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MindMap Gallery electrolyte weak electrolyte ionization

electrolyte weak electrolyte ionization

This is a mind map about the ionization of weak electrolytes. The main contents include: summary and improvement, study method guidance, ionization constant, ionization balance of weak electrolytes, ionization equations, and basic concepts of electrolytes.

Edited at 2024-01-27 16:56:58

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Outline

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electrolyte weak electrolyte ionization

Basic concepts of electrolytes

electrolytes non-electrolytes

electrolyte

Compounds that conduct electricity in aqueous solutions or in the molten state

non-electrolytes

Compounds that do not conduct electricity in aqueous solutions or in the molten state

strong electrolyte weak electrolyte

strong electrolyte

concept

An electrolyte that can completely ionize in an aqueous solution

compound

Strong acids, strong bases, salts (except CH₃COO)₂Pb, HgCl₂), active metal oxides

weak electrolyte

concept

Electrolytes that are only partially ionized in aqueous solutions

compound

Weak acid, weak base, water

conductivity of matter

Elements of matter that can conduct electricity

There are freely moving charges

ionic compounds

It can be completely ionized in both aqueous solution and molten state, producing freely moving positive and negative ions, which can conduct electricity.

Covalent compounds that are electrolytes

Can be ionized in aqueous solution to produce freely moving ions that can conduct electricity

In the molten state, it cannot ionize and cannot conduct electricity.

Metal element

There are free electrons that can conduct electricity

How to judge the conductivity of a solution

Look at the total concentration of positive and negative ions in the solution and the number of charges carried by the ions

Ionization equation

concept

The formula for electrolyte ionization

Writing method

strong electrolyte

Use "=" to connect, such as CaCO₃ = Ca²⁺ CO₃²⁻

weak electrolyte

Use "⇌" to connect, such as CH₃COOH ⇌ H⁺ CH₃COO⁻

Ionization of polybasic weak acids, written step by step: H₂CO₃ ⇌ H⁺ HCO₃⁻, HCO₃⁻ ⇌ H⁺ CO₃²⁻

Multiple weak base ionization, written in one step: Fe(OH)₃ ⇌ Fe³⁺ 3OH⁻

Ionization equilibrium of weak electrolytes

concept

When the rates at which weak electrolyte molecules ionize and ions combine into molecules are equal, The ionization process will reach an equilibrium state, which is called the ionization equilibrium of weak electrolytes.

feature

Reversible

Ionization of weak electrolytes is a reversible process

Endothermic

Ionization of weak electrolytes is an endothermic process

weak

The degree of ionization of weak electrolytes is very weak

Influencing factors

internal cause

The strength of the electrolyte itself (at the same concentration, the stronger the acid (or alkali), the greater the degree of ionization)

external factors

Take a 0.1 mol/L CH₃COOH solution as an example: CH₃COOH ⇌ H⁺ CH₃COO⁻

Three changes that cannot be directly explained by the principle of equilibrium movement

① Add the weak electrolyte to the weak electrolyte solution (without adding water). Although the equilibrium shifts positively, the ionization degree of the weak electrolyte itself decreases.

② Add water to a weak electrolyte solution, the more dilute it is, the more ionized it will be

③ When the weak acid solution is diluted, the concentration of all particles in the solution decreases (except OH⁻); the same is true for the dilution of the weak alkali solution

Ionization constant

concept

At a certain temperature, when a weak electrolyte reaches ionization equilibrium in an aqueous solution, the ratio of the product of the concentration of various ions generated by ionization in the solution to the concentration of unionized molecules is a constant, represented by K (the ionization constant of acids is represented by Kₐ Representation, base is expressed in Kb)

expression

meaning

The ionization constant indicates the degree of ionization of a weak electrolyte. At the same concentration, the greater the value of the ionization constant, the greater the degree of ionization of the weak electrolyte.

Influencing factors

The ionization constant is only affected by temperature and has nothing to do with the concentration of the weak electrolyte; the higher the temperature, the greater the ionization constant

Study guide

Comparison of monobasic strong acid and weak acid

Experimental method to prove weak electrolytes

At the same concentration and temperature, conduct a conductivity comparison experiment with a strong electrolyte. If the conductivity is not as good as that of a strong electrolyte, it is a weak electrolyte.

