Chapter 9:Solutions

Electrolyte

________ is a substance that produces ions and therefore conducts electricity when dissolved in water.

Henrys law

According to ________, the solubility (or concentration) of a gas in a liquid is directly proportional to the partial pressure of the gas over the liquid.

Nonelectrolyte

________: A substance that does not produce ions when dissolved in water.

Semipermeable membranes

________ allow water and other small molecules to pass through, but they block the passage of large solute molecules or ions.

isotonic solution

Blood is diverted from the body and pumped through a long cellophane dialysis tube suspended in a(n) ________ formulated to contain many of the same components as blood plasma.

Osmosis

________ occurs when a solution is separated from a pure solvent by a semipermeable membrane.

Molarity

________ (M) is the number of moles of solute dissolved per litre of solution.

Vapor pressure

________ is lower for a solution than for a pure solvent.

Solubility

________ is the maximum amount of a substance that will dissolve in a given amount of solvent at a specified temperature.

Miscible

________ means mutually soluble in all proportions.

Solute

________: A substance that is dissolved in a solvent.

Solids

________ that are more soluble at high temperature than at low temperature can sometimes form supersaturated solutions, which contain even more solute than a saturated solution.

→Hypertonic solutions

________ have an osmolarity greater than the surrounding blood plasma or cells.

Weak electrolyte

________: A substance that is only partly ionized in water.

pure solvent

Freezing point is lower for a solution than for a(n) ________.

Solvation

________: The clustering of solvent molecules around a dissolved solute molecule or ion.

Osmotic pressure

________: The amount of external pressure that must be applied to a solution to prevent the net movement of solvent molecules across a semipermeable membrane.

Homogeneous mixtures

________ are further classified as either solutions or colloids, according to the size of their particles.

Mixtures

________ can be classified as either heterogeneous or homogeneous, depending on their appearance.

Strong electrolyte

________: A substance that ionizes completely when dissolved in water.

→Hypotonic solutions

________ have an osmolarity less than the surrounding blood plasma or cells.

Colligative properties

________: properties that depend on the concentration of a dissolved solute but not on its chemical identity.

Osmosis

________ is the passage of solvent through a semipermeable membrane separating two solutions of different concentration.

pure solvent

Boiling point is higher for a solution than for a(n) ________.

Solvent

________: The substance in which another substance (the solute) is dissolved.

Solute

A substance that is dissolved in a solvent

Solvent

The substance in which another substance (the solute) is dissolved

Solvation

The clustering of solvent molecules around a dissolved solute molecule or ion

Mass/mass percent concentration

Concentration expressed as the number of grams of solute per 100 g of solution

Volume/volume percent concentration

Concentration expressed as the number of milliliters of solute dissolved in 100 mL of solution

mass/volume percent concentration

Concentration expressed as the number of grams of solute per 100 mL of solution

Parts per million (ppm)

Number of parts per one million 10^6 parts

Dilution factor

The ratio of the initial and final solution volumes

Strong electrolyte

A substance that ionizes completely when dissolved in water

Weak electrolyte

A substance that is only partly ionized in water

Nonelectrolyte

A substance that does not produce ions when dissolved in water

Colligative properties

properties that depend on the concentration of a dissolved solute but not on its chemical identity

→The phenomenon of osmosis

A solution inside the bulb is separated from pure solvent in the outer container by a semipermeable membrane

Osmotic pressure

The amount of external pressure that must be applied to a solution to prevent the net movement of solvent molecules across a semipermeable membrane

Osmolarity

The sum of the molarities of all dissolved particles in 1.0 litre of solution