Water and Biological Interaction

Water dissolves and transports substances in the body, moves molecules into and out of cells, separates charged molecules, and dissipates heat.

Water is a key substance for dissolving and transporting molecules in living organisms.

Water's polar structure is crucial in its ability to dissolve many biological compounds.

Water molecules have positive and negative ends (poles).

Attractive force between a slightly positive hydrogen atom of one water molecule and a slightly negative oxygen atom of another.

Water is essential for moving molecules into and out of cellular compartments.

Bonding (in water) between hydrogen and oxygen atoms.

The capability of a substance to dissolve in water due to water's polarity.

Oxygen attracts electrons more strongly than hydrogen in a water molecule.

Water helps regulate internal body temperature.

Determining the amount of a solute in a given volume of solution (e.g., molarity).

Understanding the chemical characterization of acids and bases is important in biochemistry.

Ionic substances dissolve in water because water molecules' positive and negative ends attract the positively and negatively charged ions (cations and anions), respectively.

A molecule that can interact with water, meaning it dissolves in water.

A molecule that cannot interact with water, and usually does not dissolve in water.

A molecule with both a polar and a non-polar region.

A homogeneous mixture of two or more substances, where the solvent is the major component and the solute is the minor component.

The ability of a substance to dissolve in a solvent.

The dissolving process depends on the type of solute and solvent, temperature, pressure, and the common ion effect.

Dissolving speed depends on temperature, particle size, and mixing.

The species formed when an acid loses a proton (H+). It has one less proton than the original acid.

A conjugate base is the species formed when an acid donates a proton (H+). It has one less proton than the original acid.

Acids that completely ionize in water, meaning they donate all their protons.

Acids that only partially ionize in water, meaning they donate only some of their protons.

A measure of the acidity or alkalinity of a solution, ranging from 0 to 14. Lower pH values indicate higher acidity, and higher pH values indicate higher alkalinity.

pH is a measure of the concentration of hydrogen ions (H+) in a solution. It is defined as the negative logarithm to the base 10 of the hydrogen ion concentration: pH = -log10[H+].

Solutions that resist changes in pH when small amounts of acid or base are added. They contain a weak acid and its conjugate base (or a weak base and its conjugate acid).

The pH of blood needs to be tightly regulated within a narrow range (7.35-7.45). Buffers play a crucial role in maintaining this.

The weight of a solute in 100 grams of solution. It represents the solute's mass fraction in the solution.

The volume of a solute in 100 milliliters of solution. It represents the solute's volume fraction in the solution.

The weight of a solute in 100 milliliters of solution. It measures the solute's mass relative to the solution's volume.

The number of moles of solute dissolved in 1 liter of solution. It's a measure of solute concentration.

A substance that can donate hydrogen ions (protons) when dissolved in a solution. It increases the concentration of H+ ions in a solution.

A substance that can accept hydrogen ions (protons) when dissolved in a solution. It reduces the concentration of H+ ions in a solution.

A molecule that can act as both an acid and a base, depending on the chemical environment.

The process where an acid releases a proton (H+) and becomes a base (called its conjugate base).