Acids and Bases

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

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

Their conjugate bases are too stable to form ions.

They have higher molecular weights than strong acids.

They react too quickly with water molecules.

They do not donate protons as readily as strong acids.

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.

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.

The initial concentration of weak acid present in solution.

The phase state (solid, liquid, gas) of water at room temperature.

The pKa value of the weak acid compared to water's pKa value.

The temperature at which deprotonation occurs if above ambient conditions.

CH₃COOH

HC]

NaCl

HNO₃

When NaOH has been completely consumed.

At quarter-equivalence point.

At half-equivalence point.

At equivalence point.

4x10^-3 M

2x10^-3 M

3.2x10^-5 M

2.8x10^-4 M

Between 10 and 1

Between 0 and 1

Between 14 and 11

Between 4 and 7