17. Acid and Base Equilibrium

Calculate the pH of a 0.10 M solution of hydrazine, N2H4, given that the Kb for hydrazine is 1.3×10⁻⁶.

Calculate the pH of a 0.20 M solution of KCN at 25.0 °C, given that the Kb for CN⁻ is 2.0 x 10⁻⁵.

Calculate the pH of a solution that is 0.540 M in pyridine (C5H5N) and 0.470 M in pyridinium chloride (C5H5NHCl). The Kb for pyridine is 1.7 x 10^-9.

Calculate the pH of a 0.021 M NaCN solution. Given that the Ka of HCN is 4.9 × 10^−10, what is the pH of the solution?

What is the pH of a solution formed by mixing 250.0 mL of 0.15 M NH4Cl with 200.0 mL of 0.12 M NH3, given that the Kb for NH3 is 1.8 × 10^-5?

Calculate the pH of a solution made by adding 160 mL of 1.00 M HCl to 300 mL of 1.70 M NH3 solution.

Consider the titration of a 26.0-mL sample of 0.185 M CH3NH2 (Kb = 4.4 × 10⁻⁴) with 0.155 M HBr. What is the initial pH of the CH3NH2 solution before any HBr is added?

Determine the pH of a solution that is 0.125 M in CO3^2−. For carbonic acid (H2CO3), Ka1=4.3×10^−7 and Ka2=5.6×10^−11. What is the pH of the solution?

Calculate the pH of a 0.205 M KNO2 solution, given that the Ka of nitrous acid (HNO2) is 4.6 × 10^(-4).

What is the pH of a 0.208 M NH4Cl solution at 25°C, given that the Kb of NH3 is 1.8x10^-5?

For a solution that is 0.164 M NH3 and 0.110 M NH4Cl, calculate the concentration of [H3O+].

If 0.365 g of sodium carbonate (Na2CO3) is dissolved in 1.5 L of water, what is the pH of the solution? (Kb for CO3^2- = 1.8 x 10^-4)

A solution of sodium acetate (NaCH3COO) has a pH of 9.64. The acid-dissociation constant (Ka) for acetic acid is 1.8 x 10^-5. What is the molarity of the sodium acetate solution?

What is the expression for the equilibrium constant (Kb) for the dissociation of a weak base in water?

What is the pH of a 0.05 M sodium fluoride solution, given that F⁻ has a Kb of 1.59 x 10⁻¹¹?