Ahittorf cell fitted with ag/agcl electrodes is filled with 0.0106 molal aqueous hcl (molar mass: 36.458). a 2.00 ma current was passed for 10800 sec. the cathode solution was then found to weigh 51.7436 g and contain 0.0267 g hcl after analysis. what is the transport number of h+?
a. 0.177
b. 0355
c. 0.645
d. 0.823

Explanation:

The given data is as follows.

            Current = A

            Time = 10800 sec

Weight of cathode solution = 51.7436 g

Weight of HCl after analysis = 0.0267 g (in cathode solution)

Weight of anode solution = 52.0461 g

Weight of HCl in anode solution = 0.0133 g

Amount of electrolyte present = molality × molar mass

                                                   =

                                                   =

Calculate the amount of HCl initially present as follows.

          Electricity passed = = 21.6 C

Hence, amount of electrons passed will be as follows.

                    = 0.00024 mol

Therefore, mass of HCl initially present is as follows.

                     = (51.7436 - 0.0267)      

                     = 51.7169 g of water

               =    

               = 0.01994 g

Mass of HCl present after the electrolysis in 51.7169 g of = 0.0267 g

           Mass of HCl gained = 0.0267 - 0.01994

                                             = 0.00676 g

Hence, the amount of HCl gained =    

                                                        = 0.0001853 mol

Therefore, gain of in cathodic compartment = 0.000224 mol

So, transport number of =

                                                =

                                                = 0.823

Thus, we can conclude that the transport number of is 0.823.

i believe you are right for all except the 3rd ( look at sqdancefan his answer is much better)