Podcast
Questions and Answers
In the reaction (HCl(aq) + H_2O(aq) \rightleftharpoons H_3O^+(aq) + Cl^-(aq)), which species act as Brønsted-Lowry acids?
In the reaction (HCl(aq) + H_2O(aq) \rightleftharpoons H_3O^+(aq) + Cl^-(aq)), which species act as Brønsted-Lowry acids?
- HCl, H2O, and H3O+
- HCl and H2O
- HCl and Cl-
- HCl and H3O+ (correct)
What is the conjugate base of the Brønsted-Lowry acid HPO₄²⁻?
What is the conjugate base of the Brønsted-Lowry acid HPO₄²⁻?
- H₃PO₄
- PO₄³⁻ (correct)
- HPO₄²⁻
- H₂PO₄⁻
Which of the following correctly describes an acidic solution at 25°C?
Which of the following correctly describes an acidic solution at 25°C?
- [H₃O⁺] > 1 × 10⁻⁷ M > [OH⁻] (correct)
- [H₃O⁺] > [OH⁻] > 1 × 10⁻⁷ M
- [H₃O⁺] = [OH⁻] > 1 × 10⁻⁷ M
- [H₃O⁺] < 1 × 10⁻⁷ M > [OH⁻]
Which of the following species is NOT considered a Lewis base?
Which of the following species is NOT considered a Lewis base?
What is the pH of a 0.020 M HClO₄ solution, assuming complete dissociation?
What is the pH of a 0.020 M HClO₄ solution, assuming complete dissociation?
An aqueous solution of pyridine contains 2.15 × 10⁻⁴ M hydroxide ion. Calculate the pH of this solution.
An aqueous solution of pyridine contains 2.15 × 10⁻⁴ M hydroxide ion. Calculate the pH of this solution.
The pH of a 0.150 M CH₃COOH (acetic acid) solution is 2.78. What is the value of Ka for acetic acid?
The pH of a 0.150 M CH₃COOH (acetic acid) solution is 2.78. What is the value of Ka for acetic acid?
Which of the following is the strongest acid?
Which of the following is the strongest acid?
Para-Aminobenzoic acid (PABA), p-H₂NC₆H₄(COOH), is used in some sunscreens. Calculate the pH of an aqueous solution with [PABA] = 0.030 M and Ka = 2.2 × 10⁻⁵.
Para-Aminobenzoic acid (PABA), p-H₂NC₆H₄(COOH), is used in some sunscreens. Calculate the pH of an aqueous solution with [PABA] = 0.030 M and Ka = 2.2 × 10⁻⁵.
What is the pH of a 0.100 M NH₃ solution given that Kb = 1.8 × 10⁻⁵? (NH₃(aq) + H₂O(l) ⇌ NH₄⁺(aq) + OH⁻(aq))
What is the pH of a 0.100 M NH₃ solution given that Kb = 1.8 × 10⁻⁵? (NH₃(aq) + H₂O(l) ⇌ NH₄⁺(aq) + OH⁻(aq))
If all acids are at 0.100 M concentration, which monoprotic acid is the strongest?
If all acids are at 0.100 M concentration, which monoprotic acid is the strongest?
Which of the following pairs represents a buffer solution?
Which of the following pairs represents a buffer solution?
What is the pH of a solution prepared by mixing 50.0 mL of 0.20 M HCl with 50.0 mL of 0.10 M NaOH?
What is the pH of a solution prepared by mixing 50.0 mL of 0.20 M HCl with 50.0 mL of 0.10 M NaOH?
What is the function of a buffer solution?
What is the function of a buffer solution?
Which of the following indicators would be most suitable for titrating a strong acid with a weak base?
Which of the following indicators would be most suitable for titrating a strong acid with a weak base?
What is the molar solubility of AgCl (Ksp = 1.8 × 10⁻¹⁰) in pure water?
What is the molar solubility of AgCl (Ksp = 1.8 × 10⁻¹⁰) in pure water?
The Ksp for PbCl₂ is 1.6 × 10⁻⁵. What is the [Pb²⁺] in a saturated solution of PbCl₂?
The Ksp for PbCl₂ is 1.6 × 10⁻⁵. What is the [Pb²⁺] in a saturated solution of PbCl₂?
In which of the following solutions would AgCl be least soluble?
In which of the following solutions would AgCl be least soluble?
Which of the following statements is true regarding the relationship between Q (the ion product) and Ksp (the solubility product)?
Which of the following statements is true regarding the relationship between Q (the ion product) and Ksp (the solubility product)?
Flashcards
Brønsted-Lowry Acids
Brønsted-Lowry Acids
Substances that donate protons (H+) in a chemical reaction.
Conjugate Base
Conjugate Base
The species formed when a Brønsted-Lowry acid loses a proton.
Acidic Solution
Acidic Solution
Solution where the concentration of hydronium ions is greater than the concentration of hydroxide ions.
Lewis Base
Lewis Base
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pH
pH
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Acid Dissociation Constant (Ka)
Acid Dissociation Constant (Ka)
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Base Dissociation Constant (Kb)
Base Dissociation Constant (Kb)
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Monoprotic acid
Monoprotic acid
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Study Notes
- Bronsted-Lowry acids in the reaction HCl(aq) + H2O(aq) ⇌ H3O+(aq) + Cl-(aq) are HCl and H3O+.
- The conjugate base of the Bronsted-Lowry acid HPO42- is PO43-.
- An acidic solution at 25°C has [H3O+] > 1 × 10-7 M > [OH-].
- NH4+ is not considered to be a Lewis base.
- The pH of a 0.020 M HClO4 solution is 1.70.
- The pH for an aqueous solution of pyridine that contains 2.15 × 10-4 M hydroxide ion is 10.33.
- Given that the pH of 0.150 M CH3CO2H (acetic acid) is 2.78, the value of Ka for acetic acid is 1.9 × 10-5.
- H2Te is the strongest acid among H2Se, H2Te, H2O, and H2S.
- For para-Aminobenzoic acid (PABA) with [PABA] = 0.030 M and Ka = 2.2 × 10-5, the pH of an aqueous solution is 3.09.
- The pH of a 0.100 M NH3 solution with Kb = 1.8 × 10-5, where NH3(aq) + H2O(l) ⇌ NH4+(aq) + OH-(aq), is 11.13.
- Hydrofluoric acid with Ka = 3.5 × 10-4 is the strongest monoprotic acid of the set, assuming all acids are at 0.100 M concentration.
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