Complete this equation for the dissociation of the electrolyte NaCl(aq). Omit water from the equation because?
NaCl(aq) → Na{+}(aq) + Cl{-}(aq)
Which of the following is an electrolyte when placed in aqueous solution?
(X) 1. C6H12O6 it's soluble in water ,but it cannot form ions. (X) 2. C6H6 it is not soluble in water. (X ) 3. CCl2F2 it is not soluble in water. (O) 4. NaCl it's soluble in water ,and it forms plenty of Na+ and Cl- ions (X) 5. CCl3H it is not soluble in water.
Why is electrolysis of dilute NaCl different from concentrated NaCl?
If you look up the electrode potentials, you will see that it's easier to discharge hydroxide ions than chloride ions, so in dilute solution the production of oxygen is preferred. However when the solution is concentrated, the anode is surrounded by lots of chlorides and extremely few hydroxides so it's almost as if the hydroxides are not there and the chlorides are discharged.
Electrolysis of aqueous sodium chloride is an important industrial process?
(i) Electrolysis of aqueous sodium chloride is an important industrial process, since the products are commercially important chlorine, hydrogen, and sodium hydroxide. 2 NaCl(aq) + 2 H2O(l) Cl2(g) + H2(g) + 2 NaOH(aq) Assuming you begin with 293 g of NaCl, answer the following questions: a) How many grams of Cl2 are theoretically obtainable? Answer: 178 g b) How many grams of NaOH are theoretically obtainable? Answer: 201. g (c) How many grams of water must be consumed for complete reaction? Answer: 90.3 g (ii)What are the ion concentrations in a 0.24 M solution of Na3PO4? Answer: [Na+] = 0.72 M and [PO43-] = 0.24 M (iii) We have a 5.82 x 10-10 M solution of HCl. What is the pH of this solution at 25 C? Answer: 7.00 I would appreciate any help on how to get the right answer, thank you. :)
Why does solid sodium chloride act as a nonelectrolyte while...?
Solid sodium chloride, NaCl, acts as a nonelectrolyte in the solid phase because in the solid phase the atoms are closely packed together in a rigid structure and can't move around freely. This also prevents the electrons from moving around freely so solid NaCl acts as a nonelectrolyte. Molten NaCl is an electrolyte. An aqueous solution acts as an electrolyte because when NaCl dissolves in water, it disassociates into its Na+ and Cl- ions, thereby allowing for electrical conductivity.
Why during the electrolysis of NaCl, sodium do not deposit at cathode?
The redox couple Na+/Na has a very negative redox potential, meaning it is very hard to reduce and if reduced it very strongly tries to give its electron to something else. If there is nothing to accept the electrons but Na, as in the NaCl melt Alistair referred to, then you will get (liquid) Na metal. If it is in aqueous solution, the electrons go onto H+ and you get hydrogen gas. In fact if you were to reduce some sodium metal, what does sodium do when in contact with water? It reduces H+ to hydrogen gas in a reaction so spontaneous that the heat evolved ignites the hydrogen! And you are left with NaOH solution, the Na+ from oxidation of Na metal and the OH- from water as it dissociates to replace the leaving H+ ions.
If I add table salt (NaCl) into water and do electrolysis do I get chlorine and hydrogen gases? No oxygen gas at all?
You get three useful products when you electrolyse strong salt solution, chlorine gas, hydrogen gas, and sodium hydroxide left in the electrolyte.GCSE CHEMISTRY - What is the Electrolysis of Brine? - What are the Products of the Electrolysis of Brine? - What are Half Equations? - GCSE SCIENCE.You have to use a cell with a membrane that separates the two gases. the diaphragm and membrane cells for the manufacture of chlorineThe Chloralkali processAlternatively a Mercury cell is used but these are being phased out due to the obvious hazards.Castner–Kellner process
Why is NaOH formed near cathode during electrolysis of brine?
During electrolysis of brine(aq. NaCl), NaCl and water are present as electrolyte. Na+ (from NaCl) and H+(from water) tends to move to negative terminal (i.e cathode) while Cl- (from NaCl) and OH-(from water) tends to move to positive terminal(i.e anode). Now only one from Na+ and H+ at cathode will get reduce ,which has a higher standard reduction potential. Standard reduction potential of Na+ (E°=-2.71V) which is quite less from that of H+ ion (E°=0.00V), H+ reduces at cathode and H2 gas will produce. Similarly only one from Cl-and OH- will get oxidise at anode, which has lower standard reduction potential. Standard reduction potential of Cl-is. E°=1.36V while that of H2O/OH- is 1.23 V. So Standard reduction potential of hydroxide ion is less than that of Cl- ion , which implies that O2 must be released by oxidation of hydroxide ion. But reality is different due to over potential of H2O /OH- doesn't get oxidise easily and requires high potential then calculated value, so at the given potential Cl- gets oxidise at anode and Cl2 gas is liberated . So Cl2 gas is liberated at anode and H2 gas is at cathode. The rest Na+ and OH- are in the solution and forms aq NaOH.