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Brønsted-Lowry Acids & Bases
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Brønsted-Lowry Acids & Bases
Consider the reaction:
NH3 (aq) + H2O (l) ⇌ NH4+ (aq) + OH- (aq)
Ammonia (NH3) reacts with water (H2O) to form ammonium ions (NH4+) and hydroxide ions (OH−) in an equilibrium reaction
Identify the Brønsted-Lowry acid and base in the forward reaction.
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Write the formula for the conjugate acid and conjugate base that are formed in this reaction.
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Explain why an ammonium ion can not behave as a Brønsted-Lowry base.
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An alkaline solution is formed when sodium hydrogencarbonate (NaHCO3) is dissolved in water.
Write an equation for the reaction and explain why the solution is alkaline.
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Carbonic acid (H2CO3) dissociates in two steps:
H2CO3 (aq) ⇌ H+ (aq) + HCO3− (aq)
HCO3− (aq) ⇌ H+ (aq) + CO32− (aq)
Using this information, identify the conjugate base of HCO3−. Justify your answer.
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State whether the HCO3- ion is behaving as a Brønsted–Lowry acid or as a base and give a reason for your answer.
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Consider the following reaction:
H2S (aq) + H2O (l) ⇌ HS- (aq) + H3O+ (aq)
Identify the conjugate acid-base pairs in this reaction.
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i) Determine whether H2S is a strong acid or a weak acid.
ii) Explain how the strength of its conjugate base is affected.
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Consider the reaction of pyridine (C5H5N) with water:
C5H5N (aq) + H2O (l) ⇌ C5H5NH+ (aq) + OH− (aq)
Compare the role of water in this reaction to its role in the hydrogen sulfide reaction, and explain the difference. [1 point]
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Methylamine (CH3NH2) is a weak base that reacts with water as follows:
CH3NH2 (aq) + H2O (l) ⇌ CH3NH3+ (aq) + OH− (aq)
The conjugate acid, CH3NH3+, can also act as an acid in water:
CH3NH3+ (aq) + H2O (l) ⇌ CH3NH2 (aq) + H3O+ (aq)
Identify the conjugate acid-base pairs in the reaction between methylamine and water.
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Using the equations given in part (a), explain why CH3NH3+ is considered a weak acid, while OH− is a strong base.
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Compare the role and relative strength of water in the two reactions provided.
Explain how the stability of its conjugate pairs contributes to its behavior.
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The reaction of acetic acid (CH3COOH) with ammonia (NH3) in a non-aqueous solvent is shown below:
CH3COOH + NH3 ⇌ CH3COO− + NH4+
Identify the Brønsted-Lowry acid and base in this reaction.
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Predict how increasing the concentration of NH3 in the solvent could shift the position of equilibrium in this reaction. Justify your answer.
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Explain how the solvent affects the strength of the acid and base in this reaction compared to the same reaction in water.
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