Determine solution pH

For example, if the measured pH of a 0.1 mol/L HA solution is > 1, then HA is a weak acid.

Determine the acidity and alkalinity of corresponding salt solutions

If the NaA solution is measured to be alkaline, HA is a weak acid

Measure the pH of a solution after dilution

For example, if the HA solution with pH = 2 is diluted 10 times and the pH of the new solution is < 3, then HA is a weak acid.

Prove that there is an ionization equilibrium

For example, if litmus solution is dropped into the HA solution, the solution turns red; then NaA solid is added, If the color of the solution becomes lighter, HA is a weak acid.

key to method

Proves that the electrolyte in the solution is not completely ionized, or there is an ionization equilibrium

Summary and improvement

Learning misunderstandings

Common misunderstandings about electrolytes

Electrolytes and non-electrolytes both refer to compounds

Simple substance

Copper, iron and silver can conduct electricity

Oxygen and nitrogen cannot conduct electricity

mixture

Salt water conducts electricity

Air cannot conduct electricity

Neither electrolyte nor non-electrolyte

Just because an aqueous solution of a substance can conduct electricity does not mean that the substance is an electrolyte

Aqueous solutions of CO₂, SO₂, SO₃, and NH₃ can conduct electricity, but the reason is that these substances react with water first to generate ionizable substances, making the solution conduct electricity. They themselves are still non-electrolytes.

The degree of ionization of the electrolyte is not necessarily related to the conductivity of the solution

The conductivity of a solution depends on the total concentration of ions and the number of ion charges in the solution. In a strong electrolyte solution, the total concentration of ions is not necessarily large (such as 0.0001 mol/L NaCl solution), so the conductivity of a strong electrolyte solution is not necessarily strong.

About aluminum chloride

Covalent compounds in salts include: AlCl₃, (CH₃COO)₂Pb, HgCl₂

The weak electrolytes in salt include: (CH₃COO)₂Pb and HgCl₂

Aluminum chloride is a covalent compound but a strong electrolyte

Common misunderstandings on ionization equations

Understanding of the ionization equation "="

The meaning of "=" in the strong electrolyte ionization equation is: the strong electrolyte dissolved in water is completely ionized, such as: BaSO₄ = Ba²⁺ SO₄²⁻, which means that the BaSO₄ dissolved in water is completely ionized, but does not mean that BaSO₄ is completely soluble in water.

Ionization equation for acid salts

strong acid salt

In aqueous solution, the acid radical of the acid salt of a strong acid is completely ionized NaHSO₄ = Na⁺ H⁺ SO₄²⁻

Weak acid acid salt

In aqueous solution, the acid radical of the weak acid salt is partially ionized NaHCO₃ = Na⁺ HCO₃⁻, HCO₃⁻ ⇌ H⁺ CO₃²⁻

Ionization equation for aluminum hydroxide

Aluminum hydroxide can undergo acid ionization and basic ionization. The ionization equation is written as: H⁺ AlO₂⁻ H₂O ⇌ Al(OH)₃ ⇌ Al³⁺ 3OH⁻

Knowledge improvement

The process of adding water to glacial acetic acid

The electrolyte of a covalent compound can only be ionized in water. There is no water in pure acetic acid, c(H⁺) = 0. After adding water, acetic acid begins to ionize, the equilibrium moves forward, and c(H⁺) increases with the addition of water; and From a limit point of view, when water is added until the acetic acid concentration is very small, c(H⁺) will be very close to 0; therefore, looking at the middle from both ends, the change process of c(H⁺) with the addition of water is 0→ Big → Small (close to 0)

Strong acid to weak acid

The general reaction formula of strong acid to weak acid

strong acid weak acid radical → weak acid strong acid radical

"Strong" and "weak" are not absolutely strong and weak acids. The same two weak acids can also react, such as vinegar for scale removal (reaction of acetic acid and calcium carbonate)

Common weak acids and their acidity

Stronger than carbonic acid

HF, H₂SO₃, CH₃COOH

Weaker than carbonic acid

HClO, H₂S, Al(OH)₃, phenol