To classify the salts, we need to consider the nature of the ions that make up each salt and how they affect the pH when dissolved in water.
1. LiBr (Lithium Bromide)
LiBr is formed from a strong base (LiOH) and a strong acid (HBr). The resulting solution of LiBr is neutral, so we classify LiBr as neutral.
2. NaF (Sodium Fluoride)
NaF consists of a strong base (NaOH) and a weak acid (HF). The fluoride ion (F–) will hydrolyze in water to produce some hydroxide ions, leading to a basic solution. Thus, NaF is classified as basic.
3. NH4ClO4 (Ammonium Perchlorate)
NH4ClO4 is made up of a weak base (NH4OH) and a strong acid (HClO4). The ammonium ion (NH4+) can donate protons (H+) to water, resulting in a slightly acidic solution. Therefore, NH4ClO4 is classified as acidic.
4. K3PO4 (Potassium Phosphate)
K3PO4 originates from a strong base (KOH) and a weak acid (H3PO4). The phosphate ion (PO43-) tends to accept protons, leading to a basic solution. Hence, K3PO4 is classified as basic.
5. KCl (Potassium Chloride)
KCl is produced from a strong base (KOH) and a strong acid (HCl). The solution of KCl remains neutral upon dissolution. Therefore, KCl is classified as neutral.
To summarize:
- LiBr – Neutral
- NaF – Basic
- NH4ClO4 – Acidic
- K3PO4 – Basic
- KCl – Neutral