## What is Ostwald dilution law for weak electrolyte?

Answer: Ostwald’s dilution law describes the dissociation constant of the weak electrolyte with the degree of dissociation (α) and the concentration of the weak electrolyte. Ostwald’s dilution law states that only at infinite dilution the weak electrolyte undergoes complete ionization.

### What is Ostwald dilution law formula?

An expression for the degree of dissociation of a weak electrolyte. If α is small compared with 1, then α2 = KV/n; i.e. the degree of dissociation is proportional to the square root of the dilution. The law was first put forward by Wilhelm Ostwald to account for electrical conductivities of electrolyte solutions.

**What happens to weak electrolyte on dilution?**

When more amount of solvent such as water is added to the solution, it results in dissociating the molecules into ions of a weak electrolyte. Thus, the degree of dissociation of weak electrolyte increases upon dilution.

**What is Ostwald’s dilution law What are its uses?**

Ostwald’s Dilution Law tells us that the equilibrium constant, and the initial concentration of an electrolyte (prior to dissociation or association), can be used to calculate the extent of this dissociation or association for the electrolyte.

## What is the principle of dilution?

Dilution refers to the process of adding additional solvent to a solution to decrease its concentration. This process keeps the amount of solute constant, but increases the total amount of solution, thereby decreasing its final concentration.

### Why Ostwald’s dilution law is not applicable for strong electrolyte?

NEET Question. 《》Ostwald Dilution Law. “Degree of dissociation of weak electrolyte is directly proportional to square root of dilution.” This law is not applicable for strong electrolytes because strong electrolytes completely ionize at all dilution…….

**What is the rule of dilution?**

A general rule to use in calculating the concentration of solutions in a series is to multiply the original concentration by the first dilution factor, this by the second dilution factor, this by the third dilution factor, and so on until the final concentration is known. The resulting solution is diluted 1/10.

**Which of the following is a weak electrolyte in aqueous solution?**

HF is the weak electrolyte.

## What is dilution and dilution factor?

A simple dilution is one in which a unit volume of a liquid material of interest is combined with an appropriate volume of a solvent liquid to achieve the desired concentration. The dilution factor is the total number of unit volumes in which your material will be dissolved.

### What are the two components of a dilution?

A dilution solution contains solute (or stock solution) and a solvent (called diluent). These two components proportionally combine to create a dilution. You can identify a dilution solution by the amount of solute in the total volume, expressed as a proportion.

**Which is the correct description of Ostwald’s dilution law?**

State Ostwald’s dilution law. Ostwald’s dilution law describes the dissociation constant of the weak electrolyte with the degree of dissociation (α) and the concentration of the weak electrolyte. A binary electrolyte AB which dissociates into A + and B – ions.

**How is the degree of ionization related to Ostwald’s law?**

The expressions (1) and (2) are known as Ostwald’s dilution law. Where K = equilibrium constant. Thus, the degree of ionization (or dissociation) of any weak electrolyte is inversely proportional to the square root of concentration and directly proportional to the square root of dilution. This relation is known as Ostwald’s law.

## How is the Ka of Ostwald’s law determined?

Ostwald’s law: Ionization constant (Ka) for a weak acid with a concentration (C) can be determined from the relation, Ka = α² × C, where α is the degree of ionization. When a weak acid such as acetic acid with a concentration (C) dissociates in water according to the equation

### How is the dissociation of a weak electrolyte related to the dilution?

The degree of ionization (or dissociation) of any weak electrolyte is inversely proportional to the square root of concentration and directly proportional to the square root of dilution. If α is the degree of dissociation of a weak electrolyte, C is its concentration and V is the dilution.