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

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

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

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

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

Explanation:
Cathode site of reduction, anode site of oxidation, use CROA to remember this.
Reduction is the gain of electrons.

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

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

Explanation:

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

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

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

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

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

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.