Calculate pH of 0.02 M- HA solution. Ka for HA=2 ×10^-12 .(log2=0.3 log3=0.48 ) (a) 6.65 (b) 6.7

step 1 Hello everyone, so in this question the pH of the solution is 0 .02 molar of an acid the KA for

Calculate pH of 0.02 M- HA solution. Ka for HA=2 ×10^-12...

Key Concepts

Weak Acid Equilibrium

A weak acid does not completely dissociate in solution, resulting in an equilibrium between the undissociated acid and the ions produced. The extent of this dissociation is governed by the acid's dissociation constant, meaning that only a small fraction of the acid converts to its ionic forms.

Acid Dissociation Constant (Ka)

The acid dissociation constant, Ka, quantifies the strength of a weak acid by describing the equilibrium between the undissociated acid and its ions in solution. It is calculated from the ratio of the concentrations of the products to the reactant, and a very small Ka indicates a very weak acid with minimal dissociation.

Equilibrium Approximations in Weak Acid Dissociation

For weak acids with very small Ka values, the amount that dissociates is extremely small compared to the initial concentration. This allows the approximation that the equilibrium concentration of the undissociated acid remains nearly equal to its initial concentration, simplifying the computation of ion concentrations and pH calculations.

pH Calculation

The pH of a solution is determined by the concentration of hydrogen ions, calculated as the negative logarithm of this concentration. In the context of weak acid equilibria, pH calculations involve first finding the hydrogen ion concentration from the acid dissociation equilibrium and then applying the pH definition to obtain the final value.

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