Concentration Cell

Which of the following facts about the chemical cell and concentration cell is correct?

A galvanic cell is composed of two hydrogen electrodes, one of which is a standard one. In which of the following solutions should the other electrode be immersed to get maximum $\mathrm{emf}$?

A cell contains $0.04 \mathrm{M} {\mathrm{Cr}}^{3+}$ in one compartment and $1.0 \mathrm{M} {\mathrm{Cr}}^{3+}$ in the other, with $\mathrm{Cr}$ electrodes in both. Which is the anode compartment?

The $\mathrm{emf}$ of a galvanic cell composed of two hydrogen electrodes is $272 \mathrm{mV}$. What is the $\mathrm{pH}$ of the solution in which the anode is immersed if, the cathode is in a solution with a $\mathrm{pH}$ of $3$?

Round off your answer to the first place of decimal.

Calculate the potential of the cell,

${\mathrm{Cl}}_2 \left(\mathrm{p}=0.9 \mathrm{atm}\right)\left|\mathrm{NaCl}\text{ solution }\right|{\mathrm{Cl}}_2\left(\mathrm{p}=0.1 \mathrm{atm}\right)$

Answer correct up to three decimal places with proper sign on the potential.

For the cell, $\mathrm{Pt}| {\mathrm{H}}_2 \left(1 \mathrm{atm}\right) | {\mathrm{H}}^{+}\left(\mathrm{pH} \mathrm{unknown}\right)\left|\right|{\mathrm{H}}^{+} \left(\mathrm{pH}=1\right)\left|{\mathrm{H}}_2\left(1 \mathrm{atm}\right)\right|\mathrm{Pt}$. The measured cell potential at $25°\mathrm{C}$ is $0.16 \mathrm{volt}$  Calculate the unknown $\mathrm{pH}$.

A galvanic cell is constructed of two hydrogen electrodes, one immersed in a solution with ${\mathrm{H}}^{+}$ at $1 \mathrm{M}$ and the other in $1 \mathrm{M}$ $\mathrm{KOH}$. Calculate $E_{\text{cell }}.$ If $1 \mathrm{M} \mathrm{KOH}$ solution is replaced by $1 \mathrm{M} {\mathrm{NH}}_3,$ will $E_{\text{cell }}$ be higher or lower than in $1 \mathrm{M} \mathrm{KOH}?$

Calculate the potential of a cell in which hydrogen electrode is immersed, in a solution with a $\mathrm{pH}$of $3.5$ and in a solution with a $\mathrm{pH}$ of $10.7.$ Round off your answer to three decimal places.

Calculate the potential of a silver electrode in a saturated solution of $\mathrm{AgBr} \left({\mathrm{K}}_{\mathrm{sp}}=6\times {10}^{-13}\right)$ containing, in addition, $0·1$ mole per litre $\mathrm{KBr}$. ${\mathrm{E}}_{{\mathrm{Ag}}^{+}/Ag}^0=0.80 \mathrm{volt}$.

Round off the answer up to two places of decimal.

Neglecting the liquid-junction potential, calculate the $\mathrm{emf}$ of the following cell at $25°\mathrm{C}$

${\mathrm{H}}_2(1 \mathrm{atm})|0·5 \mathrm{M} \mathrm{HCOOH}|\left|1 \mathrm{M} {\mathrm{CH}}_3\mathrm{COOH} \right| {\mathrm{H}}_2(1 \mathrm{atm})$

The dissociation constants of $\mathrm{HCOOH}$ and ${\mathrm{CH}}_3\mathrm{COOH}$ are $1.77\times {10}^{-4}$ and $1.8\times {10}^{-5}$, respectively. 

report your answer in volts.

What is the potential of a cell containing two hydrogen electrodes; the negative one in contact with ${10}^{-8} \mathrm{M}$ of ${\mathrm{H}}^{+}$, and the positive one in contact with $0.025 \mathrm{M}$ of ${\mathrm{H}}^{+}?$