NaCI(s) + H2SO4(I) → HCI(g) + NaHSO4(s).
In the reaction above, H2SO4 behaves as?
a strong acid
an oxidizing agent
a good solvent
a dehydrating agent
Explanation
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Discussions (17)
The selected answer is wrong:
The correct answer is A as in a chemical reaction like that involving two acids in such manner, the acid in the reactant position is a strong acid and the acid appearing as the product is volatile
Answer- B: Oxidizing agent
Explanation:
When an electropositive metal (e.g Na, etc) is being added to any specie (ion, atom, compound, etc), it said to have undergo REDUCTION
Therefore, when Sodium (Na) was added to H2SO4, it was reduced and the substance being reduced (H2SO4) is called the Oxidizing agent
B is the answer because the removal of hydrogen in the product is reduce therefore it is oxidizing agent
option A is correct. Please take note that the reaction is not REDOX. First, because their oxidation number remains the same in both reactants and product. Even if Na, an electropositive element was added to H2SO4 to form NaHSO4. It's still not REDOX
e.g
NaCl + PbSO4 ---> NaSO4 + PbCl
first you can notice the oxidation number of Na changed from +1 to +2 and Pb, from +2 to +1. This is the first sign to notice in a REDOX rxn. Even if the redox rxn is based on addition and removal of electropositive element, there must be a change in oxidation number.
Prep 50 made a mistake i feel it is supposed to be except bcos in my chemistry prep 50 thsy choose good solvent as the answer lol
option A and D are all correct about Sulphur
but in this case option A is very correct
