Multiple Choice
Which of the following best indicates that a solution is saturated?
69
views
6. Chemical Quantities & Aqueous Reactions
Solubility Rules
Multiple Choice
Which of the following compounds would you expect to have poor solubility in water?
A
AgCl
B
NaNO3
C
NH4Br
D
K2SO4
Verified step by step guidance1
Step 1: Understand the concept of solubility in water, which is largely influenced by the ionic nature of the compound and the strength of the ionic bonds. Water is a polar solvent, so ionic compounds that dissociate easily into ions tend to be soluble.
Step 2: Recall the solubility rules for common ionic compounds in water. For example, most nitrates (NO\_3\^-), ammonium (NH\_4\^+), and alkali metal salts (like K\^+) are generally soluble in water.
Step 3: Analyze each compound based on these rules: NaNO\_3 contains the nitrate ion, which is highly soluble; NH\_4Br contains ammonium and bromide ions, both of which form soluble salts; K\_2SO\_4 contains potassium and sulfate ions, and potassium salts are usually soluble.
Step 4: Consider AgCl, which contains silver (Ag\^+) and chloride (Cl\^-). According to solubility rules, most silver salts are poorly soluble in water, especially silver chloride, which is known to be sparingly soluble.
Step 5: Conclude that AgCl is expected to have poor solubility in water compared to the other compounds listed, based on the solubility rules and the nature of the ions involved.
Related Videos
Related Practice
