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MindMap Gallery Chapter 1 Dispersion System

Chapter 1 Dispersion System

This is a mind map about Chapter 1 Dispersion System. The main contents include: composition, liquid, and gas. The knowledge points are summarized and organized, covering all core contents, which is very convenient for everyone to learn. Suitable for exam review and preview to improve learning efficiency. Hurry up and collect it to learn together!

Edited at 2024-10-18 19:46:50

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Chapter 1 Dispersion System

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Outline

Chapter 1 Dispersion System

composition

Dispersant: substance to be dispersed

Dispersoid: a substance that disperses other substances

liquid

Liquid evaporation: liquid molecules break away from the liquid surface and become gas When a liquid molecule wants to escape from the constraints of nearby liquid molecules, The kinetic energy of the molecule must be greater than a certain minimum value E

solution

Composition measure

Quantity concentration c1=n1/V0

Molarity b1=n1/M2

Mole fraction x1=n1/n0

Mass fraction w1=M1/M0

Mass concentration (density) ρ1=M1/V0

colligative properties of dilute solutions

The vapor pressure of a dilute solution drops

Mixing a certain amount of less volatile substances into a pure solvent will cause the vapor pressure of the mixed solution to drop.

Rule: At a certain temperature, the vapor pressure of a dilute solution of a non-volatile non-electrolyte = the saturated vapor pressure of the pure solvent * the mole fraction of the solvent (P0=P1*x1=P1*n1/n0) detP=P1*x2 P1*n2/n0

The boiling point of the solution increases

Refractory non-electrolyte solutions have lower boiling points than pure solvents

The boiling point of a liquid is the temperature of the liquid when the liquid vapor pressure = 101.325kPa

Formula: detT1=K1b2=K1*n1/M2 (increased boiling point of solution = boiling point increase constant of solvent * molar concentration of solute)

Therefore, when the solution boils, the boiling point will continue to increase (the solvent continues to evaporate, causing n0 to decrease)

The freezing point of the solution decreases

Refractory non-electrolyte solutions have a higher freezing point than pure solvents

detTf=Kf*b2=Kf*n2/M2

Among them, Kf is only related to the solvent, and b2 is the molar concentration of the solute.

Osmotic pressure of solution

The solution and the pure solvent are separated by a semipermeable membrane. If an additional pressure is added to the solution to balance the osmosis, this additional pressure is the osmotic pressure.

Formula: The osmotic pressure of the solution is related to the temperature and the concentration of the solution - Π=c2*R*T (concentration of the solute*R*T R=8.314J*mol^-1*K^-1)

diffusion phenomenon

When a semipermeable membrane is used to separate a solution and a pure solvent, the diffusion phenomenon will cause the solvent molecules in the pure solvent to move into the solution at a rate greater than the rate at which the solvent molecules in the solution move toward the pure solvent. This will eventually lead to the liquid levels in the containers on both sides being inconsistent. Even.

Colloidal solution

Definition: A system composed of a dispersion with a particle size of 10^-9~10^-7m

Classification: 1. Multiphase system composed of small molecules, ions, and atoms aggregated into larger particles 2. Solution composed of polymer compounds

Dispersion: measured by specific surface area - s=S/V

Properties: 1. Tyndall effect - a simple way to test colloids 2. Electroosmosis phenomenon - Colloidal particles are weakly charged. Under directional current, the colloidal particles will move directionally and concentrate next to the oppositely charged electrode. 3. Brownian motion

Micelle: composed of colloidal particles and a diffusion layer. The colloidal particles are divided into adsorption layers and colloidal cores. The colloidal cores are usually charged insoluble particles (AgI). The adsorption layer is adsorbed by the colloidal core charges and has an oppositely charged potential. The ions are composed of counterions with the same charge as the colloidal core that are attracted by the excess charge of the potential ions. The diffusion layer is the counter ions adsorbed by the ionic charges in the adsorption layer

Structural formula expression: {(glue core)m-n potential ion-(n-x) counterion}x/x- -x counterion

Stability of sol: Dispersed particles are less affected by the gravity field under Brownian motion and are difficult to aggregate and settle (dynamic stability) The colloidal particles are charged and repel each other without agglomeration (coalescence stability)

coagulation of sol

Reasons: The concentration of sol molecules is too high; the sol is heated for a long time; a strong electrolyte is added; it is shaken and vibrated strongly;...

The agglomeration of sol by strong electrolytes is mainly ions with opposite charge to the colloidal particles. The higher the ionic charge, the greater the effect on sol agglomeration.

Coagulation value: The concentration of electrolyte solution that causes a certain sol to coagulate under certain conditions.

gas

ideal gas equation of state

Conditions of use: low pressure, high temperature environment, between gas molecules The distance is quite far, and the forces between gas molecules have almost no effect , at this time the actual gas can be regarded as an ideal gas.

Formula: pv=nRT

Among them, R=8.314J*mol^-1*K^-1

Dalton's ideal gas partial pressure law

Definition: When multiple gases are mixed, if they do not react chemically with each other Then the pressure generated by the collision of any group of gas molecules is will not be changed by other gas components, it is called the gas component partial pressure.

P1=n1*RT/V

P1/P0=n1/n0

saturated vapor pressure

At a certain temperature, the liquid is placed in a closed container, and a vacuum is drawn above the liquid. The gas molecules above the liquid will increase as the evaporation proceeds, causing the vapor pressure to gradually increase. When the evaporation rate of the liquid is equal to the condensation rate of the gas, the gas molecules in the unit volume above the page The number remains unchanged. The pressure of the vapor when the liquid is in equilibrium with its vapor at this temperature is called the saturated vapor pressure of the liquid at that temperature.