The general solution is y = Ce^(4x). Using the initial condition y(0) = 2, we find C = 2, thus y = 2e^(4x).

Percentage by mass = (mass of solute / total mass) × 100 = (15 g / (15 g + 85 g)) × 100 = 17.65%.

Percentage concentration = (mass of solute / mass of solution) × 100 = (15 g / 150 g) × 100 = 10%

Percentage concentration = (mass of solute / mass of solution) × 100 = (20 g / 200 g) × 100 = 10%.

Argon is located in Period 3 of the periodic table.

Lithium is located in period 2 of the periodic table.

Lithium is located in period 2 of the periodic table.

Sodium is in period 3 of the periodic table.

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.

At 25°C, the pH of a neutral solution is 7.

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

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

Na2CO3 is a salt of a weak acid (H2CO3) and a strong base (NaOH). The pH can be estimated using the hydrolysis of CO3^2- which gives a pH around 11.0.

Using the formula for weak acids, pH = 0.5(pKa - logC) = 0.5(4.00 - log(0.01)) = 5.00.

pH = -log[H+]. pH = -log(0.001) = 3.