Home
Class 12
CHEMISTRY
Adding powdered Pb and Fe to a solution ...

Adding powdered Pb and Fe to a solution containing `1.0 `M each of `Pb^(+2) and Fe^(+2)` ions would result in the formation of :

A

More of Pb and `Fe^(+2)` ions

B

More of Fe and `Pb^(2+)` ions

C

More of Fe and Pb both

D

More of `Fe^(+2 )and Pb^(+2)` ions

Text Solution

Verified by Experts

The correct Answer is:
A
Promotional Banner

Similar Questions

Explore conceptually related problems

Adding powdered Pb and Fe to a solution containing 1.0 M each of Pb^(2+) and Fe^(2+) ions would result into the formation of:

Adding powdered Cu and Zn to a solution containing 1.0 M is each of Cu^(​2+) and Zn^(​2+) ions would result into the formation of :-

An iron rod is immersed in a solution containing 1.0 M NiSO_(4) and 1.0 M ZnSO_(4) Predict giving reasons which of the following reactions is likely to proceed ? (i) Fe reduces Zn^(2+) ions, (ii) Iron reduces Ni^(2+) ions. Given : E_(Zn^(2+)| Zn )^(0) = -0.76 volt and , E_(Fe^(2+)|Fe)^(0) = -0.44 volt and E_(Ni^(2+)|Ni)^(0) = -0.25 V

Assertion (A): A solution contains 0.1M each of pB^(2+), Zn^(2+),Ni^(2+) , ions. If H_(2)S is passed into this solution at 25^(@)C . Pb^(2+), Ni^(2+), Zn^(2+) will get precpitated simultanously. Reason (R): Pb^(2+) and Zn^(2+) will get precipitated if the solution contains 0.1M HCI . [K_(1) H_(2)S = 10^(-7), K_(2)H_(2)S = 10^(-14), K_(sp) PbS =3xx 10^(-29) K_(sp) NiS = 3 xx 10^(-19). K_(sp) ZnS = 10^(-25)]

An aq. Solution containing Hg^(2+),Pb^(2+) and Cd^(2+) ions is mixed with dil. HCl . Which will be precipitated

An aqueous solution containing 0.1M Fe^(3+) and 0.01 M Fe^(2+) was titrated with a concentrated solution of NaOH at 30^(@)C , so that changes in volumes were negligible. Assuming that the new species formed during titration are Fe(OH)_(3) and Fe(OH)_(2) only. Given E^(c-)._(Fe^(3+)|Fe^(2+))=0.80V, K_(spFe(OH)_(3))=10^(-37), and K_(sp Fe(OH)_(2))=10^(-19) The redox potential of Fe^(3+)|Fe^(2+) electrode at pH=6 is

MnO_(4)^(-) ions are reduced in acidic conditions to Mn^(2+) ions whereas they are reduced in neutral condition to MnO_(2) . The oxidation of 25 mL of a solution x containing Fe^(2+) ions required in acidic condition 20 mL of a solution y containing MnO_(4) ions. What value of solution y would be required to oxidize 25 mL of solution x containing Fe^(2+) ions in neutral condition ?

Statement-1: No yellow precipitate is formed when an excess of a more concentrated (6M) solution of KI is added to a solution containing Pb^(2+) ions. Statement-2: Solution of [PbI_(4)]^(2-) on dilution with water produces yellow precipitate of PbI_(2) .

An aqueous solution containing Hg^(2+),Hg_(2)^(2+),Pb^(2+) and Cd^(2+) ions will give precipitate of _______ with dil. HCl