Acids & Bases Test

What defines an Arrhenius acid?

An Arrhenius acid is a substance that increases the concentration of hydrogen ions (H+) in aqueous solution.

What defines a Brønsted-Lowry acid?

A Brønsted-Lowry acid is a substance that donates a proton (H+) to another substance.

What are the strong acids to memorize?

HCl, HBr, HI, HNO3, H2SO4, HClO4.

What is the difference between a strong acid and a weak acid?

Strong acids completely dissociate in solution, while weak acids only partially dissociate.

What are the strong bases to memorize?

Group 1 and 2 hydroxides, except LiOH and Mg(OH)2.

What does the autoionization of water produce?

Water produces equal concentrations of H+ and OH- ions.

What is the formula for the ion product of water (Kw)?

Kw = [H+][OH-].

What does the pH scale measure?

The pH scale measures the acidity or basicity of a solution.

How is pH calculated?

pH = -log[H+].

What is the acid ionization constant (Ka)?

Ka is a measure of the strength of an acid in solution.

What is the base ionization constant (Kb)?

Kb is a measure of the strength of a base in solution.

How do you calculate the pH of a strong acid?

pH = -log[H+] because strong acids fully dissociate.

How do you calculate the pH of a weak acid?

Use the formula: pH = -log[H+] determined from the acid dissociation constant (Ka).

What is the relationship between pKa and Ka?

pKa = -log(Ka).

What is percent ionization?

Percent ionization is the ratio of the concentration of ionized acid to the initial concentration of acid, expressed as a percentage.

What distinguishes acidic, basic, and neutral salts?

Acidic salts produce H+ in solution; basic salts produce OH-; neutral salts do not affect the pH.

What is the common-ion effect?

The common-ion effect is a decrease in the ionization of a weak acid or base due to the addition of a strong electrolyte that provides a common ion.

How is the Henderson-Hasselbalch equation used?

It relates pH, pKa, and the ratio of the concentration of base to acid.

What is buffer capacity?

Buffer capacity is the ability of a buffer solution to resist changes in pH upon the addition of acids or bases.

What type of titration occurs between a strong acid and a strong base?

The pH will sharply rise at the equivalence point.

What occurs at the half-way equivalence point of a titration?

At the half-way equivalence point, [HA] = [A-], and pH = pKa.

What happens during the before equivalence point of titration?

The solution contains a mixture of unreacted weak acid and its conjugate base.

What is observed after the equivalence point in titration?

The pH will be greater than 7 due to excess strong base.

What are the three types of titrations?

Strong acid/strong base, weak acid/strong base, weak base/strong acid.

What indicates the equivalence point on a titration curve?

The equivalence point is where the amount of titrant is stoichiometrically equivalent to the amount of substance being titrated.

What is the formula to calculate pH of a buffer?

Use Henderson-Hasselbalch equation: pH = pKa + log[base]/[acid].

What occurs in a weak acid/strong base titration at the equivalence point?

The resulting solution will be basic due to the presence of the conjugate base.

What is the pH at the equivalence point of a strong acid/strong base titration?

The pH is typically around 7.

What happens to pH during the titration of a weak base with a strong acid at equivalence?

The pH will be less than 7.

What two factors influence the strength of an acid or base?

Concentration and the inherent strength of the acid or base.

What should pH be in a neutral solution at 25°C?

pH should be 7 at 25°C.

In a buffered solution, how does the addition of strong acid affect the pH?

It change the pH only slightly due to the buffer's capacity to neutralize added acid.

What is the pH of a solution with [H+] = 1.0 x 10^-5 M?

pH = 5.

What does a low pH indicate?

A low pH indicates a high concentration of hydrogen ions, representing an acidic solution.

Why is it important to understand the properties of acids and bases?

It is crucial for predicting the behavior of substances in chemical reactions and solutions.

How can you determine if a solution is acidic or basic?

By measuring its pH or determining its H+ and OH- concentrations.

What is the significance of weak acids and bases in titrations?

They create buffering effects, making the endpoint harder to detect without indicators.

How is the pOH of a solution calculated?

pOH = -log[OH-].

If a solution has a pH of 9, what can be said about its state?

It is basic.