Explanation:​
The student must identify the reagents and conditions for three reactions. Only information stated explicitly in the syllabus is needed and no interpretation of structural formulas is required. This question is therefore, categorized as “easy”.
Alkenes react with HCl in an addition reaction, alkanes react with halogens in the presence of UV light through free radical substitution, and halogenoalkanes react with NaOH in a nucleophilic substitution reaction.

Explanation:​
Oxidation involves the loss of electrons and an increase in oxidation state.

Explanation​:
$)$ gains electrons and is reduced to $\mathrm{Zn}(\mathrm{s})$ at the cathode. $\mathrm{l})$ loses electrons and is oxidised to Cl2(g) at the anode

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

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​:
Use the mnemomic CNAP; cathode negative, anode positive for the polarity in electrolytic cells.

Explanation:​
A nucleophile is a species that is electron-rich and an electron donor.
An electrophile is an electron deficient species.

Explanation:​
The HPO4^− ion contains two negatively charged oxygen atoms which can bond to hydrogen ions, producing phosphoric acid (H3PO4​).
The HPO4^− ion can therefore react with two H+ ions.
This question is moderately difficult as the student must recognise that H^+ ions bond to the negatively charged oxygen atoms, or that HPO4^− is derived from H3PO4​.

Explanation:​
Lewis bases are electron pair donors and so, must have a lone (non-bonding) pair of electrons.

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

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

Explanation:​

A 1.0M solution of KOH would have a pH of 14. Methyl orange, bromocresol green, and phenolphthalein would be orange, yellow, and green respectively at this pH.

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​:
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:​
H2O is more readily oxidized than Cl^− and SO4^2−, however, when concentrated aqueous NaCl is used, chlorine is produced at the anode

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:
By definition, the more readily an acid releases a proton, the less likely the conjugate base is to accept a proton.

Explanation​:
$\mathrm{NaOH}$ is a strong base and so would release a high concentration of OH− ions in water. Choices A and C are incorrect as $\mathrm{HCl}$ and H2SO4 are strong acids and would give low pHs. $\mathrm{NaCl}$ is a neutral salt.

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