Multiple Choice
Which of the following best describes the process of dissolution in water?
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6. Chemical Quantities & Aqueous Reactions
Solubility Rules
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Which of the following compounds will dissolve most slowly in water due to its low solubility according to common solubility rules?
A
AgCl
B
NH4Br
C
NaNO3
D
K2SO4
Verified step by step guidance1
Recall the common solubility rules for ionic compounds in water, which help predict whether a compound is soluble or insoluble.
Identify the solubility of each compound based on these rules:
- Compounds containing NH4+ (ammonium) are generally soluble.
- Compounds containing NO3- (nitrate) are generally soluble.
- Most salts of K+ (potassium) are soluble.
- Salts containing Ag+ (silver) and Cl- (chloride) are often insoluble or have low solubility, except for some exceptions.
Compare the given compounds: NH4Br, NaNO3, K2SO4, and AgCl. Since NH4Br, NaNO3, and K2SO4 contain ions that form soluble salts, they will dissolve readily in water.
AgCl is known to have low solubility in water because silver chloride is one of the classic examples of an insoluble salt according to solubility rules.
Therefore, based on the solubility rules, AgCl will dissolve most slowly in water due to its low solubility.
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