If you know the degree of dissociation (which can also be calculated by Kohlrausch’s law), the dissociation constant for weak electrolyte at specific concentration of the solution can be calculated by using following formula-\[{K_c} = \frac{{C{a^2}}}{{1 - \alpha }}\] Where K = dissociation constant C = concentration of the solution Degree of dissociation of weak electrolyte formula Ask for details ; Follow Report by Indusati488 01.10.2019 Log in to add a comment Calculate its degree of dissociation and dissociation constant. Strong electrolytes dissociate almost completely in solution, the degree of dissociation … For the strong electrolyte, the molar conductivity increases sharply with increasing concentration. For weak electrolytes, however, the molar conductivity shoots at lower concentrations. Conversely, such electrolytes have lower molar conductivity at higher concentrations due to a reduced degree of dissociation. It depends on the type of electrolyte at a given temperature for a given solvent. The concept of the degree of electrolytic dissociation made it possible to divide electrolytes into weak and strong, but this is somewhat arbitrary, since the degree of dissociation depends on the concentration. The degree of dissociation (α) of a weak electrolyte ,A x B y is related to van't Hoff factor (i) by the expression. In a solution of any electrolyte there is an equilibrium between the free ions (cations and anions), on the one hand, and undissociated molecules (CatAn), on the other hand, one Due to an increase in dilution degree of dissociation increases and which results in an increase in the molar conductivity. 2. 665 Views. The degree of dissociation of weak electrolyte can be calculated from the molar conductivity at a given concentration and the molar conductivity in infinite dilution using the formula. Electrolyte Power Degree of dissociation (α) depends on electrolyte concentration and usually decreases with increase in concentration. The degree of dissociation of a weak electrolyte AxBy is related to van t Hoff factor i by the expression A. According to Ostwald’s dilution law K a = \(\frac{\alpha^2C}{1-\alpha}\) Substituting a value in the above equation The molar conductivity is the conductance of all the ions produced by one mole of the electrolyte. A strong electrolyte has a high degree of dissociation (ionisation) in solution: For a strong electrolyte which is made up of a salt with the formula MX dissolving in water: MX (aq) ⇋ M + (aq) + X-(aq) the equilibrium position lies very far to the right, there are many ions in solution 1. Where A is the slope of the plot.

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