Explanation:​
Spontaneous reactions occur in voltaic cells converting chemical energy to electrical energy, whereas, non-spontaneous reactions occur in electrolytic cells requiring electrical energy and converting this to chemical energy.
Electrolytic cells typically consist of one reaction vessel containing the aqueous of molten electrolyte. No salt bridge is therefore required.

Explanation:​
NaOH is a base so reacts with a hydrogen ion. HNO3​, nitric acid, releases a hydrogen ion through the breaking (heterolysis) of the O-H bond.
This question is moderately difficult as the student must recognise that NaOH is a base and HNO3​ an acid and correctly interpret a structural formula that may be unfamiliar.

Explanation​:
Weak acids produce strong conjugate bases. The salt when dissolved in solution would therefore be basic.

Explanation:​
Water accepts a hydrogen ion to produce H3O^+. This question is easy as the formation of H3O^+ is covered explicitly in the syllabus.

Explanation​:
By definition an acid is a proton donor. Weak acids only partially dissociate in aqueous solution leading to poor conductivity.

Explanation​:
NH3​ has a non-bonding pair of electrons it can donate to a central metal ion. BH3​ and CH4 do not have non-bonding electrons.

Explanation​:
Statement II is incorrect as acids produce solutions with $\mathrm{pH}$ lower than 7.

Explanation​:
Strong acids and weak bases react to produce acidic salts $(\mathrm{pH}<7)$ as the conjugate acid to a weak base is strong.

Explanation​:
Recall of the nitration intermediate covered in the syllabus. This is formed after the NO2^+ electrophile has been attacked by benzene’s pi electrons.

Explanation​:
Non-spontaneous reactions take place in electrolytic cells using an external power supply.
The positive electrode is the anode where oxidation takes place.
The aqueous metal ion (Mx^+) is reduced at the cathode to produce the solid metal.

Explanation:
In a primary alcohol, the OH group is bonded to a CH2​ group. The alcohol group initially reacts with KMnO4​ to form an aldehyde (CHO) group, as in option B.
However, the aldehyde is further oxidzed to a carboxylic acid (COOH) group unless it is removed by distillation. Here, the solution is heated under reflux, so the carboxylic acid is the major product.

Explanation:​
In electroplating, the anode is made of silver metal, which is oxidized to Ag^+ ions. The Ag^+ ions are then reduced at the cathode to Ag metal, resulting in a coating around this object.
Any impurities will sink to the bottom of the vessel.
In electrolytic cells, the anode is positive, and the cathode is negative. As a result, electrons travel from positive to negative.

Explanation:​
Lewis acids are electron pair acceptors.
BF3 and AlCl3​ both have incomplete octets and so can accept a pair of electrons.
Electrophiles, by definition, are electron-deficient species that accept pairs of electrons. Nucleophiles are electron-rich species that donate pairs of electrons (Lewis bases).

Explanation:​

Acids react with carbonates to produce a salt, water, and carbon dioxide.

Explanation​:
An acidic buffer solution contains a weak acid and the salt of its conjugate base.

Explanation:​
By definition, these are the standard conditions that must be recalled.

Explanation​:
By definition, strong acids completely dissociate in water.