please complete the following worksheet no irrelevant answers, please best answer=brainliest
Answers
(2) Pure water is almost a non-electrolyte and a polar solvent. It can be electrolytically decomposed by addition of traces of dilute acid which dissociates as ions and help in dissociating water into hydrogen and hydroxide ions. Therefore, electrolysis of acidulated water is considered to be an
(3)
(a) During electrical conductivity of copper sulphate solution, the the CuSO4 splits into Cu2+ and SO42-
ions. Whereas, copper metal only conducts electricity but does not undergo any change.
(b)
i) At Cathode, copper metal is deposited.
At Anode, Oxygen gas and water.
ii) The blue colour of copper sulphate solution becomes light and discharges at the end.
iii) At Cathode
Cu2+ + 2e- ----------> Cu
At Anode
4 OH- + 4e- ----------> 2H2O + O2
(4)
(a) Solid sodium chloride does not conduct electricity, because there are no electrons which are free to move. When it melts, sodium chloride undergoes electrolysis, which involves conduction of electricity because of the movement and discharge of the ions.
(b) The presence of water in dilute sulphuric acid increases the hydrogen ion concentration. Hence it is a stronger acid than concentrated sulphuric acid which contains comparatively less water.
(c) Normally, Carbon is used as a reducing agent during extraction of metals (e.g Fe), However Aluminium is a strong reducing agent and cannot be reduced by 'C'. Also, Al-O bond is extremely strong and requires high energy to break which requires very high temp. (above 2000°C), which is difficult to maintain. Hence, electrolytic reduction method is easier and cheaper.
(d) The metal anode continuously dissolves as ions in solution and hence needs to be replaced periodically.
(5)
(a) An aqueous solution of nickel sulphate with few drops of dilute sulphuric acid.
(b) The key chain
(c) Pure nickel bar
(d) At Cathode
Ni2+ + 2e- --------> Ni
At Anode
Ni- + 2e- ----------> Ni2+
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