NaHCO3 is a weak base. The pH can be calculated using the formula pH = 7 + 0.5(pKa - log[C]). pKa of HCO3- is about 10.3, so pH ≈ 8.3.

Using the formula for weak bases, pH = 14 - 0.5(pKb - logC) = 14 - 0.5(4.74 - log(0.05)) = 5.25.

pOH = -log[OH-] = -log(0.1) = 1, thus pH = 14 - pOH = 14 - 1 = 13.

pOH = -log(0.2) = 0.7, thus pH = 14 - 0.7 = 13.3.

Ionization = 1% of 0.1 M = 0.001 M, so [H+] = 0.001 M.

[H+] = 10^(-pH) = 10^(-2.87) ≈ 0.001 M.

C1V1 = C2V2; (0.1 M)(50 mL) = C2(250 mL); C2 = 0.02 M.

pH = 3 means [H+] = 10^-3 M = 0.001 M.

For a weak acid, pH ≈ pKa for a 0.1 M solution, so pH ≈ 4.76.

A buffer solution typically consists of a weak acid and its conjugate base (salt), which helps to resist changes in pH when small amounts of acid or base are added.

Concentration of H+ = 10^(-pH) = 10^(-3) = 0.001 M.

[H+] = 10^(-pH) = 10^(-4) = 0.0001 M.

The solubility product constant (Ksp) for AgCl is expressed as Ksp = [Ag+][Cl-], where [Ag+] and [Cl-] are the molar concentrations of the ions in a saturated solution.

Ksp = [Ag+][Cl-] = (1.33 x 10^-5)(1.33 x 10^-5) = 1.78 x 10^-10.

Using the formula for weak acids, pH = 0.5(pKa - logC) = 0.5(4.74 - log(0.001)) = 3.87.

pH = -log(0.001) = 3.

For a strong acid like HCl, pH = -log[H+] = -log(0.01) = 2.

Na2CO3 is a basic salt, pH is approximately 11.5.

pOH = -log(0.01) = 2; pH = 14 - pOH = 14 - 2 = 12.

H3PO4 is a triprotic acid; for a dilute solution, the first dissociation dominates, giving pH ≈ 2.

Using the formula for weak acids, pH = 0.5(pKa - log[C]) where pKa = -log(1.8 x 10^-5) ≈ 4.74. pH = 0.5(4.74 - log(0.05)) ≈ 4.7.

NaCl is a neutral salt, so the pH remains 7.

NH4Cl is a salt of a weak base and strong acid, pH < 7. Calculate using hydrolysis: pH ≈ 4.75.

K2CO3 is a salt of a weak acid (H2CO3) and strong base (KOH), resulting in a basic solution with pH around 10.

K2SO4 is a neutral salt formed from a strong acid (H2SO4) and a strong base (KOH). Therefore, the pH of the solution is 7.

NH4Cl is an acidic salt, pH is approximately 5.1.

Using the formula for salt of weak acid, pH = 14 + 0.5(pKa + logC) = 14 + 0.5(4.74 + log(0.1)) = 9.25.

NaHCO3 is a weak base, pH ≈ 8.00 due to its bicarbonate ion acting as a weak base.

H2SO4 is a strong acid; it dissociates completely, so [H+] = 0.1 M; pH = -log(0.1) = 1.

Using the Henderson-Hasselbalch equation, pH = pKa + log([A-]/[HA]) = 4.74 + log(1) = 4.74.