Acetate is a relative strong base.

A buffered solution

At the mid point of titration, the ratio of the concentration of the weak acid with its conjugate base

Buffer solutions

A Bronsted acid becomes __________ upon losing a proton.

What is the ratio of [A-]:[HA] in a solution at pH 5 that contains a weak acid with pKa = 5?

What is the concentration, in moles/liter, of the hydrogen ion, if pH of a solution is 7?

Polyprotic acids such as H3PO4, can act as acid-base buffers

The effectiveness or capacity of a buffer solution can be affected by

Phosphoric acid is tribasic, with pKa’s of 2.14, 6.86, and 12.4. The ionic form that predominates at pH 3.2 is:

Which of the following statements about buffers is true?

An initial pH of 9.5 and an equivalence point at pH 4.5 correspond to a titration curve for a

Water can act as an acid or a base.

In a titration of monoprotic acids and bases, there is a large change in pH __________

Two weak acids, A and B, have pKa values of 4 and 6, respectively. Which statements true?

The ratio of the concentration of a ________ over ________ describes the proportions of forms of a weak acid necessary to satisfy the Henderson-Hasselbalch equation.

What is the pH of a buffer solution where [HA] = [A–]?

When an acetic acid solution is titrated with sodium hydroxide, the slope of the titration curve (pH vs volume of NaOH added) increases when sodium hydroxide is first added. This change shows that __________.

At values of pH above the pKa value, an acid is mostly deprotonated.

Identify all the correct statements about an acid–base buffer solution. I. It can be prepared by combining a strong acid with a salt of its conjugate base. II. It can be prepared by combining a weak acid with a salt of its conjugate base. III. It can be prepared by combining a weak base with its conjugate acid. IV. The pH of a buffer solution does not change when the solution is diluted. V. A buffer solution resists changes in its pH when an acid or base is added to it.

At the mid point of titration, volume of analyte volume of titrant are not necessarily equal.

The slope of a titration curve is steep within one pH unit of the pKa value.

Equivalence point = [acid] and [conjugate base] are equal.

Weak acids act as back up source of protons.

At the midpoint of the titration, one-half of the original acid has undergone dissociation, so that the concentration of the proton donor equals that of the proton acceptor.

For any weak acid-strong base titration, the pH at the equivalence point will be lesser than 7.

A titration is an acid-base reaction, in which the hydrogen ions (H+) from the acid react with hydroxide ions (OH-) from the base to form a salt.

An acid-base titration is a neutralization reaction.

The equivalent point of a titration of a strong base with a strong acid occurs at pH = 7

The value of the equivalence point of titration of a weak acid with a strong base varies depending on the pKa of the acid.

At the equivalence point, 50% of a weak acid titrated with a strong base is neutralized and converted to its conjugate base.

A the equivalence point the molar concentration of the proton donor equals the molar concentration of the proton acceptor.

The equivalence point allows us to determine the pKa of an unknown acid.

The pKa of acetic acid is 4.76. That means that at pH = 4.76, acetic acid is half dissociated.

Phosphoric acid has three pKas.

Acetic acid is mostly protonated at pH = 7.

Acetic acid is mostly protonated a pH = 2

The titration curve of acetic acid has two buffering regions.

When a weak acid is 50% dissociated, pH of the solution is equal to the pKa of the acid.

The slope of a titration curve is shallow within one pH unit of the pKa value.

The equivalence point of a titration is also called the end point.