What is the effect of adding acid to a buffer solution?

The buffer resists the change in pH by reacting with the added acid.

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What is the effect of adding acid to a buffer solution?

The buffer resists the change in pH by reacting with the added acid.

What is the effect of adding base to a buffer solution?

The buffer resists the change in pH by reacting with the added base.

What happens to pH as $[H^+]$ increases?

pH decreases (becomes more acidic).

What happens to pOH as $[OH^-]$ increases?

pOH decreases (becomes more basic).

What happens to the pH at half equivalence point?

pH = pKa

What happens to the pH at equivalence point?

The number of moles of acid and base are equal, so the pH depends on the strength of the acid and base.

How do you calculate pH from $[H^+]$ ?

pH = -log $[H^+]$

How do you calculate pOH from $[OH^-]$ ?

pOH = -log $[OH^-]$

How do you calculate $K_a$ from $pK_a$ ?

$K_a = 10^{-pK_a}$

How do you calculate $K_b$ from $pK_b$ ?

$K_b = 10^{-pK_b}$

Describe the process of titration.

A solution of known concentration (titrant) is added to a solution of unknown concentration (analyte) until the reaction is complete, usually indicated by a color change or pH meter.

How to determine pH using the Henderson-Hasselbalch equation?

pH = pKa + log $[A^-]/[HA]$ , where $[A^-]$ is the concentration of the conjugate base and $[HA]$ is the concentration of the weak acid.

Define acid.

Substances with a pH less than 7 that donate H+ ions.

Define base.

Substances with a pH greater than 7 that accept H+ ions.

Define pH.

A measure of the concentration of free protons (H+) in a solution.

Define pOH.

A measure of the concentration of hydroxide ions (OH-) in a solution.

Define buffer.

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

Define $K_a$ .

Acid dissociation constant; measures the strength of a weak acid.

Define $K_b$ .

Base dissociation constant; measures the strength of a weak base.

All Flashcards

What is the effect of adding acid to a buffer solution?

The buffer resists the change in pH by reacting with the added acid.

What is the effect of adding base to a buffer solution?

The buffer resists the change in pH by reacting with the added base.

What happens to pH as $[H^+]$ increases?

pH decreases (becomes more acidic).

What happens to pOH as $[OH^-]$ increases?

pOH decreases (becomes more basic).

What happens to the pH at half equivalence point?

pH = pKa

What happens to the pH at equivalence point?

The number of moles of acid and base are equal, so the pH depends on the strength of the acid and base.

How do you calculate pH from $[H^+]$ ?

pH = -log $[H^+]$

How do you calculate pOH from $[OH^-]$ ?

pOH = -log $[OH^-]$

How do you calculate $K_a$ from $pK_a$ ?

$K_a = 10^{-pK_a}$

How do you calculate $K_b$ from $pK_b$ ?

$K_b = 10^{-pK_b}$

Describe the process of titration.

A solution of known concentration (titrant) is added to a solution of unknown concentration (analyte) until the reaction is complete, usually indicated by a color change or pH meter.

How to determine pH using the Henderson-Hasselbalch equation?

pH = pKa + log $[A^-]/[HA]$ , where $[A^-]$ is the concentration of the conjugate base and $[HA]$ is the concentration of the weak acid.

Define acid.

Substances with a pH less than 7 that donate H+ ions.

Define base.

Substances with a pH greater than 7 that accept H+ ions.

Define pH.

A measure of the concentration of free protons (H+) in a solution.

Define pOH.

A measure of the concentration of hydroxide ions (OH-) in a solution.

Define buffer.

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

Define $K_a$ .

Acid dissociation constant; measures the strength of a weak acid.

Define $K_b$ .

Base dissociation constant; measures the strength of a weak base.