18 Questions
In which type of solvent do non-polar solutes dissolve?
Non-polar solvents
What happens if the forces of attraction between solute molecules (A-A) are greater than the forces between solvent molecules (B-B)?
The solvent will not be able to break the binding forces of the solute molecules.
Which type of forces hold the sodium chloride crystal together?
Electrovalent forces
In which type of solvent do non-electrolytes typically dissolve?
Polar solvents
What happens if B-B > A-B, according to the text?
The solvent molecules will form aggregations excluding the solute.
Which step involves creating a hole in the solvent just large enough to accept the solute molecule?
Step 2: Creation of a hole in the solvent
Which type of forces are stronger if A-B > A-A or B-B?
A-B forces
'Steps of Solubility' mentioned in the text involve which of the following first?
'The removal of a molecule from the solute phase'
In which scenario will the solute disperse and form a solution?
A-B > A-A
If the solvent molecules are attracted to each other and form aggregations from which the solute is excluded, what does it signify?
B-B > A-B
What type of solvent would benzene be classified as based on its inability to penetrate closely bound water aggregates?
Non-polar solvent
Which forces are holding the sodium chloride crystal together, making it insoluble in benzene?
A-A forces
What is the first step in the process of solubility described in the text?
Removal of a molecule from the solute phase
What happens if B-B exceeds A-B in terms of their affinities?
The solvent molecules form aggregations excluding the solute.
If A-A > B-B, what happens to the solute in the solvent?
It remains insoluble.
Based on the text, what characteristic defines non-polar solvents?
They can form aggregations excluding certain solutes.
When A-B exceeds A-A and B-B, what happens to the solute?
It disperses and forms a solution.
Which step in the process of solubility deals with placing the solute molecule in a hole in the solvent?
Third step
Study Notes
Electrolytes and Non-Electrolytes
- Electrolytes are substances that dissolve in water and yield ions (cations and anions)
- Types of electrolytes: • Strong electrolytes (e.g., HCl, NaOH, NaCl) that ionize completely (100%) • Slightly soluble electrolytes (e.g., AgCl, AgI) • Weak electrolytes (e.g., acetic acid, ammonia) that ionize partially (1-10%)
- Non-electrolytes are substances that dissolve in water but do not yield ions (e.g., sucrose, urea, glycerin)
Solvents
- Solvents are dispersion media or solution components present in large excess
- Types of solvents: • Polar solvents (e.g., water, glycerol) with high dielectric constants, dissolving ionic solutes • Semi-polar solvents (e.g., n-propanol, acetone) acting as intermediate solvents for miscibility • Non-polar solvents (e.g., benzene, chloroform) unable to reduce attraction between ions due to low dielectric constants
Solubility
- Solubility is the concentration of the solute in a saturated solution at a certain temperature and pressure
- Maximum amount of solute that can dissolve in a solvent under specific conditions
- Expressed in terms of mass of solute per volume of solvent (e.g., grams per liter)
Solubility Expressions
- USP (United States Pharmacopeia) descriptions for solubility: • Very soluble: less than 1 part of solvent required for 1 part of solute • Freely soluble: 1-10 parts of solvent required for 1 part of solute • Soluble: 10-30 parts of solvent required for 1 part of solute • Sparingly soluble: 30-100 parts of solvent required for 1 part of solute • Slightly soluble: 100-1000 parts of solvent required for 1 part of solute • Very slightly soluble: 1000-10,000 parts of solvent required for 1 part of solute • Practically insoluble: more than 10,000 parts of solvent required for 1 part of solute
Test your knowledge on electrolytes, weak acids, weak bases, strong electrolytes, and non-electrolytes. Understand the differences between substances that ionize completely and partially, and those that dissolve as molecules in solutions.
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