La constante de disociación ácida del ácido hipocloroso...

La constante de disociación ácida del ácido hipocloroso (HClO) es de $3.0 \times 10^{-8}$. Calcule las concentraciones de $\mathrm{H}_3 \mathrm{O}^{+}, \mathrm{ClO}^{-}$y $\mathrm{HClO}$ al equilibrio si la concentración inicial de $\mathrm{HClO}$ es $0.0075 \mathrm{M}$.

Key Concepts

Acid Dissociation Constant (Ka)

The acid dissociation constant is a quantitative measure of the strength of an acid in solution. It is defined by the equilibrium concentrations of the products and reactants in the acid’s ionization reaction and indicates the extent to which the acid donates protons. A lower Ka value means the acid is weak and dissociates to a small extent in water.

Chemical Equilibrium

Chemical equilibrium refers to the state in which the rates of the forward and reverse reactions are equal, so that the concentrations of reactants and products remain constant over time. In the context of acid-base reactions, reaching equilibrium means that the formation of hydronium and conjugate base ions balances the reformation of the undissociated acid.

ICE Table Analysis

The ICE (Initial, Change, Equilibrium) table is a systematic method used to organize and calculate the concentrations of species in a reaction that has reached equilibrium. This method helps in visualizing the initial concentrations, the changes that occur as the reaction proceeds, and the final equilibrium concentrations, which is particularly useful in equilibrium calculations for weak acids.

Small x Approximation

The small x approximation is an assumption used in equilibrium calculations for weak acids when the degree of dissociation is minimal compared to the initial concentration. This simplification allows one to approximate changes in concentration (denoted as x) as being negligible relative to the starting concentration, making the algebra easier to solve without significantly affecting accuracy.

Transcript

Please give Ace some feedback