Final answer:
The percent ionization of nicotinic acid in a 0.10 M solution is 0.014%.
To find the percent ionization of a 0.10 M nicotinic acid solution, use its Ka value to create an ICE table, solve for the hydrogen ion concentration at equilibrium, and apply the percent ionization formula related to the concentration of ionized acid.
Step-by-step explanation:
The percent ionization of a weak acid can be calculated using the equation: percent ionization = (Ka / [acid]) * 100, where Ka is the acid dissociation constant and [acid] is the concentration of the acid. In this case, the Ka of nicotinic acid is 1.4 x 10⁻⁵ and the concentration of the solution is 0.10 M. Plugging in the values, we get: percent ionization = (1.4 x 10⁻⁵ / 0.10) * 100 = 0.014%.
To find the percent ionization of a 0.10 M nicotinic acid solution, use its Ka value to create an ICE table, solve for the hydrogen ion concentration at equilibrium, and apply the percent ionization formula related to the concentration of ionized acid.
To calculate the percent ionization of nicotinic acid in a 0.10 M solution, we first need to understand that percent ionization is a measure of the extent to which a weak acid ionizes in a solution. We use the acid dissociation constant, Ka, and the initial concentration of the acid to find the equilibrium concentration of the hydrogen ions (H+) and the conjugate base. For nicotinic acid with a Ka of 1.4 x 10⁻⁵, we set up an ICE (Initial, Change, Equilibrium) table to solve for the equilibrium concentrations. Given that the initial concentration of nicotinic acid is 0.10 M and assuming that x represents the concentration of H+ at equilibrium, the ICE table reads as follows: initial concentrations are 0.10 M for nicotinic acid and 0 for H+ and the conjugate base, the change is +x for both H+ and the conjugate base and -x for nicotinic acid, leading to equilibrium concentrations of 0.10-x M for the nicotinic acid, x M for H+ and x M for the conjugate base.
With these values, the expression for Ka becomes 1.4 x 10⁻⁵ = (x)(x)/(0.10-x). Assuming that x is much smaller than 0.10 M, which is valid for weak acids, we can simplify the denominator to 0.10. The equation then simplifies to x² = (1.4 x 10⁻⁵)(0.10), from which we can calculate x. Once we find the value of x, the percent ionization is calculated using the formula: percent ionization = (concentration of ionized acid / initial concentration of acid) x 100%. After solving for x and computing the percent ionization, we can determine how much of the nicotinic acid is ionized in the solution.