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Questions and Answers
Which of the following statements correctly describes the behavior of ampholytes?
Which of the following statements correctly describes the behavior of ampholytes?
- They can only donate protons in a solution.
- They neither accept nor donate protons.
- They can either accept or donate protons. (correct)
- They can only accept protons in a solution.
According to the Brønsted-Lowry definition, what characterizes a base?
According to the Brønsted-Lowry definition, what characterizes a base?
- A substance that increases the concentration of hydronium ions in water.
- A substance that donates protons (H+).
- A substance that accepts protons (H+). (correct)
- A substance that donates hydroxide ions (OH-).
Which of these aqueous solutions would be considered alkaline?
Which of these aqueous solutions would be considered alkaline?
- A solution with a pH of 8. (correct)
- A solution with a pH of 0.
- A solution with a pH of 6.
- A solution with a pH of 7.
In the following reaction: HBr + H2O → Br- + H3O+, which species acts as the Brønsted-Lowry acid?
In the following reaction: HBr + H2O → Br- + H3O+, which species acts as the Brønsted-Lowry acid?
Which of the following is the conjugate base of sulfuric acid (H2SO4)?
Which of the following is the conjugate base of sulfuric acid (H2SO4)?
Which of the following best describes the behavior of water in the autoprotolysis process?
Which of the following best describes the behavior of water in the autoprotolysis process?
Which of the following is a strong base that forms a kalilauge (potash lye) when dissolved in water?
Which of the following is a strong base that forms a kalilauge (potash lye) when dissolved in water?
Which of the following acids is commonly known as Essigsäure?
Which of the following acids is commonly known as Essigsäure?
How do acids influence the concentration of hydrogen ions (H+) in an aqueous solution, according to Arrhenius?
How do acids influence the concentration of hydrogen ions (H+) in an aqueous solution, according to Arrhenius?
What characterizes the pH value of a neutral solution?
What characterizes the pH value of a neutral solution?
Flashcards
What is a Bronsted acid?
What is a Bronsted acid?
A substance that donates protons (H⁺ ions) in a chemical reaction.
What is a Bronsted base?
What is a Bronsted base?
A substance that accepts protons (H⁺ ions) in a chemical reaction.
What are ampholytes?
What are ampholytes?
Substances that can act as both acids and bases by either donating or accepting protons.
What is the pH value?
What is the pH value?
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What is the pH value of an acidic solution?
What is the pH value of an acidic solution?
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What is the pH value of a basic solution?
What is the pH value of a basic solution?
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What are conjugate acid-base pairs?
What are conjugate acid-base pairs?
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What is Sodium Hydroxide (NaOH)?
What is Sodium Hydroxide (NaOH)?
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How do acids affect H+ ion concentration?
How do acids affect H+ ion concentration?
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How do bases affect OH- ion concentration?
How do bases affect OH- ion concentration?
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Study Notes
- These are notes on acid-base reactions.
Important Molecular Ions
- SO42- is a sulfate ion.
- PO43- is a phosphate ion.
- NO3 is a nitrate ion.
- CO32- is a carbonate ion.
- OH- is a hydroxide ion.
- NH4+ is an ammonium ion.
- H3O+ is an oxonium ion.
- Na+ is a sodium ion.
- K+ is a potassium ion.
- Cl- is a chloride ion.
Important Acids
- H2SO4 is sulfuric acid.
- H3PO4 is phosphoric acid.
- HNO3 is nitric acid.
- H2CO3 is carbonic acid.
- HCN hydrocyanic acid.
- HCl is hydrochloric acid.
- CH3COOH is acetic acid.
- HBR is hydrogen bromide.
Important Bases
- NaOH sodium hydroxide becomes sodium hydroxide solution in water.
- KOH potassium hydroxide becomes potassium hydroxide solution in water.
- Ca(OH)2 calcium hydroxide becomes limewater in water.
- NH3 ammonia becomes ammonia water (NH4OH) in water.
- Na2CO3 is sodium carbonate.
Ampholytes
- Ampholytes can both accept and donate protons (H+ ions).
- Examples of ampholytes include H2O (water), CH3COOH (acetic acid), and NH3 (ammonia).
PH Value
- The pH value is a measure for characterizing an acidic, basic, or neutral solution; pH indicates the concentration of hydroxide ions.
- pH values range from 0 to 6.9 representing acidic.
- pH value of 7 is neutral.
- pH values range from 7.1 to 14, which is basic.
Acids
- According to Arrhenius, acids are substances that release protons (H+ ions) in aqueous solutions; this only applies to aqueous solutions.
- Acids increase the H+ ion concentration in water.
- According to Brønsted, acids are substances that release protons (H+ ions), and bases are substances that accept protons.
- Acids dissociate (break down) in aqueous solution into positively charged hydrogen ions (protons) and negatively charged acid residue ions.
- Acids are proton donors.
- Bases are proton acceptors; this also applies in gases and other solvents, not just water.
Bases
- Bases are substances that accept protons (proton acceptors).
- In solutions, bases are alkaline and have a higher pH value than 7.
- Bases dissociate in aqueous solution into positively charged metal ions and negatively charged hydroxide ions (OH-).
Autoprotolysis of Water
- Water can both accept and donate protons.
- In most cases, water accepts protons to form oxonium ions (H3O+).
Acid-Base Pairs
- Each time an acid releases a proton, it forms a conjugate base.
- Conversely, when a base accepts a proton, it forms a conjugate acid.
- HBr + H2O → Br- + H3O+
- Hydrogen bromide (HBr) is acid 1.
- Water (H2O) is base 2.
- Bromide ion (Br-) is base 1.
- Oxonium ion (H3O+) is acid 2.
- Acid 1 transforms into base 1.
- Acid 2 transforms into base 2.
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