Using the Henderson-Hasselbalch equation: pH = pKa + log([A-]/[HA]) = 4.76 + log(0.1/0.2) = 5.74

Using the Henderson-Hasselbalch equation, pH = pKa + log([A-]/[HA]) = 4.76.

HCl and NaOH neutralize each other completely, resulting in a neutral solution with a pH of 7.

pH is calculated as pH = -log[H+]. For [H+] = 1 x 10^-5 M, pH = -log(1 x 10^-5) = 5.

pH is calculated as pH = -log[H3O+]. For [H3O+] = 1 x 10^-5 M, pH = -log(1 x 10^-5) = 5.

pOH = -log[OH-] = -log(1.0 x 10^-3) = 3. Therefore, pH = 14 - pOH = 14 - 3 = 11.

pH = -log[H+] = -log(1 x 10^-7) = 7.

Using Henderson-Hasselbalch equation: pH = pKa + log([A-]/[HA]); pKa of acetic acid = 4.76, so pH = 4.76 + log(1) = 4.76

pOH = -log[OH-] = -log(0.001) = 3; pH = 14 - pOH = 14 - 3 = 11

To find the pH, first calculate pOH = -log[OH-] = 4, then use pH + pOH = 14, so pH = 14 - 4 = 10.

Using the formula pH = -log[H+], we find pH = -log(1 x 10^-6) = 6.

A precipitate forms when the ionic product exceeds the solubility product (Ksp) of the salt.

All of the above factors contribute to the increase in pH during the titration of a weak acid with a strong base.

In a solution of acetic acid, the primary species present is the undissociated acetic acid (CH3COOH), along with some dissociated ions.

In a solution of sodium acetate, the acetate ion (CH3COO-) is the primary species that affects the pH.

For a conjugate acid-base pair, the relationship is Ka * Kb = Kw, where Kw is the ion product of water.

The relationship is given by the equation pKa = -log(Ka), where Ka is the acid dissociation constant.

The relationship is given by the formula pKa = -log(Ka), where Ka is the acid dissociation constant.

The relationship is given by pKa = -log(Ka), where Ka is the acid dissociation constant.

Acetic acid (CH3COOH) is a weak acid, while HCl, H2SO4, and HNO3 are strong acids.

Cl- ions will react with Ag+ ions from AgNO3 to form AgCl, which is insoluble in water and will precipitate out.

The presence of SO4^2- ions will react with Ba2+ ions to form insoluble BaSO4, causing precipitation.

Cl- ions will react with Ag+ ions to form the insoluble salt AgCl, causing precipitation.

NH4+ is the conjugate acid of a weak base (NH3) and will increase the acidity of the solution.

A buffer solution is designed to resist changes in pH when small amounts of acid or base are added.

NaOH (sodium hydroxide) is a strong base that completely dissociates in solution.

A buffer solution resists changes in pH upon the addition of small amounts of acid or base.

Na2CO3 is a salt of a weak acid (H2CO3) and a strong base (NaOH), thus it will produce a basic solution.

Strong acids completely dissociate in solution, producing a high concentration of H+ ions, which allows them to conduct electricity.

The common ion effect states that the solubility of a salt decreases in the presence of a common ion.