The compound in question is potassium sulfate, which has the chemical formula \( \text{K}_2\text{SO}_4 \).
Step 2: Apply solubility rules
According to general solubility rules for ionic compounds in water:
Compounds containing alkali metal ions (such as potassium, \( \text{K}^+ \)) are generally soluble.
Sulfates (\( \text{SO}_4^{2-} \)) are generally soluble, with some exceptions (e.g., \( \text{BaSO}_4 \), \( \text{PbSO}_4 \), \( \text{CaSO}_4 \)).
Step 3: Determine solubility
Since \( \text{K}_2\text{SO}_4 \) contains the potassium ion, which is an alkali metal ion, it follows the rule that compounds with alkali metal ions are soluble.