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Questions and Answers
Which statement accurately describes a Bronsted-Lowry acid?
Which statement accurately describes a Bronsted-Lowry acid?
- It donates electrons to a base.
- It accepts a proton from another substance.
- It donates a proton to a base. (correct)
- It remains neutral during a reaction.
In the Bronsted-Lowry theory, what is a base characterized by?
In the Bronsted-Lowry theory, what is a base characterized by?
- A substance that increases the concentration of hydroxide ions in solution.
- A substance that donates electrons to the surrounding environment.
- A substance that has no effect on the solution's acidity.
- A substance that accepts a proton from an acid. (correct)
Which of the following pairs is an example of a Bronsted-Lowry acid-base reaction?
Which of the following pairs is an example of a Bronsted-Lowry acid-base reaction?
- NH3 + H2O ⇌ NH4+ + OH− (correct)
- H2 + Cl2 → 2HCl
- CaCO3 + H2SO4 → CaSO4 + H2O + CO2
- NaOH + HCl → NaCl + H2O
What happens during the ionization of a Bronsted-Lowry acid in water?
What happens during the ionization of a Bronsted-Lowry acid in water?
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What is the conjugate base of the strong acid hydrochloric acid (HCl)?
What is the conjugate base of the strong acid hydrochloric acid (HCl)?
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Study Notes
Bronsted-Lowry Acids
- A Bronsted-Lowry acid is a substance that donates a proton (H+)
- A proton is the nucleus of a hydrogen atom, which consists of a single positively charged particle
Bronsted-Lowry Bases
- A Bronsted-Lowry base is a substance that accepts a proton (H+)
Bronsted-Lowry Acid-Base Reactions
- In a Bronsted-Lowry acid-base reaction, a proton is transferred from an acid to a base
- The acid loses a proton and becomes its conjugate base
- The base gains a proton and becomes its conjugate acid
- Example of a Bronsted-Lowry acid-base reaction: HCl (acid) + H2O (base) -> H3O+ (conjugate acid) + Cl- (conjugate base)
Ionization of Bronsted-Lowry Acids in Water
- When a Bronsted-Lowry acid ionizes in water, it donates a proton to a water molecule
- The water molecule acts as a base and accepts the proton, forming the hydronium ion (H3O+)
Conjugate Base of Hydrochloric Acid
- The conjugate base of hydrochloric acid (HCl) is chloride ion (Cl-)
- When HCl acts as a Bronsted-Lowry acid, it donates a proton (H+), leaving behind the chloride ion (Cl-)
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