Liquid Mixtures and Their Properties

A solution that resists changes in pH when small amounts of acid or base are added. Contains a weak acid and its conjugate base.

A mixture of a weak base (ammonium hydroxide) and its salt (ammonium chloride) that acts as a buffer.

The salt in a buffer solution is completely ionized, meaning it breaks down into its ions in solution.

The weak acid in a buffer solution only partially ionizes, meaning it doesn't fully break down into ions.

The process by which buffer solutions resist changes in pH, involving the reaction of the weak acid and its conjugate base with added acid or base.

A reaction where an acid (H+) reacts with an acetate ion (CH3COO-) from a buffer solution to form acetic acid (CH3COOH).

This reaction occurs when acid is added to a buffer solution. The acid (H+) reacts with the acetate ion (CH3COO-) from the buffer, forming undissociated acetic acid (CH3COOH). This helps to maintain the pH of the solution by reducing the concentration of H+ ions.

The addition of a base, such as hydroxide (OH-), to a buffer solution will lead to the neutralization of hydroxide ions by hydrogen ions (H+).

The hydroxide ions (OH-) from the base react with the hydrogen ions (H+) present in the buffer, forming water (H2O). This process effectively removes the hydroxide ions from the solution, preventing a significant change in pH.

A buffer system involves a weak acid (HA) and its conjugate base (A-), which helps to maintain pH stability. For example, in the acetic acid/acetate buffer, the weak acid is acetic acid (CH3COOH) and the conjugate base is acetate (CH3COO-).

A solution containing a weak base and its salt with a strong acid.

The pH of a base buffer solution is calculated using the Henderson-Hasselbalch equation: pH = pKa + log ([base]/[salt]).

The pKa value represents the negative logarithm of the acid dissociation constant (Ka).

The pKb value represents the negative logarithm of the base dissociation constant (Kb).

The sum of the pKa and pKb values of a conjugate acid-base pair is always 14 at 25°C.

The concentration of hydronium ions (H3O+) in a solution is a measure of its acidity.

A buffer solution is a mixture of a weak acid and its conjugate base. It resists changes in pH when small amounts of acid or base are added.

The Henderson-Hasselbalch equation is a helpful tool for calculating the pH of a buffer solution. It relates the pH to the pKa of the weak acid and the ratio of the concentrations of the acid and its conjugate base.

The pKa of a weak acid is a constant that reflects its acidity. It's the pH at which the acid is half ionized.

The pH of a solution is a measure of its acidity. A lower pH indicates a higher acidity.

A weak acid is an acid that only partially ionizes in solution, meaning it doesn't donate all of its hydrogen ions (H+). This results in an equilibrium between the undissociated acid (HA) and its conjugate base (A-), which is represented by the equation HA + H2O ⇋ H+ + A- .

The equilibrium constant for the dissociation of a weak acid is called the acid dissociation constant (Ka). It indicates the strength of the acid: a larger Ka value represents a stronger acid. The equation for Ka is Ka = [H+][A-]/[HA].

A buffer solution is a solution that resists changes in pH when small amounts of acid or base are added. An acid buffer is made up of a weak acid and its conjugate base, such as HA and A-. The pH of an acid buffer depends on the pKa of the weak acid and the ratio of salt (conjugate base) to acid. The equation for the pH of an acid buffer is: pH = pKa + log([salt]/[acid])

The salt of a weak acid is the conjugate base of that acid. In the equation HA + H2O ⇋ H+ + A-, A- represents the salt of the weak acid HA. The concentration of salt in an acid buffer directly affects the pH of the buffer

Buffer solutions help maintain the optimal pH range for enzymes to function properly. They prevent drastic changes in acidity or alkalinity, ensuring that the enzymes remain active and efficient.

If there's no buffer, enzymes might slow down, lose their ability to work, or even become denatured (lose their shape and function).

Buffers prevent drastic pH shifts, ensuring the environment stays within the optimal range for enzyme activity. They act like pH regulators, maintaining a stable internal environment for enzymes.

Enzymes are biological catalysts that speed up reactions in living organisms. They are very sensitive to pH changes, requiring a specific pH range for optimal activity.

Denaturation refers to the loss of an enzyme's natural shape and function due to factors like extreme temperature or pH changes. Denatured enzymes no longer work properly.