Question

write the relative between degree of dissociation and dissociation constant Ka of weak acid​

Answer 1

Explanation:

degree of dissociation(α):

[H+]=Cα2

Ka=Cα2

α=√Ka/C

Answer 2

Answer:

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Explanation:

It is defined as the fraction (or percentage) of the total salt which is hydrolysed at equilibrium. For example, if 90% of a salt solution is hydrolysed, its degree of hydrolysis is 0.90 or as 90%. It is generally represented by ‘h’.

• It is defined as the fraction (or percentage) of the total salt which is hydrolysed at equilibrium. For example, if 90% of a salt solution is hydrolysed, its degree of hydrolysis is 0.90 or as 90%. It is generally represented by ‘h’.Salts of strong acids and strong bases do not undergo hydrolysis (they undergo only ionization) hence the resulting aqueous solution is neutral.

It is defined as the fraction (or percentage) of the total salt which is hydrolysed at equilibrium. For example, if 90% of a salt solution is hydrolysed, its degree of hydrolysis is 0.90 or as 90%. It is generally represented by ‘h’.Salts of strong acids and strong bases do not undergo hydrolysis (they undergo only ionization) hence the resulting aqueous solution is neutral.ACID DISSOCIATION CONSTANT

• It is defined as the fraction (or percentage) of the total salt which is hydrolysed at equilibrium. For example, if 90% of a salt solution is hydrolysed, its degree of hydrolysis is 0.90 or as 90%. It is generally represented by ‘h’.Salts of strong acids and strong bases do not undergo hydrolysis (they undergo only ionization) hence the resulting aqueous solution is neutral.ACID DISSOCIATION CONSTANTThe acid dissociation constant is the equilibrium constant of the dissociation constant of an acid and is denoted by Ka. This equilibrium constant is a quantitative measure of the strength of an acid in a solution. Ka is commonly expressed in units of mol/L. There are tables for acid dissociation constant, for easy reference. For an aqueous solution, the general form of the equilibrium reaction is:

• It is defined as the fraction (or percentage) of the total salt which is hydrolysed at equilibrium. For example, if 90% of a salt solution is hydrolysed, its degree of hydrolysis is 0.90 or as 90%. It is generally represented by ‘h’.Salts of strong acids and strong bases do not undergo hydrolysis (they undergo only ionization) hence the resulting aqueous solution is neutral.ACID DISSOCIATION CONSTANTThe acid dissociation constant is the equilibrium constant of the dissociation constant of an acid and is denoted by Ka. This equilibrium constant is a quantitative measure of the strength of an acid in a solution. Ka is commonly expressed in units of mol/L. There are tables for acid dissociation constant, for easy reference. For an aqueous solution, the general form of the equilibrium reaction is:HA + H2O ⇆ A- + H3O+

It is defined as the fraction (or percentage) of the total salt which is hydrolysed at equilibrium. For example, if 90% of a salt solution is hydrolysed, its degree of hydrolysis is 0.90 or as 90%. It is generally represented by ‘h’.Salts of strong acids and strong bases do not undergo hydrolysis (they undergo only ionization) hence the resulting aqueous solution is neutral.ACID DISSOCIATION CONSTANTThe acid dissociation constant is the equilibrium constant of the dissociation constant of an acid and is denoted by Ka. This equilibrium constant is a quantitative measure of the strength of an acid in a solution. Ka is commonly expressed in units of mol/L. There are tables for acid dissociation constant, for easy reference. For an aqueous solution, the general form of the equilibrium reaction is:HA + H2O ⇆ A- + H3O+where HA is an acid which dissociates in the conjugate base of the acid A- and a hydrogen ion that combines with water to form the hydronium ion H3O+. When the concentrations of HA, A-, and H3O+ no longer change over time, the reaction is at equilibrium and the dissociation constant may be calculated:

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