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Chapter 6: Problem 36

Which of the following species cannot have conjugate base? (a) \(\mathrm{HSO}_{4}^{-}\) (b) \(\mathrm{HPO}_{4}^{-2}\) (c) \(\mathrm{PO}_{4}^{-3}\) (d) \(\mathrm{H}_{2} \mathrm{PO}_{2}^{-}\)

Short Answer

Expert verified
Answer: (c) \(\mathrm{PO}_{4}^{-3}\)

Step by step solution

01

Determine if each species can lose a proton.

Examine each species and determine if they can lose a proton: (a) \(\mathrm{HSO}_{4}^{-}\): Yes, it can lose an \(\mathrm{H}\), forming \(\mathrm{SO}_{4}^{-2}\). (b) \(\mathrm{HPO}_{4}^{-2}\): Yes, it can lose an \(\mathrm{H}\), forming \(\mathrm{PO}_{4}^{-3}\). (c) \(\mathrm{PO}_{4}^{-3}\): It doesn't have any \(\mathrm{H}\) to lose, so it cannot form a conjugate base. (d) \(\mathrm{H}_{2} \mathrm{PO}_{2}^{-}\): Yes, it can lose an \(\mathrm{H}\), forming \(\mathrm{HPO}_{2}^{-2}\).
02

Identify the species that cannot have a conjugate base.

Based on our analysis, the species that cannot have a conjugate base is option (c) \(\mathrm{PO}_{4}^{-3}\), because it cannot lose a proton.

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Most popular questions from this chapter

Which of the following acts as both Bronsted acid and Lewis acid? (a) \(\mathrm{Cu}^{+2}\) (b) \(\mathrm{SO}_{2}\) (c) \(\mathrm{Fe}^{+3}\) (d) \(\mathrm{NH}_{4}{ }^{+}\)

State whether the following statements are true or false. \(\mathrm{S}^{-2}\) is the conjugate base of \(\mathrm{HS}^{-}\)

Which of the following cannot show acidic nature? (a) \(\mathrm{H}_{2} \mathrm{CO}_{3}\) (b) \(\mathrm{CaCO}_{3}\) (c) \(\mathrm{HCl}\) (d) \(\mathrm{HSO}_{4}^{-}\)

Which of the following \(\mathrm{pH}\) values at \(25^{\circ} \mathrm{C}\) corresponds to the strongest acid? (a) 2 (b) 4 (c) 6 (d) 8

State whether the following statements are true or false. \(\mathrm{K}_{2} \mathrm{SO}_{4} \cdot \mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3} 24 \mathrm{H}_{2} \mathrm{O}\) gives reactions of both \(\mathrm{K}^{+}\) and \(\mathrm{Al}^{+3}\) ions respectively.
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