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. The molar conductivity is the conductance of all the ions produced by one mole of the electrolyte. Conversely, such electrolytes have lower molar conductivity at higher concentrations due to a reduced degree of dissociation. 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 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 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. For weak electrolytes, however, the molar conductivity shoots at lower concentrations. 665 Views. 1. A. It depends on the type of electrolyte at a given temperature for a given solvent. 2. According to Ostwald’s dilution law K a = \(\frac{\alpha^2C}{1-\alpha}\) Substituting a value in the above equation Strong electrolytes dissociate almost completely in solution, the degree of dissociation … For the strong electrolyte, the molar conductivity increases sharply with increasing concentration. 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. 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 Due to an increase in dilution degree of dissociation increases and which results in an increase in the molar conductivity. 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 Where A is the slope of the plot. The degree of dissociation (α) of a weak electrolyte ,A x B y is related to van't Hoff factor (i) by the expression.

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