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Chapter 15: Problem 46

Write the formula for the conjugate base of the following acids: (a) \(\mathrm{HBrO}_{3}\) (b) \(\mathrm{NH}_{4}^{+}\) (c) \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}\)

Short Answer

Expert verified
(a) \(\text{BrO}_3^-\), (b) \(\text{NH}_3\), (c) \(\text{HPO}_4^{2-}\)

Step by step solution

01

Identify the Acid

Determine the acid given in each part of the problem. For part (a), the acid is \(\text{HBrO}_3\). For part (b), the acid is \(\text{NH}_4^+\). For part (c), the acid is \(\text{H}_2 \text{PO}_4^-\).
02

Understand the Concept of Conjugate Base

A conjugate base is formed by removing one proton (H⁺) from the acid. For each given acid in the problem, subtract one hydrogen ion (H⁺) from the molecular formula.
03

Calculate the Conjugate Base for \(\text{HBrO}_3\)

Remove one proton (H⁺) from \(\text{HBrO}_3\) resulting in the conjugate base \(\text{BrO}_3^-\text{H}-H^+ = \text{BrO}_3^-\). The conjugate base is \(\text{BrO}_3^-\).
04

Calculate the Conjugate Base for \(\text{NH}_4^+\)

Remove one proton (H⁺) from \(\text{NH}_4^+\) resulting in the conjugate base \(\text{NH}_3\text{H} - H^+ = \text{NH}_3\). The conjugate base is \(\text{NH}_3\).
05

Calculate the Conjugate Base for \(\text{H}_2 \text{PO}_4^-\)

Remove one proton (H⁺) from \(\text{H}_2 \text{PO}_4^-\) resulting in the conjugate base \(\text{HPO}_4^{2-}\text{H} - H^+ = \text{HPO}_4^{2-}\). The conjugate base is \(\text{HPO}_4^{2-}\).

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Acid-Base Chemistry
Acid-base chemistry focuses on the reactions between acids and bases. An acid is a substance that donates a proton (H⁺), and a base is a substance that accepts a proton. The strength of an acid or a base depends on its ability to lose or gain a proton.

  • Strong acids completely dissociate in water, releasing protons.
  • Weak acids only partially dissociate in water.
  • Similarly, strong bases fully accept protons, while weak bases do so partially.


When acids and bases react, they form conjugate pairs. When an acid loses a proton, its conjugate base is formed. Conversely, when a base gains a proton, it forms its conjugate acid. This concept is crucial in understanding the following topic of proton transfer.
Proton Transfer
Proton transfer is a fundamental process in acid-base reactions. It involves the movement of a proton (H⁺) from an acid to a base. This step is pivotal in defining conjugate acid-base pairs.

Let's explore this concept with examples:
  • For the acid \(\mathrm{HBrO}_3\), removing a single proton forms the conjugate base \(\mathrm{BrO}_3^{-}\).
  • In the case of \(\mathrm{NH}_4^{+}\), subtraction of a proton yields \(\mathrm{NH}_3\), the conjugate base.
  • Finally, \(\mathrm{H}_2 \mathrm{PO}_4^{-}\) loses one proton to form \(\mathrm{HPO}_4^{2-}\).


Proton transfer is integral to numerous chemical reactions. It allows chemists to predict the outcomes of acid-base reactions. Understanding how substances behave as acids or bases in different reactions is foundational in chemistry.
Chemical Formulas
Chemical formulas represent the composition of molecules and compounds. Each formula contains symbols of the elements present and subscripts indicating the number of atoms of each element in the compound.

For acidity and basicity assessments, knowing the chemical formula helps identify potential proton sources or sinks.

Take the following acids, for example:
  • \(\mathrm{HBrO}_3\): Here, one hydrogen atom is available for transfer.
  • \(\mathrm{NH}_4^{+}\): Four hydrogen atoms are present; one can be removed to form \(\mathrm{NH}_3\).
  • \(\mathrm{H}_2 \mathrm{PO}_4^{-}\): Two hydrogen atoms are candidates for removal, leading to \(\mathrm{HPO}_4^{2-}\) with one less proton.


Chemical formulas also reflect charge changes resulting from proton transfer. Post-transfer, acids become conjugate bases with altered charges, showcasing the direct connection between proton transfer and chemical formulas.

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Most popular questions from this chapter

Determine whether each of the following is a strong acid, weak acid, strong base, or weak base. Then write an equation describing the process that occurs when the substance is dissolved in water. (a) \(\mathrm{NH}_{3}\) (b) \(\mathrm{HCl}\) (c) \(\mathrm{KOH}\) (d) \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\)

A \(10.0-\mathrm{mL}\) sample of \(\mathrm{HNO}_{3}\) was diluted to a volume of \(100.00 \mathrm{~mL}\). Then \(25 \mathrm{~mL}\) of that diluted solution were needed to neutralize \(50.0 \mathrm{~mL}\) of \(0.60 \mathrm{M} \mathrm{KOH}\). What was the concentration of the original nitric acid?

Sulfuric acid reacts with NaOH: (a) Write a balanced equation for the reaction producing \(\mathrm{Na}_{2} \mathrm{SO}_{4}\). (b) How many milliliters of \(0.10 \mathrm{M} \mathrm{NaOH}\) are needed to react with \(0.0050 \mathrm{~mol} \mathrm{H}_{2} \mathrm{SO}_{4}\) ? (c) How many grams of \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) will also form?

Determine how many grams of \(\mathrm{Al}(\mathrm{OH})_{3}\) will be required to neutralize \(275 \mathrm{~mL}\) of \(0.125 \mathrm{M} \mathrm{HCl}\) according to the reaction: $$ 3 \mathrm{HCl}(a q)+\mathrm{Al}(\mathrm{OH})_{3}(s) \longrightarrow \mathrm{AlCl}_{3}(a q)+3 \mathrm{H}_{2} \mathrm{O}(l) $$

Identify the conjugate acid-base pairs in each of the following equations: (a) \(\mathrm{NH}_{3}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{NH}_{4}^{+}+\mathrm{OH}^{-}\) (b) \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}^{-}+\mathrm{H}_{3} \mathrm{O}^{+}\) (c) \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}+\mathrm{OH}^{-} \rightleftharpoons \mathrm{HPO}_{4}^{2-}+\mathrm{H}_{2} \mathrm{O}\) (d) \(\mathrm{HCl}+\mathrm{H}_{2} \mathrm{O} \longrightarrow \mathrm{Cl}^{-}+\mathrm{H}_{3} \mathrm{O}^{+}\)
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