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Questions and Answers
A solution has a hydroxide ion concentration of $1.0 x 10^{-5}$ M at 25°C. What is the pH of the solution?
A solution has a hydroxide ion concentration of $1.0 x 10^{-5}$ M at 25°C. What is the pH of the solution?
- 9.0 (correct)
- 5.0
- 10.0
- 4.0
Which statement accurately describes a Brønsted-Lowry acid?
Which statement accurately describes a Brønsted-Lowry acid?
- A substance that donates an electron pair.
- A substance that accepts a proton.
- A substance that donates a proton. (correct)
- A substance that accepts an electron pair.
What is the pH of a 0.020 M solution of a strong monoprotic acid?
What is the pH of a 0.020 M solution of a strong monoprotic acid?
- 1.70 (correct)
- 3.40
- 12.00
- 2.00
A 0.10 M solution of a weak base has a pH of 11.3. What is the approximate value of Kb for this base?
A 0.10 M solution of a weak base has a pH of 11.3. What is the approximate value of Kb for this base?
Which of the following salts will produce a basic solution when dissolved in water?
Which of the following salts will produce a basic solution when dissolved in water?
For a diprotic acid, H2A, which of the following relationships is always true?
For a diprotic acid, H2A, which of the following relationships is always true?
What is the hydronium ion concentration in a neutral solution at 25°C?
What is the hydronium ion concentration in a neutral solution at 25°C?
Which of the following is a conjugate acid-base pair according to the Brønsted-Lowry theory?
Which of the following is a conjugate acid-base pair according to the Brønsted-Lowry theory?
What is the pOH of a solution with a pH of 3.6 at 25°C?
What is the pOH of a solution with a pH of 3.6 at 25°C?
Which of the following is true regarding strong acids and bases in aqueous solutions?
Which of the following is true regarding strong acids and bases in aqueous solutions?
Flashcards
Brønsted theory
Brønsted theory
Acids are proton donors, and bases are proton acceptors.
Kw
Kw
The ion-product constant for water, representing the equilibrium between H3O+ and OH- in water.
Formula for pH Calculation
Formula for pH Calculation
pH = -log[H3O+], where [H3O+] is the concentration of hydronium ions.
Strong acids/bases
Strong acids/bases
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Weak acid/base
Weak acid/base
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Salts
Salts
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Diprotic acids
Diprotic acids
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Study Notes
- Quiz 5 on Chapter 17 will have 6 questions and you will have 60 minutes to complete it.
Brønsted Theory
- Understand the concepts of Brønsted theory.
Kw and Ion-Product Constant for Water
- Kw = [H3O+][OH-] = 1.0 x 10^-14 at 25°C, which is the ion-product constant for water.
pH Calculations
- Be able to perform pH calculations in solutions of:
- Strong acids/bases
- Weak acids/bases
- Salts
- Diprotic acids
Study Tip
- Practice problems are recommended as a good way to study.
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