Water Solutions and Solubility Factors

A homogeneous mixture of two or more components, where the components can be liquids, gases, or solids.

The dissolving medium in a solution, usually the major component.

The substance being dissolved in a solution.

A solution where water (H₂O) is the solvent.

The ability of a solute to dissolve in a given solvent.

Similar polarity (both polar or both nonpolar) between solute and solvent creates better solubility.

Solute structure, temperature, and pressure.

A combination of substances that mix evenly and are uniform throughout.

A molecule that does not dissolve in water due to lacking attraction to water molecules.

Polar substances dissolve well in polar solvents, and non-polar substances dissolve well in non-polar solvents. This is due to similar intermolecular forces.

A carboxylic acid with a large non-polar benzene portion, making it insoluble in water.

A carboxylic acid with a smaller non-polar portion, making it soluble in water.

A long-chain carboxylic acid with a polar head (-COOH) and a non-polar hydrocarbon tail.

A spherical structure formed by fatty acids in water, where the hydrophobic tails cluster together and the hydrophilic heads face outward.

A molecule made up of only carbon and hydrogen atoms, typically non-polar.

Soaps are made of fatty acids, which form micelles in water. The hydrophobic tails trap dirt and grease, while the hydrophilic heads interact with water, allowing the dirt to be washed away.

Water is a polar molecule, meaning it has a slightly positive and slightly negative end. This allows it to attract and dissolve other polar molecules and ionic compounds.

Sugars are polar molecules because they contain many polar hydroxyl (OH) groups. This makes them compatible with water's polarity, allowing them to dissolve.

Salts are ionic compounds, meaning they are made up of positively charged ions (cations) and negatively charged ions (anions). Water molecules surround and separate these ions, dissolving the salt.

A non-polar molecule has a balanced distribution of electrons, making it lack a positive and negative end. It doesn't have a strong attraction to water.

Vitamin A is mainly composed of non-polar C-H bonds, making it non-polar. It can only dissolve in other non-polar substances, like fats and oils.

Vitamin C has several polar O-H bonds, making it a polar molecule. These polar bonds attract water molecules, enabling it to dissolve in water.

Hydrophilic means 'water-loving'. Substances that are hydrophilic dissolve easily in water due to their attraction to water molecules.

Hydrophobic means 'water-fearing'. Substances that are hydrophobic don't dissolve in water due to their lack of attraction to water molecules.

Oil, composed largely of C-C and C-H bonds, is a hydrophobic molecule. Its interactions with water are weaker than water-water or water-polar solute interactions, causing it to float rather than mix.

Temperature significantly affects the solubility of solids, liquids, and gases in water. Generally, increasing temperature increases solubility, but there are exceptions.

The solubility of most solids in water increases with increasing temperature. However, specific solids like Na2SO4 and Ce2(SO4)3 exhibit decreased solubility with increasing temperature.

Determining the impact of temperature on solid solubility requires experimental observation. There's no universal prediction, so experiments are essential.

Hydrophobic hydrocarbon tails of molecules cluster together within a micelle, while hydrophilic heads interact with surrounding water.

Micelles form spherical structures where hydrophobic tails are shielded from water by hydrophilic heads, allowing for the solubilization of non-polar substances in water.

A measure of how acidic or basic a solution is. It is a scale ranging from 0 to 14, with 0 being the most acidic and 14 being the most basic.

A solution with a pH value less than 7. It contains a higher concentration of hydrogen ions (H+).

A solution with a pH value greater than 7. It contains a lower concentration of hydrogen ions (H+).

A solution with a pH value of 7. It contains an equal concentration of hydrogen ions (H+) and hydroxide ions (OH-).

Increasing the concentration of hydrogen ions ([H+]) decreases the pH of a solution, making it more acidic.

Decreasing the concentration of hydrogen ions ([H+]) increases the pH of a solution, making it more basic.

Each 1 unit change in pH represents a 10x change in the concentration of hydrogen ions.

The decrease in the pH of ocean water due to the absorption of carbon dioxide (CO2) from the atmosphere.

A logarithmic scale used to express the acidity or basicity of a solution, with a range from 0 to 14. Lower pH values indicate a higher concentration of hydrogen ions (H+), making the solution acidic. Higher pH values indicate a lower concentration of H+, making the solution basic (alkaline). A pH of 7 is considered neutral.

A change in pH by 1 unit represents a tenfold change in the concentration of hydrogen ions (H+). For example, a solution with a pH of 2 is 10 times more acidic than a solution with a pH of 3.

Substances can be classified as acidic, basic (alkaline), or neutral based on their pH. Examples of acidic substances include lemon juice, vinegar, and HCl solutions. Examples of basic substances include soap, NaOH solutions, and seawater. Pure water is considered neutral.

The pH scale provides a convenient way to express acidity or basicity using simple numbers, rather than dealing with extremely large or small concentrations of hydrogen ions (H+).

The pH scale is a logarithmic scale, meaning each whole number change represents a tenfold change in the concentration of hydrogen ions (H+).