Home
Class 12
CHEMISTRY
pH of the solution in the anode compartm...

pH of the solution in the anode compartment of the following cell at `25^@C` is x when Eced `E_("cell")-E_("cell")^(@)=0.0591V`.
`underset("1 atm")(PT (H_(2))|pH=Xx|| Ni^(2+)(M)|Ni`
Find the value of x.

Text Solution

Verified by Experts

The correct Answer is:
1
`Ni^(2+) +H_(2) to Ni+2H^(-1)`
`K=([H^(+)]^(2))/([Ni^(2+)])=[H^(+)]^(2)`
`E_("cell")-E_("cell")^(@)=0.0591 xx pH`
pH=1
Promotional Banner

Topper's Solved these Questions

  • ELECTROCHEMISTRY

    FIITJEE|Exercise Exercise 1|1 Videos

  • ELECTROCHEMISTRY

    FIITJEE|Exercise Exercise 2|1 Videos

  • ELECTROCHEMISTRY

    FIITJEE|Exercise Matrix Type Single Correct Question|3 Videos

  • CONCEPT OF ACIDS AND BASES

    FIITJEE|Exercise SINGLE INTEGER ANSWER TYPE QUESTIONS|4 Videos

  • ELECTROPHILIC AROMATIC SUBSTITUTION

    FIITJEE|Exercise NUMERICAL BASED QUESTIONS INDICATED BY DIGITAL INTERGER|1 Videos

Similar Questions

Explore conceptually related problems

pH of the anodic solution of the following cell is Pt, H_2(1atm)|H^+(xM)||H^(+)(1M)|H_2(1 atm ),Pt if E_("cell") =0.2364V.

The potential of the following cell is 0.34 V at 25^(@)C calculate the standard reduction potential of the copper half cell Pt|H_(2)(1 atm)| H^(+)(1 M)||Cu^(2+)(1 M)|Cu

Determine of pH : The following cell has a potential of 0.55 V at 25^(@)C : Pt(s)|H_(2)(1 bar)|H^(+)(aq. ? M)||Cl^(-)(1 M)|Hg_(2)Cl_(2)(s)|Hg(l) What is the pH of the solution in the anode compartment? Strategy: First, read the shorthand notation to obtain the cell reaction. Then, calculate the half cell potential for the hydrogen electrode from the observed cell potential and the half cell poten-tial for the calomel reference electrode. Finally, apply the Nernst equation to find the pH .

(a) What type of a cell is the lead storage battery ? Write the anode and the cathode reactions and the overall reaction occuring in a lead storage battery while operating . (b) A voltaic cell is set up at 25^(@)C with the half-cells , Al|Al^(3+) (0.001M) and Ni| Ni^(2+) (0.50 M) . Write the equation for the reaction that occurs when the cell generates an electric current and determine the cell potential. (Given : E_(Ni^(2+)|Ni)^(@) = -0.25 V , E_(Al^(3+)|Al)^(@) = -1.66V ).

In the electrochemic al cell Zn|Zn^(2+)||H^(+)|Pt,H_(2) E_("cell")^(@)=E_("cell") when

(a) A cell is prepared by dipping a zinc rod in 1M zinc sulphate solution and a silver electrode in 1M silver nitrate solution. The standard electrode potential given : E^(@)Zn_(2+1//Zn) = -0.76V, E^(@)A_(g+//)A_(g) = +0.80V What is the effect of increase in concentration of Zn^(2+) " on the " E_(cell) ? (b) Write the products of electrolysis of aqueous solution of NaCI with platinum electrodes. (c) Calculate e.m.f. of the following cell at 298 K: "Ni(s)"//"Ni"^(2+)(0.01M)////"Cu"^(2+)(0.1M)//"Cu(s)" ["Given"E_(Ni2+//Ni)^(@) = -0.025 V E_(Cu2+//Cu)^(@) = +0.34V] Write the overall cell reaction.

The pH of LHE in the following cell is : Pt, H_(2)(1atm)|H^(o+)(x M)||H^(o+)(0.1M)|H_(2)(0.1atm)Pt E_(cell)=0.295V .