Find the pH and percent ionization of a 0.100 M solution of a weak monoprotic acid having the gi

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Find the pH and percent ionization of a 0.100 M solution of...

Find the pH and percent ionization of a 0.100 $\mathrm{M}$ solution of a weak monoprotic acid having the given $K_{\mathrm{a}}$ values.
a. $K_{\mathrm{a}}=1.0 \times 10^{-5}$ b. $K_{\mathrm{a}}=1.0 \times 10^{-3}$ c. $K_{\mathrm{a}}=1.0 \times 10^{-1}$

Key Concepts

Acid Dissociation Constant (Ka)

Ka is a quantitative measure of a weak acid's strength, defined by the ratio of the concentration of dissociated ions to the concentration of the undissociated acid at equilibrium. It provides key insight into the extent of ionization in solution.

Percent Ionization

Percent ionization indicates the extent to which a weak acid ionizes in solution. It is expressed as the percentage of the original acid molecules that dissociate, providing a clear measure of the acid's contribution to the solution's pH.

pH Calculation

The pH of a solution is determined by the negative logarithm of the hydrogen ion concentration. For weak acids, the equilibrium established by the acid dissociation process is used to calculate these ion concentrations and thus the pH of the solution.

Acid Dissociation Reaction

This reaction describes the process by which a weak monoprotic acid donates a proton to water, forming hydronium (or hydrogen ions) and its conjugate base. It lays the groundwork for understanding how equilibrium is established in a weak acid solution.

Weak Acid Equilibrium

In solutions of weak acids, the acid does not fully ionize, resulting in an equilibrium between the undissociated acid and its conjugate base along with hydrogen ions. This equilibrium is essential for deriving calculations for pH and percent ionization.

Transcript

0:00 My name is ahmad ali.

00:02 This question is longer question, but we will try to solve it quickly.

00:08 In this question, we have a weak acid monoprotic, which you can write as h .y.

00:15 This weak acid has the value of k .a.

00:19 The forgiving start is equal.

00:22 Timbauer negative 5, and its concentration is 0 .1 molarity.

00:30 For this acid we want to calculate the ph and the percentage of ionization so we can solve it quickly how this weak acid win be in water small amount of eight ionize according to the value of ka to h positive and y negative so i write here it's h's y we suppose it's 1.

01:03 So its initial concentration is 0 .1 but when dissolving water small amount ionized so it's a concentration now 0 .1 negative x.

01:12 These amount are nice which is x is unites to each plus event y negative.

01:18 So even write the kia law which is equal team power negative 5 which is represent the concentration of protonium times by the concentration of an i.

01:31 So x times x is x squared divided by the concentration of each y ion ionized, which is 0 .1 negative x.

01:42 Here, due to the k a value is very small compared to the initial value, initial concentration.

01:51 So now the x value can be neglected.

01:55 So we can calculate the x which is a concentration which is 0 .1 times 5 10 power negative 5 and it takes the root of them.

02:07 So by calculator we found that the value is equal 0 .1 times 5 10 power negative 5 and takes the root of answer so it will be equal 10 power negative 3...

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