NDA Ionic Equilibrium

The ionic product of water (Kw) at 25°C is 1.0 × 10⁻¹⁴. What is the pH of a neutral solution at this temperature?

A weak acid HA has a Ka value of 1.8 × 10⁻⁵. Which of the following correctly describes the strength of this acid relative to strong acids?

The solubility product (Ksp) of AgCl at 25°C is 1.8 × 10⁻¹⁰. If the concentration of Cl⁻ ions in a saturated solution is 1.34 × 10⁻⁵ M, what is the concentration of Ag⁺ ions?

Which of the following salts will hydrolyze in water to produce an acidic solution?

The Ka of acetic acid is 1.8 × 10⁻⁵ and its Kb is 5.6 × 10⁻¹⁰. What is the relationship between Ka, Kb, and Kw for the acetate ion (CH₃COO⁻)?

The ionic product of water (Kw) at 25°C is 1.0 × 10⁻¹⁴. What is the pH of a neutral solution at this temperature?

A weak acid HA has a Ka value of 1.8 × 10⁻⁵. Which statement correctly describes its ionization behavior?

The pKa of acetic acid is 4.74. What is the Ka value?

For a weak base ammonia (NH₃) with Kb = 1.8 × 10⁻⁵, what is the pOH of a 0.1 M NH₃ solution (assuming [OH⁻] = √(Kb × C))?

A salt solution of NaA (where A⁻ is a weak conjugate base) shows basic pH. This is due to which process?

The common ion effect in the solution of a weak acid HA with added salt NaA will:

At 25°C, if the pH of a solution is 3.5, what is the [OH⁻] concentration (Kw = 1.0 × 10⁻¹⁴)?

Which of the following salts will produce an acidic solution in water?

A weak acid HA has Ka = 1.8 × 10⁻⁵. If 0.1 M solution of this acid is prepared, what is the degree of ionization (α)? (Assume α << 1)

The solubility product (Ksp) of AgCl at 25°C is 1.8 × 10⁻¹⁰. What is the solubility of AgCl in a 0.1 M NaCl solution?

A buffer solution is prepared by mixing 50 mL of 0.1 M acetic acid (Ka = 1.8 × 10⁻⁵) and 50 mL of 0.1 M sodium acetate. What is the pH of this buffer? (Use log 1.8 ≈ 0.26)