ?

Which of the following pairs will give displacement reactions? (i) NaCl solution and copper metal (ii) MgCl_(2) solution and aluminium metal (iii) FeSO_(4) solution and silver metal (iv) AgNO_(3) solution and copper metal

Which is the wrong pair? (i) Starch solution : sol (ii) Aq. NaCl : true solution (iii) Milk : emulsion (iv) Aq. BaSO_4 : true solution The correct choice is :

What happens when a zinc rod is dipped in copper sulfate solution ? Give the reason for this observation.

Aqueous copper sulphate solution and aqueous silver nitrate solution are electrolysed by 1 ampere current for 10 minutes in separate electrolytic cells. Will the mass of copper and silver deposited on the cathode be same of different? Explain your answer.

Hydroxylamine reduce iron (III) according to the equation : 2NH_(2)OH + 4 Fe^(3+) rarr N_(2)O(g)uarr + H_(2)O + 4Fe^(2+) + 4H^(+) Iron (II) thus produced is estimated by titration with a standard permanganate solution. The reaction is MnO_(4)^(-) + 5 Fe^(2+) + 8H^(+) rarr Mn^(2+) + 5Fe^(3+) + 4H_(2)O A 10 mL sample of hydroxylamine solution was diluted to 1 litre. 50 mL of this diluted solution was boiled with an excess of iron (III) solution. The resulting solution required 12 mL of 0.02 M KMnO_(4) solution for complete oxidation of iron (II). Calculate the weight of hydroxylamine in one litre of the original solution