Acids and Bases

CH₃COOH

HC]

NaCl

HNO₃

When NaOH has been completely consumed.

At quarter-equivalence point.

At half-equivalence point.

At equivalence point.

Between 10 and 1

Between 0 and 1

Between 14 and 11

Between 4 and 7

The hydroxyl group (-OH) fully dissociates, releasing a proton and OH⁻ ions.

Acetic acid forms strong hydrogen bonds with water, thus it completely dissociates.

It partially ionizes because the carboxyl group can lose a proton, forming acetate and H⁺.

The methyl group (CH3-) donates electrons to stabilize the conjugate base.

Cannot return to its original form after coming in contact with water

Always raises the concentration of H⁺ ions and the temperature of the solution

Removes excess hydrogen ions and hydroxide anions when mixed with water

Incompletely disassociates after coming in contact with water

The pH changes minimally with small additions of acid or base.

The equivalence point is reached immediately after adding titrant.

There is no visible change on the pH indicator used in titration.

The pH changes dramatically with small additions of acid or base.

It is the quickest step in the pathway.

It is the slowest step in the pathway.

It involves the highest concentration of substrate.

It has the least amount of intermediates formed.

An indicator that changes color at a pH above 7

Bromothymol blue because it changes color between pH range of 6-7.6

Methyl orange because it has a mid-point around pH 4-4.5

Phenolphthalein because it changes color below pH 7

The equilibrium shifts toward the side with fewer moles of gas.

Decreasing pressure increases both forward and reverse reactions equally without shifting balance.

The equilibrium shifts toward the side with more moles of gas.

A decrease in pressure has no effect on gaseous equilibria systems.

4x10^-3 M

2x10^-3 M

3.2x10^-5 M

2.8x10^-4 M