Intermolecular Forces and Properties

Decreases solubility

Causes precipitation until temperature is decreased

Does not affect solubility

Increases solubility

75 grams

The mass can't be determined.

50 grams

25 grams

Formation of hydrogen bonds between water molecules after salt dissolution reduces overall motion of solvent molecules..

Decrease in volume due to interaction between Na+ ions with negatively charged oxygen atom on water molecules..

Dispersion of Na+ and Cl- ions throughout the solvent creating more microstates for particles positionally..

Liberation of heat during dissolution leading to increased kinetic energy among solvent molecules..

Solute-solute interactions that are stronger than solute-solvent interactions.

Solute-solvent interactions that mirror the solvent-solvent interactions.

Ideal behavior based on weak, negligible solute-solvent interactions.

Non-ideal behavior indicative of strong solute-solvent interactions.

Ionic bonds strengthen because of increased electrostatic attraction between oppositely charged ions.

London dispersion forces dominate, holding dissolved ions closely together in solution.

Hydration shells form around ions due to water molecules orienting themselves with opposite charges near the ions.

Water molecules break down into hydrogen and oxygen atoms during the dissolution process.

Viscosity decreases due to an error in measurement rather than genuine solution properties.

Decreased viscosity is primarily attributed to temperature fluctuations despite controlled conditions.

Specific ion effects related to structure breaking or making phenomena could account for anomalous behavior.

Uniform salts should not show any change in water viscosity as colligative properties are concentration-based.

Sodium chloride (NaCl)

Glucose (C6H12O6)

Ethanol (C2H5OH)

Acetic acid (CH3COOH)

Fluorine (F), given its high electronegativity, creates a large positive charge on the hydrogen atom.

Oxygen (O), being denser than fluorine, providing a greater pull on the shared electrons toward itself.

Sulfur (S), having a larger radius, is less effective at inducing charges in nearby hydrogen atoms.

Carbon (C), being one of the least electronegative elements listed, making it the weakest donor.

A solute that is dissolved by a solvent

A solvent that dissolves other substances

A substance whose aqueous solution contains ions

A substance that forms a solution containing no ions

Potassium (K), being an alkali metal with high reactivity and propensity to lose one electron easily.

Copper (Cu), as it commonly forms compounds that are not fully dissociated in water.

Silver (Ag), due to its relatively low reactivity compared to other metals and tendency for covalent bonding.

Mercury (Hg), since it tends to form poorly soluble salts limiting ion availability in solution.