At 298 K, if emf of the cell corresponding to the reaction, $\mathrm{Zn}(\mathrm{s})+2 \mathrm{H}^{+}(\mathrm{aq}) \rightarrow \mathrm{Zn}^{2+}(0.01 \mathrm{M})+\mathrm{H}_2(\mathrm{~g})(1 \mathrm{~atm})$ is 0.28 V, then the pH of the solution at the hydrogen electrode is $\left(\frac{2.303 \mathrm{RT}}{\mathrm{~F}}=0.06 \mathrm{~V}\right),\left(\mathrm{E}_{\mathrm{Zn}^{2+} \mid \mathrm{Zn}}^{\mathrm{o}}=-0.76 \mathrm{~V}\right)$

• A

  $7$
• B

  $8$
• Correct answer
  C

  $9$
• D

  $10$

Hence, the correct answer is option: 'C'.