General Chemistry
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Morphine is a weak base. A 0.150 M solution of morphine has a pH of 10.7. What is Kb for morphine?
A 3.93×10–5 M solution of methylamine, a weak organic base, has a pH of 9.56. What are the Kb and pKb for this base?
Using an ICE table, determine the pH of a 0.55 M KClO solution (Ka HClO = 2.9×10–8).
Using the ICE table method, determine the pH of a solution containing 0.42 M C2H5NH2 and 0.64 M C2H5NH3Br (Kb C2H5NH2 = 5.6×10–4).
Calculate the [OH–], pH, and pOH for a solution of hydroxylamine (HONH2, Kb = 1.1×10–8) that has a concentration of 0.40 M.
A 0.85 M solution of the weak base pyridine (C5H5N) has a pH of 9.58. Determine the Ka of the conjugate acid of pyridine.
Consider a hypothetical liquid, HX, that undergoes autoionization similar to water. The autoionization constant for HX is 1 × 10–20. Suppose you have a 0.051 M solution of KF in HX. If the dissociation constant of HF in HX solvent is 2.3 × 10–8, calculate the equilibrium concentration of H2X+.
Calculate the molality and freezing point of a solution of sodium butanoate that has a pH of 8.96 and a density of 1.01 g/mL. In aqueous solutions, sodium butanoate acts as a strong electrolyte. Note that the Ka for butanoic acid is 1.48×10−5.
Pyrrolidine (C4H9N), a common building block used in organic synthesis, has a pKb of 2.69. For a 0.41 M solution of pyrrolidine, determine the pH and the concentration of all species present (C4H9N, C4H9NH+, H3O+, OH–).
Caffeine (C8H10N4O2), a stimulant found in coffee, has a Kb of 4.1 × 10–4. What is the pH of a 0.35 M solution of caffeine?
Propionic acid (C2H5COOH) has a pKa of 4.886. What is the pH of a 0.065 M sodium propionate solution?
Determine the [OH–] and pH for a 0.105 M K2C2O4 solution. (H2C2O4: Ka1 = 5.9×10–2; Ka2 = 6.4×10–5)
Piperidine is essential in drug production. It is a weak organic base.
C5H10NH + H2O ⇌ C5H10NH2+ + OH–
What is the Kb for piperidine if 0.067 M solution of piperidine has a pH of 11.94?
Calculate the pH of a 0.245 M hydrazine (H2NNH2) solution. The Kb of hydrazine is 1.3×10–6.
Mg(C2H3O2)2 is a salt of acetic acid. A solution containing this salt has a [Mg2+] = 0.16 M and a pH = 9.12. Calculate the Ka of acetic acid.
A solution contains 0.650 M BrO–. Calculate the [OH–] and pH of the solution.
Calculate the pH of a solution containing 545 mg/L of morphine (C17H19NO3). Morphine is a weak base with a pKb of 5.80.
For a 2.50 M NaClO solution, what would be the concentration of the species present at equilibrium?
What is the pH of a 0.20 M solution of sodium benzoate (NaC6H5COO) if its Ka is 6.5x10-5?
What is the Kb for a 0.200 M solution of CH3NH2 with a pH of 11.961?
Calculate the concentration of a base (Kb = 7.60 × 10-5) that will give a pH of 11.31.
Calculate the pH of a 0.023 M C6H5NH2 ( Kb = 6.5x10-4).
Determine the pH of 150.0 mL of 0.40 M pyridine (C5H4N) solution. What is the pH after addition of 5.0 g pyridinium hydrochloride (C5H4NHCl)? Assume the addition of pyridinium hydrochloride does not affect the volume.
Enumerate the species present in a 0.284 M CH3NH3Cl (Kb = 4.47×10−4) solution with their concentration in molarity.