Home
Class 12
CHEMISTRY
H2 (gas) is bubbled through an aqueous s...

`H_2` (gas) is bubbled through an aqueous solution of `HCl(pH = 2.5)` at `25^@C`. If at `P_(H_2(g)) = 10^(-x))` bar the electrode potential will be zero. Then find value of x.

Text Solution

AI Generated Solution

The correct Answer is:
To solve the problem, we need to find the value of \( x \) such that the electrode potential of the hydrogen electrode becomes zero when hydrogen gas is bubbled through an aqueous solution of hydrochloric acid (HCl) with a given pH. ### Step-by-Step Solution: 1. **Understand the Reaction**: The half-reaction for the hydrogen electrode can be represented as: \[ \text{H}_2(g) \rightleftharpoons 2\text{H}^+(aq) + 2e^- \] 2. **Determine the Concentration of \( \text{H}^+ \)**: The pH of the solution is given as 2.5. We can find the concentration of \( \text{H}^+ \) ions using the formula: \[ [\text{H}^+] = 10^{-\text{pH}} = 10^{-2.5} \] 3. **Calculate \( [\text{H}^+] \)**: \[ [\text{H}^+] = 10^{-2.5} \approx 0.00316 \, \text{mol/L} \] 4. **Write the Reaction Quotient \( Q \)**: The reaction quotient \( Q \) for the hydrogen electrode can be expressed as: \[ Q = \frac{[\text{H}^+]^2}{P_{\text{H}_2}} \] where \( P_{\text{H}_2} \) is the partial pressure of hydrogen gas. 5. **Substitute Values into \( Q \)**: Substituting the concentration of \( \text{H}^+ \) into the equation for \( Q \): \[ Q = \frac{(10^{-2.5})^2}{P_{\text{H}_2}} = \frac{10^{-5}}{P_{\text{H}_2}} \] 6. **Set the Electrode Potential to Zero**: The electrode potential \( E \) is given by the Nernst equation: \[ E = E^\circ - \frac{RT}{nF} \ln Q \] For the standard hydrogen electrode, \( E^\circ = 0 \). Setting \( E = 0 \): \[ 0 = 0 - \frac{RT}{nF} \ln Q \] This implies: \[ \ln Q = 0 \implies Q = 1 \] 7. **Equate \( Q \) to 1**: From our earlier expression for \( Q \): \[ \frac{10^{-5}}{P_{\text{H}_2}} = 1 \] Thus, we have: \[ P_{\text{H}_2} = 10^{-5} \, \text{bar} \] 8. **Relate \( P_{\text{H}_2} \) to \( x \)**: We are given that \( P_{\text{H}_2} = 10^{-x} \, \text{bar} \). Therefore: \[ 10^{-x} = 10^{-5} \] This implies: \[ x = 5 \] ### Final Answer: The value of \( x \) is \( 5 \).

To solve the problem, we need to find the value of \( x \) such that the electrode potential of the hydrogen electrode becomes zero when hydrogen gas is bubbled through an aqueous solution of hydrochloric acid (HCl) with a given pH. ### Step-by-Step Solution: 1. **Understand the Reaction**: The half-reaction for the hydrogen electrode can be represented as: \[ \text{H}_2(g) \rightleftharpoons 2\text{H}^+(aq) + 2e^- ...
Promotional Banner

Topper's Solved these Questions

  • JEE MAIN REVISION TEST - 18

    VMC MODULES ENGLISH|Exercise CHEMISTRY - SECTION 2|5 Videos
  • JEE MAIN REVISION TEST - 13

    VMC MODULES ENGLISH|Exercise CHEMISTRY (SECTION 2)|5 Videos
  • JEE MAIN REVISION TEST - 19

    VMC MODULES ENGLISH|Exercise CHEMISTRY|26 Videos

Similar Questions

Explore conceptually related problems

A gas X at 1 atm is bubbled through a solution containing a mixture of 1M Y^(-) and 1M Z^(-) at 25^(@)C . If the reduction potential of ZgtYgtX , then

What happens when SO_2 gas is bubbled through an aqueous solution of copper sulphate in the presence of potassium thiocyanate?

The gas X at 1 atm is bubbled through a solution containing a mixture of 1M Y^(-) and 1M Z^(-) at 25^(@)C . If the order of reduction potential is ZgtYgtX , then

When H_(2)S gas is passed through aqueous solution of CuCl_(2), HgCl_(2), BiCl_(3) and CoCl_(2) in the presence of excess of dilute HCl, it fails to precipitate

Assertion (A): Magnesium can be obtained by the electronlysis of aqueous solution of MgCl_(2) . Reason (R ): The electrode potential of Mg^(2+) is much higher than H^(o+) .

A hydrogen electrode is prepared by using a sample of HCl solution with pH=4 and H_(2) gas at 1 atm pressure. What is the electrode potential of the electrode?

In pure water at 298 K, the electrode potential of H-electrode will be (Given P_H_2= 10^(-14 )atm)

A huydrgen electrode is dipped is a solution of pH = 3.0 at 25^@C The potential fo the cell will be .

A huydrgen electrode is dipped is a solution of pH = 3.0 at 25^@C The potential fo the cell will be .

Given 2H_(2)O rarr O_2 + 4H^+ + 4e^- , E_0 = -1.23 V . Calculate electrode potential at pH = 5.