Quiz 1 - Chemical Reactions and Properties of Solutions | Chemical Reactions and Properties of Solutions

A net ionic equation only shows the ions that form a solid, so here MnCO₃

Solubility is the maximum quantity of solute dissolvable in a solvent at a particular temperature. A solid is more soluble at higher temperatures and in a solvent with similar types of intermolecular forces.

A Brönsted base is a substance that can accept a proton (H⁺ acceptor)

A Lewis base is an electron-pair donor and so must have a lone pair of electrons

• Charge of H₂CO₃ = 0 ⇒ Oxidation Number (O.N.) of C + 2 O.N. of H + 3 O.N. of O = 0
• O.N. of H = +1; O.N. of O = -2
• O.N. of C + 2 x 1 + 3 x (-2) = 0 ⇒ O.N. of C = +4

A reducing agent is a substance that is oxidized in a redox reaction. CO (oxidation number of C: +2) becomes CO₂ (oxidation number of C: +4) ⇒ CO is oxidized since the oxidation number of the carbon atom increases.

NaCl (sodium chloride) is a strong electrolyte because it completely dissociates into Na⁺ and Cl^- ions in solution, allowing it to conduct electricity efficiently.

Copper (Cu²⁺) is reduced to Cu (elemental copper) as it gains two electrons in the reaction.

In H₂SO₄, hydrogen has an oxidation number of +1, and oxygen has an oxidation number of -2. The total oxidation number for the compound must be zero. Therefore, the oxidation number of sulfur is x + 4 x (−2) + 2 x (+1) = 0 ⇒ x = +6

This reaction produces AgCl, a solid precipitate, making it a precipitation reaction.