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Physical & Chemical properties

## Dissociation constant

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##### Reference
Endpoint:
dissociation constant
Type of information:
calculation (if not (Q)SAR)
key study
Study period:
2012-07-02
Reliability:
1 (reliable without restriction)
Qualifier:
no guideline followed
Principles of method if other than guideline:
The available data was calculated from the solubility product of the correspondent substance.
Dissociating properties:
yes
No.:
#1
pKa:
ca. 2.34
Temp.:
25 °C
Remarks on result:
other: Calculation basis: study result on water solubility (no pKa but pKsp; sp = solubility product)
Conclusions:
Ksp for lithium nitrate could be calculated to 218.87 mol^2/L^2. Expressed in a logarithmic form the Ksp is log Ksp = 2.34.
Executive summary:

The solubility equilibrium of lithium nitrate exists when the chemical compound in the solid state is in chemical equilibrium with a solution of that compound. The equilibrium is an example of dynamic equilibrium in that some individual molecules migrate between the solid and solution phases such that the rates of dissolution and precipitation are equal to one another. When equilibrium is established, the solution is saturated. The concentration of the solute in a saturated solution is known as the solubility. Dissolution with dissociation is a characteristic of salts like lithium nitrate. Thus, one type of solubility equilibrium is the reversible dissolution with dissociation. Lithium nitrate dissociates in its constituent ions when it is dissolving in water:

LiNO3(s) <=> Li+(aq) +NO3-(aq)

The corresponding solubility product Ksp is expressed as:

Ksp= [Li+]*[ NO3-]

The relation between the solubility S and the solubility product Ksp of a salt AmBn like lithium nitrate is as follows:

S = (Ksp/(m^m * n^n))^(1/(m+n))

m = 1

n = 1

As the solubility S of lithium nitrate at 25 °C is 1020 g/L, the solubility product Ksp could be calculated to be 218.87 mol2/L2. Expressed in a logarithmic form, the Ksp log10 value is 2.34.

### Description of key information

Ksp for lithium nitrate could be calculated to be 218.87 mol^2/L^2. Expressed in a logarithmic form the Ksp is log Ksp = 2.34.

### Key value for chemical safety assessment

pKa at 20°C:
2.34

The solubility equilibrium of lithium nitrate exists when the chemical compound in the solid state is in chemical equilibrium with a solution of that compound. The equilibrium is an example of dynamic equilibrium in that some individual molecules migrate between the solid and solution phases such that the rates of dissolution and precipitation are equal to one another. When equilibrium is established, the solution is saturated. The concentration of the solute in a saturated solution is known as the solubility. Dissolution with dissociation is a characteristic of salts like lithium nitrate. Thus, one type of solubility equilibrium is the reversible dissolution with dissociation. Lithium nitrate dissociates in its constituent ions when it is dissolving in water:

LiNO3(s) <=> Li+(aq) +NO3-(aq)

The corresponding solubility product Ksp is expressed as:

Ksp= [Li+]*[ NO3-]

The relation between the solubility S and the solubility product Ksp of a salt AmBn like lithium nitrate is as follows:

S = (Ksp/(m^m * n^n))^(1/(m+n))

m = 1

n = 1

As the solubility S of lithium nitrate at 25 °C is 1020 g/L the solubility product Ksp could be calculated to 218.87 mol2/L2. Expressed in a logarithmic form the Ksp log10 value is 2.34.