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chem question
AN10:
white phosphorus reacts with dilute aq. solutions of copper (II) sulfate to deposit metallic copper and produce a strongly alkaline sol.
In an experiment to investigate this reaction, 0.31g of white phosphorus reacted in excess aq. copper sulfate giving 1.6g of metallic copper.
(i) Calculate the new oxidation number of the phosphorus after the reaction.
(ii) In the reaction, the phosphorus forms an acid HPOn, what is the value of n.
nid404:
(i) Ideally it should be +2...but i'm not very confident..think it's two cuz copper will accept two electron from phosphorous to become metal
(ii) H should also be having a subscrip...i've heard of nothing like this...plz check again
what is the answer though?
AN10:
i checked there is no subscript of H....n i dont know da answer....Thanks anywayz!...By the way do u hav any idea wht will be da equation for this reaction?
nid404:
nope the question is strange....i don't know how there's an alkaline solution being formed in the first place....I'll find out anyways
if the question is correct, then it's pretty unusual
nid404:
okay here you go...very strange reaction...
A Piece of ordinary phosphorus when placed in a solution of copper sulphate becomes covered with a black film of copper phosphide and then with a firm coating of bright metallic copper. The black phosphide is always found between the phosphorus and the copper.
check the pdf....i didn't get the head and tail of this reaction...a little new for me....
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