Electrolytes and Non-Electrolytes Quiz

In which type of solvent do non-polar solutes dissolve?

What happens if the forces of attraction between solute molecules (A-A) are greater than the forces between solvent molecules (B-B)?

Which type of forces hold the sodium chloride crystal together?

In which type of solvent do non-electrolytes typically dissolve?

What happens if B-B > A-B, according to the text?

Which step involves creating a hole in the solvent just large enough to accept the solute molecule?

Which type of forces are stronger if A-B > A-A or B-B?

'Steps of Solubility' mentioned in the text involve which of the following first?

In which scenario will the solute disperse and form a solution?

If the solvent molecules are attracted to each other and form aggregations from which the solute is excluded, what does it signify?

What type of solvent would benzene be classified as based on its inability to penetrate closely bound water aggregates?

Which forces are holding the sodium chloride crystal together, making it insoluble in benzene?

What is the first step in the process of solubility described in the text?

What happens if B-B exceeds A-B in terms of their affinities?

If A-A > B-B, what happens to the solute in the solvent?

Based on the text, what characteristic defines non-polar solvents?

When A-B exceeds A-A and B-B, what happens to the solute?

Which step in the process of solubility deals with placing the solute molecule in a hole in the solvent?

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 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 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)

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