Chemistry Solutions and States of Matter Quiz

A Brønsted-Lowry base is a substance that accepts a proton (H+).

A conjugate acid-base pair consists of two species that differ by a single proton. In the reaction, HC2O4- acts as an acid, donating a proton to form C2O42-, its conjugate base. H2O acts as a base, accepting a proton to form H3O+, its conjugate acid.

A Lewis acid is an electron pair acceptor. In the reaction, AlCl3 accepts a lone pair of electrons from Cl- to form AlCl4-.

The conjugate base of HCO3- is formed by removing one proton from the molecule.

A Lewis base is an electron pair donor.

A mixture where one substance is dissolved completely into another, like salt dissolving in water.

A mixture where two or more solids are combined, like in bronze (copper and tin).

A mixture where a gas is dissolved in a liquid, like carbon dioxide in soda.

A mixture where two liquids combine, like water and alcohol.

A mixture where a gas is dissolved in another gas, like the air we breathe (nitrogen and oxygen).

A gas is a state of matter that has no fixed shape or volume. It takes the shape of its container and expands to fill the entire space.

A liquid is a state of matter that has a fixed volume but no fixed shape. It takes the shape of its container but cannot expand to fill the entire space.

Air is a mixture of gases, primarily nitrogen and oxygen.

Water is a liquid at room temperature.

Acetone, ethanol, and water are all examples of liquids.

A solid substance that dissolves completely in a liquid solvent.

A mixture where one substance of microscopically dispersed insoluble particles is suspended throughout another substance.

Milk, jelly, and muddy water are all examples of colloids.

Light can pass through a colloid, but the particles scatter the light, making the path visible.

A colloid consists of two parts: a dispersed phase (the tiny particles) and a dispersing medium (the substance in which the particles are suspended).

A colloid is a mixture where the particles are evenly distributed throughout the medium but not dissolved.

A temporary attractive force that arises between molecules due to temporary fluctuations in electron distribution, making them weakly attracted to each other.

A mixture where two substances do not mix uniformly, forming distinct layers. For example, oil and water.

A mixture where two substances mix completely, forming a homogeneous solution. For example, water and alcohol.

The rule that states that substances with similar polarities dissolve in each other. Polar solvents dissolve polar solutes, and nonpolar solvents dissolve nonpolar solutes.

A type of intermolecular force arising from temporary fluctuations in electron distribution around atoms or molecules. These forces are weaker than dipole-dipole forces and hydrogen bonding.

The ability of a substance to dissolve in another substance. How much can one substance dissolve in another?

A homogeneous mixture is a type of mixture where the components are evenly distributed throughout the mixture. The substances in a homogeneous mixture are indistinguishable from one another.

In a solution, one substance dissolves completely into another. The substance that dissolves is called the solute, and the substance it dissolves in is the solvent.

The rate at which a solid dissolves in a liquid is called the rate of dissolution. This rate depends on several factors. One key factor is the surface area of the solid. The bigger the surface area, the faster the dissolution.

Miscibility refers to the ability of two liquids to mix together and form a homogeneous solution. Liquids that are miscible mix in any proportion, while liquids that are immiscible do not mix.

A gas-liquid solution is a type of solution where a gas dissolves in a liquid. A common example is carbon dioxide dissolved in water, creating soda water.

An ideal solution is a hypothetical solution where the interactions between the molecules of the solute and solvent are identical to the interactions between like molecules. This leads to no change in volume or enthalpy upon mixing.

Raoult's Law states that the partial vapor pressure of a component in an ideal solution is equal to the vapor pressure of the pure component multiplied by its mole fraction in the solution.

The mole fraction of a solute is the ratio of the number of moles of the solute to the total number of moles in the solution.

A positive deviation from Raoult's Law occurs when the vapor pressure of the solution is higher than predicted by Raoult's Law. This happens when the interactions between the solute and solvent molecules are weaker than those between the molecules of the pure components.

A negative deviation from Raoult's Law occurs when the vapor pressure of the solution is lower than predicted by Raoult's Law. This happens when the interactions between the solute and solvent molecules are stronger than those between the molecules of the pure components.

In chemistry, the rate of dissolution is how quickly a solid solute dissolves in a liquid solvent. Various factors affect this rate, including the intermolecular forces between the solute and solvent molecules. If these interactions are strong, the rate of dissolution is likely to be faster.

The surface area of a solid solute is the total area of its exposed surfaces. A larger surface area allows for more contact points between the solvent and the solute, which increases the rate of dissolution. Imagine a sugar cube versus powdered sugar; the powder will dissolve faster because its surface area is much larger.

This law describes a direct relationship between the pressure of a gas and its solubility in a liquid. In simpler terms, higher pressure forces more gas molecules into the liquid, increasing its solubility. Think about how soda fizzes when you open the bottle; the pressure is released, and the gas escapes, decreasing its solubility.

Non-volatile solutes have a very low vapor pressure, meaning they don't readily evaporate. When such a solute is added to a solvent, it disrupts the solvent molecules' ability to escape into the gas phase. Therefore, the vapor pressure of the solvent decreases. Think of a salt solution; the salt doesn't evaporate as easily, making the solution less likely to evaporate compared to just water.