In Dennis method fluorine prepared in the electrolytic cell is passed through U-tubes containing sodium fluoride to remove HF vapors present in fluorine as `NaHF_(2)` .The compound `NaHF_2` contains the species

KF combines with HF to form KHF_(2) The compound contains the species .

The same amount of electricity was passed through molten cryolite containing Al_(2)O_(3) and NaCl. If 1.8 g of Al were liberated in one cell, the amount of Na liberated in the other cell is

(i) Why could fluorine not be prepared for a long time from HF and metal fluorides either by electrolysis or by any chemical reaction ? (ii) Describe the modern method for the preparation of fluorine by giving: (a) Materials used in the construction of the cell. (b) Electrolyte used. (c) Electrode reactions.

3 faraday electricity was passed through the three electrolytic cells connected in series containing Ag^(+)Ca^(2+) and Al^(+3) ions respectively. The molar ration in which the three metl ions are liberated at the electrodes is :

A current of 10 A is passed for 80 min and 27 seconds through a cell containing dilute sulfuric acid. (1) How many moles of oxygen gas will be liberated at the anode ? (2) Calculate the amount of zinc deposited at the cathode when another cell containing ZnSO_(4) solution is connected in series.

What are reactions involved in removing SO_(2) from the atmosphere by passing it through a solution containing citrate ions ?

In Ostwald and Walker's appratus, dry air is passed through a solution containing 20 gram of an organic non-volatile solute in 250 ml of water. Then the air was passed through pure water and then through a U-tube containing anhydroous CaCl_(2) . The mass lost in solution is 26 gram and the mass gained in the U-tube is 26.48 gram. Calculate the molecular mass of organic solute.

In passing 3F of electricity through three electrolytic cells connect in series containing Ag^(o+),Ca^(2+), and Al^(3+) ions, respectively. The molar ratio in which the three metal ions are liberated at the electrodes is

In passing 3F of electricity through three electrolytic cells connect in series containing Ag^(o+),Ca^(2+), and Al^(3+) ions, respectively. The molar ratio in which the three metal ions are liberated at the electrodes is a.1 : 2 : 3 b.2 : 3 : 1 c.6 : 3 : 2 d.3 : 4 : 2

(a) A steady current of 2 amperes was passed through two electrolytic cells X and Y connected in series containing electrolytes FeSO_(4) and ZnSO_(4) until 2.8 g of Fe deposited at the cathode of cell X. How long did the current flow ? Calculate the mass of Zn deposited at the cathode of cell Y (Molar mass : Fe= 56 g mol^(-1) Zn-65.3g mol^(-1) , 1F -96500 C mol^(-1) ) (b) In the plot of molar conductivity (wedge_(m)) vs Square root of concentration (c^(1//2)) , following curves are obtained for two electrolytes. A and B: Answer the following : (i) Predict the nature of electrolytes A and B. (ii) What happens on extrapolation of wedge_(m) to concentration approaching zero for electrolytes A and B ?