Textbook Question
The following picture represents the hydrated metal cation M1H2O26 n + , where n = 1, 2, or 3.
(b) Does the equilibrium constant increase, decrease, or remain the same as the value of n increases? Explain.
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Ch.16 - Aqueous Equilibria: Acids & Bases
Chapter 16, Problem 48
Which of the following are Brønsted–Lowry bases but not Arrhenius bases? (a) NH3 (b) HCO3-
Verified step by step guidance1
Step 1: Understand the definitions of Brønsted–Lowry and Arrhenius bases. A Brønsted–Lowry base is a substance that can accept a proton (H+), while an Arrhenius base is a substance that increases the concentration of OH- ions in aqueous solution.
Step 2: Analyze NH3 (ammonia). NH3 can accept a proton to form NH4+, making it a Brønsted–Lowry base. However, it does not directly produce OH- ions in solution, so it is not an Arrhenius base.
Step 3: Analyze HCO3- (bicarbonate ion). HCO3- can accept a proton to form H2CO3, making it a Brønsted–Lowry base. It can also react with water to produce OH- ions, so it can act as an Arrhenius base as well.
Step 4: Compare the two substances. NH3 is a Brønsted–Lowry base but not an Arrhenius base, while HCO3- can act as both.
Step 5: Conclude that NH3 is the substance that fits the criteria of being a Brønsted–Lowry base but not an Arrhenius base.
Related Practice
Textbook Question
The following picture represents the hydrated metal cation M1H2O26 n + , where n = 1, 2, or 3. (c) Which M1H2O26n + ion 1n = 1,2, or 32 is the strongest acid, and which has the strongest conjugate base?
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Textbook Question
Look at the electron-dot structures of the following molecules
and ions:
(b) Which can behave as a Lewis acid? Which can behave as
a Lewis base?
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Open Question
Which of the following can behave both as a Brønsted–Lowry acid and as a Brønsted–Lowry base? (a) HCO3- (b) CN- (c) H2O (d) H2CO3
Textbook Question
Aqueous solutions of hydrogen sulfide contain H2S, HS-,
S2-, H3O+ , OH-, and H2O in varying concentrations. Which
of these species can act only as an acid? Which can act only as
a base? Which can act both as an acid and as a base?
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Textbook Question
The hydronium ion H3O+ is the strongest acid that can exist
in aqueous solution because stronger acids dissociate by
transferring a proton to water. What is the strongest base
that can exist in aqueous solution?
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