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

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:​

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

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

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

Explanation​:
The student must be sufficiently familiar with the reactions covered in the syllabus to realize that sodium hydroxide would not be useful for producing a diol from an alkene. Alternatively, the question could be answered by recalling the use of sodium hydroxide in the other three reactions. The question is categorized as easy as only limited knowledge of reactions in the literature is needed.
Reactions B and C are both acid-base reactions where NaOH deprotonates the organic species.
Reaction D is a nucleophilic substitution of a halogenoalkane with OH− as the nucleophile.
Reaction A would require first halogenation (with e.g. Br2​) followed by nucleophilic substitution.

Explanation:​
C3H8 is a saturated alkane and C3H6 is an unsaturated alkene. The test of unsaturation using Br2(aq) can demonstrate the presence or absence of a carbon-carbon double bond.
In the presence of a double bond, Br2(aq) can add across the double bond in the alkene producing a dibromo-alkane, and a change of color from brown to colorless will be observed.
In the case of the absence of a double bond (saturated hydrocarbon), no color change would occur.

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

Explanation​:
Ligands are Lewis bases with a lone pair of electrons that they can donate to a central metal ion.

Explanation:​

Metals and acids react to produce a salt and hydrogen gas. The formulae of the ions are Mg^2+ and NO3^−, therefore for a neutral salt, two nitrate ions are required for each magnesium ion.

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

Explanation​:
Ethanoic acid is a weak acid and sodium hydroxide is a strong base. At the equivalence point, $\mathrm{pH}>7$, therefore the indicator chosen must have an endpoint>7(as determined by its pKa​).

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

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:​
A tenfold decrease in [H+], leads to a pH increase of 1.

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

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

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:​
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​.