Intermolecular Forces and Properties

Decreases solubility

Causes precipitation until temperature is decreased

Does not affect solubility

Increases solubility

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.

The compound breaks into Na+ and Cl- ions.

Water molecules break into H+ and OH- ions.

NaCl(s) keeps clustered together without separating.

NaCl(s) reacts with water and forms HCL & NaOH.

liters per mole

kilograms per liter

moles per liter

grams per milliliter

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.

Color of the solid

Size of the solid particles

Stirring speed

Temperature of the solvent

Sodium chloride (NaCl)

Glucose (C6H12O6)

Ethanol (C2H5OH)

Acetic acid (CH3COOH)

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..

Salts are more soluble in polar solvents due to ion-dipole interactions while nonpolar substances are less soluble.

Salts are less soluble in polar solvents because they disrupt hydrogen bonding networks within the solvent.

Solvent polarity has no significant effect on salt dissolution but affects nonpolar substances greatly.

Nonpolar substances dissolve equally well in both polar and nonpolar solvents due to van der Waals forces.