Doro Acetic Acid Concepts

This video tutorial explains how to calculate the acid ionization constant (KA) for a weak acid. It covers four main steps: converting pH to hydronium ion concentration, writing the ionization equation, using an ICE table to find equilibrium concentrations, and calculating the KA value. The tutorial uses a 2 mol solution of Doro acetic acid with a pH of 1.13 as an example, demonstrating the process of determining the KA value through detailed calculations and explanations.

What is the initial concentration of Doro acetic acid given in the problem?

• 3 mol

• 0.5 mol

• 2 mol

• 1 mol

Which formula is used to convert pH to hydronium ion concentration?

• Ka = [H+][A-]/[HA]

• pH = pKa + log([A-]/[HA])

• [H3O+] = 10^(-pH)

• pH = -log[H+]

What is the hydronium ion concentration when the pH is 1.13?

• 0.00741 M

• 0.0741 M

• 0.741 M

• 7.41 M

What is the conjugate base of Doro acetic acid?

• CH3COO-

• CHCl3COO-

• CHCl2COO-

• CHCl2COOH

In the ICE table, what is the initial concentration of the Doro acetate ion?

• 0 M

• 0.741 M

• 2 M

• 1 M

How does the concentration of Doro acetic acid change during ionization?

• It remains constant

• It doubles

• It decreases

• It increases

What is the equilibrium concentration of hydronium ions?

• 0.741 M

• 0.0741 M

• 2 M

• 1.259 M

What is the expression for the acid ionization constant (Ka)?

• [H3O+][A-]/[HA]

• [HA]/[H3O+][A-]

• [H3O+]/[A-][HA]

• [A-]/[H3O+][HA]

What is the calculated value of Ka for Doro acetic acid?

• 4.4 x 10^-4

• 4.4 x 10^-2

• 4.4 x 10^-3

• 4.4 x 10^-1

Why is the final answer rounded to two significant figures?

• Because the pH was given to two decimal places

• Because the concentration was given to two decimal places

• Because the Ka value is always rounded to two significant figures

• Because the ICE table requires it