Multiple Choice
For which of the following aqueous solutions will a decrease in pH increase the solubility of the compound?
2
views
6. Chemical Quantities & Aqueous Reactions
Solubility Rules
Struggling with General Chemistry?
Join thousands of students who trust us to help them ace their exams!Watch the first videoMultiple Choice
Which of the following interactions and processes primarily contribute to the dissolution of ionic compounds in water?
A
Hydrogen bonding between the ions themselves
B
London dispersion forces between ions and water molecules
C
Ion-dipole interactions between water molecules and ions, and the hydration process
D
Covalent bonding between ions and water molecules
Verified step by step guidance1
Understand that ionic compounds dissolve in water primarily due to interactions between the charged ions and the polar water molecules.
Recognize that water is a polar molecule with a partial positive charge on hydrogen atoms and a partial negative charge on the oxygen atom, enabling it to interact with ions.
Identify that the key interaction responsible for dissolution is the ion-dipole interaction, where the positive or negative ions attract the opposite partial charge on water molecules.
Know that this ion-dipole interaction leads to the hydration process, where water molecules surround and stabilize the ions, preventing them from recombining into a solid.
Eliminate other options such as hydrogen bonding between ions (which do not form hydrogen bonds), London dispersion forces (which are weak and non-specific), and covalent bonding (which does not occur between ions and water in this context).
2:07mWatch next
Master Solubility and Insolubility with a bite sized video explanation from Jules
Start learningRelated Videos
Related Practice
Solubility Rules practice set
Problem sets built by lead tutorsExpert video explanations