Identifying and Defining Acids and Bases - SAT Subject Test in Chemistry

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Question

Which of the following cannot act as a Bronsted-Lowry base (proton recipient) in aqueous solution?

Answer

cannot receive another proton because then it would become $NH_5^{2+}$ , which does not exist. All of the other answer choices are fine:

$NH_3 \Rightarrow NH_4^+$

$HCO_3^-\Rightarrow H_2CO_3$

$H_2O\Rightarrow H_3O^+$

$OH^-\Rightarrow H_2O$

Compare your answer with the correct one above

Question

Which of the following cannot act as a Bronsted-Lowry base (proton recipient) in aqueous solution?

Answer

cannot receive another proton because then it would become $NH_5^{2+}$ , which does not exist. All of the other answer choices are fine:

$NH_3 \Rightarrow NH_4^+$

$HCO_3^-\Rightarrow H_2CO_3$

$H_2O\Rightarrow H_3O^+$

$OH^-\Rightarrow H_2O$

Compare your answer with the correct one above

Question

Which of the following cannot act as a Bronsted-Lowry base (proton recipient) in aqueous solution?

Answer

cannot receive another proton because then it would become $NH_5^{2+}$ , which does not exist. All of the other answer choices are fine:

$NH_3 \Rightarrow NH_4^+$

$HCO_3^-\Rightarrow H_2CO_3$

$H_2O\Rightarrow H_3O^+$

$OH^-\Rightarrow H_2O$

Compare your answer with the correct one above

Question

Which of the following cannot act as a Bronsted-Lowry base (proton recipient) in aqueous solution?

Answer

cannot receive another proton because then it would become $NH_5^{2+}$ , which does not exist. All of the other answer choices are fine:

$NH_3 \Rightarrow NH_4^+$

$HCO_3^-\Rightarrow H_2CO_3$

$H_2O\Rightarrow H_3O^+$

$OH^-\Rightarrow H_2O$

Compare your answer with the correct one above

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