Ionic Equilibrium in Aqueous Solutions
Chemistry ⇒ Chemical Kinetics and Equilibrium
Ionic Equilibrium in Aqueous Solutions starts at 12 and continues till grade 12.
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A 0.1 M solution of a weak acid HA is 1% ionized. Calculate the concentration of H+ ions.
A solution contains 0.1 M NH3 and 0.1 M NH4Cl. Kb for NH3 is 1.8 × 10–5. Calculate the pH of the solution.
A solution has [H+] = 2 × 10–4 M. Calculate its pH.
A solution has a pOH of 4. What is its pH at 25°C?
A solution is prepared by mixing 50 mL of 0.1 M HCl and 50 mL of 0.1 M NaOH. What is the pH of the resulting solution?
A solution contains 0.1 M NH3 and 0.1 M NH4Cl. Kb for NH3 is 1.8 × 10–5. Calculate the pH of the solution.
A solution is prepared by mixing 50 mL of 0.1 M HCl and 50 mL of 0.1 M NaOH. What is the pH of the resulting solution?
The Ksp of BaSO4 is 1.1 × 10–10 at 25°C. Will a precipitate form if [Ba2+] = 1 × 10–5 M and [SO42–] = 2 × 10–5 M?
A solution is prepared by mixing 100 mL of 0.1 M H2SO4 with 100 mL of 0.1 M NaOH. Calculate the pH of the resulting solution, assuming complete dissociation of H2SO4.
Which of the following is a Bronsted-Lowry base?
(1) H2O
(2) NH3
(3) HCl
(4) Na+
Which of the following is a Lewis acid?
(1) NH3
(2) BF3
(3) H2O
(4) Cl–
Which of the following is a strong electrolyte in aqueous solution?
(1) CH3COOH
(2) NaCl
(3) NH3
(4) H2O
Which of the following is NOT a property of a buffer solution?
(1) It maintains a constant pH
(2) It is formed by a strong acid and its salt
(3) It resists change in pH upon dilution
(4) It contains a weak acid and its conjugate base
The pH of a 0.01 M HCl solution is ________.
The pH of pure water at 25°C is ________.
If the pH of a solution is 8.5, the concentration of OH– ions is ________ M.
The Ksp of BaSO4 is 1.1 × 10–10 at 25°C. Will a precipitate form if [Ba2+] = 1 × 10–5 M and [SO42–] = 2 × 10–5 M?
True or False: The addition of a common ion increases the solubility of a sparingly soluble salt.
True or False: The ionic product of water (Kw) increases with increase in temperature.
True or False: The pH of a buffer solution changes significantly upon addition of a small amount of strong acid.
