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:
$\mathrm{l}$ is a neutral salt, Na2CO3 is a basic salt, and NaOH is a strong base.

Explanation:
ΔGθ = $-$.
For spontaneous reactions, ΔGθ is negative, therefore Ecellθ must be positive.

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:

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

Explanation:
Mg(s) loses electrons to produce $).$ Loss of electrons is oxidation which takes place at the anode.

Explanation:
Acidic solutions have high H^+ concentrations. Bases have a high concentration of OH^− ions

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

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:
Indicators are weak acids or bases where the components of their conjugate base/acid have different colours.

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:
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:
$\mathrm{NaOH}$ 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:
By definition an acid is a proton donor. Weak acids only partially dissociate in aqueous solution leading to poor conductivity.

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