The period T of a simple pendulum is given by T = 2π√(L/g). For L = 1 m and g ≈ 9.8 m/s², T = 2π√(1/9.8) ≈ 2 s.

The period of a satellite in a circular orbit at a height of 300 km is approximately 90 minutes.

Satellites in low Earth orbit have a much shorter orbital period compared to geostationary satellites due to their proximity to Earth.

Electronegativity increases across a period from left to right.

The pH level of pure water is 7, which is considered neutral.

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.

The pH of a 0.01 M HCl solution is 2, as HCl is a strong acid and fully dissociates.

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

For NaOH, which is a strong base, pOH = -log[OH-]. [OH-] = 0.01 M, so pOH = 2. Therefore, pH = 14 - pOH = 14 - 2 = 12.

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.

Sodium acetate is a salt of a weak acid (acetic acid) and a strong base (sodium hydroxide). The pH can be calculated using the formula pH = 7 + 0.5(pKa - log[C]), where pKa of acetic acid is 4.76.

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

H2SO4 is a strong acid and dissociates completely, so pH = -log(0.01) = 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.

H2SO4 is a strong acid and dissociates completely; [H+] = 0.05 M, so pH = -log(0.05) ≈ 1.3

pOH = -log[OH-] = -log(0.1) = 1; pH = 14 - pOH = 14 - 1 = 13

Using the formula for weak acids, pH = 0.5(pKa - log[C]) = 0.5(4.74 - log(0.1)) = 4.76.

NH4Cl is a salt of a weak base and a strong acid; it hydrolyzes to give H+, resulting in a pH < 7.

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

The pH of a strong acid like HCl is calculated using the formula pH = -log[H+]. For 0.1 M HCl, [H+] = 0.1 M, so pH = -log(0.1) = 1.

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.

KHP is a weak acid; its pKa is approximately 5.0, so the pH of a 0.1 M solution is around 5.0.

pH = 7 + 0.5(pKa + log[C]) = 7 + 0.5(4.76 + log(0.1)) = 9.24

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