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Magazine Chapter 15: Problem 91
Write the conjugate base for each of the following: a. \(\mathrm{H}_{3} \mathrm{PO}_{4}\) b. \(\mathrm{HCO}_{3}^{-}\) C. \(HF\) d. \(\mathrm{H}_{2} \mathrm{SO}_{4}\)
Short Answer
Expert verified
The conjugate bases are:
a. \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}\)
b. \(\mathrm{CO}_{3}^{2-}\)
c. \(F^{-}\)
d. \(\mathrm{HSO}_{4}^{-}\)
Step by step solution
01
Remove a proton (H+) from the given acid for (a)
For the first acid, \(\mathrm{H}_{3} \mathrm{PO}_{4}\), we will remove one proton (H+). So we get,
\(\mathrm{H}_{3} \mathrm{PO}_{4} - \mathrm{H}^{+}\)
02
Write the conjugate base for (a)
After removing one proton from \(\mathrm{H}_{3} \mathrm{PO}_{4}\), the remaining chemical species is \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}\) . So, the conjugate base for (a) is \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}\).
03
Remove a proton (H+) from the given acid for (b)
For the second chemical species, \(\mathrm{HCO}_{3}^{-}\), we will remove one proton (H+). So we get,
\(\mathrm{HCO}_{3}^{-} - \mathrm{H}^{+}\)
04
Write the conjugate base for (b)
After removing one proton from \(\mathrm{HCO}_{3}^{-}\), the remaining chemical species is \(\mathrm{CO}_{3}^{2-}\) . So, the conjugate base for (b) is \(\mathrm{CO}_{3}^{2-}\).
05
Remove a proton (H+) from the given acid for (c)
For the third compound, \(HF\), we will remove one proton (H+). So we get,
\(HF - \mathrm{H}^{+}\)
06
Write the conjugate base for (c)
After removing one proton from \(HF\), the remaining chemical species is \(F^{-}\) . So, the conjugate base for (c) is \(F^{-}\).
07
Remove a proton (H+) from the given acid for (d)
For the fourth acid, \(\mathrm{H}_{2} \mathrm{SO}_{4}\), we will remove one proton (H+). So we get,
\(\mathrm{H}_{2} \mathrm{SO}_{4} - \mathrm{H}^{+}\)
08
Write the conjugate base for (d)
After removing one proton from \(\mathrm{H}_{2} \mathrm{SO}_{4}\), the remaining chemical species is \(\mathrm{HSO}_{4}^{-}\) . So, the conjugate base for (d) is \(\mathrm{HSO}_{4}^{-}\).
The conjugate bases for the given acids are:
a. \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}\)
b. \(\mathrm{CO}_{3}^{2-}\)
c. \(F^{-}\)
d. \(\mathrm{HSO}_{4}^{-}\)
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Acid-Base Reactions
In chemistry, acid-base reactions are fundamental processes in which acids and bases interact to form different substances. Think of an acid as a substance that can donate a proton (H+), while a base is something that can accept a proton. When they meet, they often form water and a salt.
This process of proton donation and acceptance forms the basis of many chemical reactions.
This process of proton donation and acceptance forms the basis of many chemical reactions.
- For example, if we mix hydrochloric acid (HCl) with sodium hydroxide (NaOH), an acid-base reaction will occur, producing water (H2O) and sodium chloride (NaCl), which is common table salt.
- These reactions are central to a wide range of chemical processes, from digestion in living organisms to acid rain formation in the environment.
Bronsted-Lowry Theory
The Bronsted-Lowry theory brings a new perspective to the concept of acids and bases. This theory defines acids and bases by their ability to donate or accept protons.
An acid is a substance that donates a proton, while a base is one that accepts it. This idea broadens the kinds of molecules that can be considered acids or bases.
An acid is a substance that donates a proton, while a base is one that accepts it. This idea broadens the kinds of molecules that can be considered acids or bases.
- For instance, water is not only a compound that can act as a solvent but also plays dual roles in acid-base reactions, either accepting protons to become hydronium ions (H3O+) or donating protons to become hydroxide ions (OH-).
- This approach replaces the older concept of acids and bases being limited to those substances that produce H+ or OH- in water.
Proton Transfer
Proton transfer is a critical aspect of chemical reactions, particularly in the context of the Bronsted-Lowry theory. When we say a "proton," we refer to a hydrogen atom that has lost its electron, making it a positively charged ion (H+).
In acid-base chemistry, proton transfer involves moving this proton from an acid to a base, which changes the chemical nature of these substances.
In acid-base chemistry, proton transfer involves moving this proton from an acid to a base, which changes the chemical nature of these substances.
- For example, when hydrogen fluoride (HF) acts as an acid, it donates a proton to become fluoride (F鈭�), while the proton is transferred to a base, like water, producing hydronium (H3O+).
- This movement of protons is a key process in not only simple chemical reactions but also complex biological functions, like cellular respiration and metabolism.
