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Chapter 8: Problem 50

Write the formula of each base's conjugate acid. a. \(\mathrm{BrO}_{3}^{-}\) b. \(\mathrm{NH}_{3}\) c. \(\mathrm{CH}_{3} \mathrm{COO}^{-}\) d. \(\mathrm{HCO}_{3}^{-}\) e. \(\mathrm{CN}^{-}\) f. \(\mathrm{HPO}_{4}^{2-}\) g. HS- \(\mathrm{h} . \mathrm{SO}_{4}^{2-}\) i. \(\mathrm{CO}_{3}^{2-}\) \(\mathrm{j} . \mathrm{HCO}_{3}^{-}\) k. \(\mathrm{PH}_{3}\)

Short Answer

Expert verified
Add a proton to each base to find its conjugate acid: HBrO鈧�, NH鈧勨伜, CH鈧僀OOH, H鈧侰O鈧�, HCN, H鈧侾O鈧勨伝, H鈧係, HSO鈧勨伝, HCO鈧冣伝, H鈧侰O鈧�, PH鈧勨伜.

Step by step solution

01

Identify the Base

A base is a substance that can accept a proton (a hydrogen ion, H鈦�). We need to identify each base from the problem question.
02

Add a Proton

To find the conjugate acid of each base, add one hydrogen ion (H鈦�) to the chemical formula of the base. This addition increases the positive charge of the base by +1.
03

Write the Conjugate Acid Formula

For each base provided:- a. Add \[\mathrm{H^{+}} + \mathrm{BrO}_{3}^{-} \rightarrow \mathrm{HBrO}_{3}\]- b. Add \[\mathrm{H^{+}} + \mathrm{NH}_{3} \rightarrow \mathrm{NH}_{4}^{+}\]- c. Add \[\mathrm{H^{+}} + \mathrm{CH}_{3} \mathrm{COO}^{-} \rightarrow \mathrm{CH}_{3} \mathrm{COOH}\]- d. Add \[\mathrm{H^{+}} + \mathrm{HCO}_{3}^{-} \rightarrow \mathrm{H}_{2}\mathrm{CO}_{3}\]- e. Add \[\mathrm{H^{+}} + \mathrm{CN}^{-} \rightarrow \mathrm{HCN}\]- f. Add \[\mathrm{H^{+}} + \mathrm{HPO}_{4}^{2-} \rightarrow \mathrm{H}_{2}\mathrm{PO}_{4}^{-}\]- g. Add \[\mathrm{H^{+}} + \mathrm{HS}^{-} \rightarrow \mathrm{H}_{2}\mathrm{S}\]- h. Add \[\mathrm{H^{+}} + \mathrm{SO}_{4}^{2-} \rightarrow \mathrm{HSO}_{4}^{-}\]- i. Add \[\mathrm{H^{+}} + \mathrm{CO}_{3}^{2-} \rightarrow \mathrm{HCO}_{3}^{-}\]- j. Add \[\mathrm{H^{+}} + \mathrm{HCO}_{3}^{-} \rightarrow \mathrm{H}_{2}\mathrm{CO}_{3}\]- k. Add \[\mathrm{H^{+}} + \mathrm{PH}_{3} \rightarrow \mathrm{PH}_{4}^{+}\]
04

Confirmation

Double-check the charge conservation and correct molecular structure for the conjugate acids found in the previous step to ensure each conjugate acid is formed correctly.

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Key Concepts

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

Acid-Base Reactions
Acid-base reactions are fundamental chemical processes where an acid donates a proton (H鈦�) and a base accepts it. In these reactions, two things happen simultaneously. The acid becomes its conjugate base, and the base becomes its conjugate acid. This concept is crucial for understanding the behavior of substances in a solution. Consider the acid as a proton donor: when it loses this proton, it transforms into its conjugate base. The base, on the other hand, acts as a proton acceptor. When it gains a proton, it becomes its conjugate acid. These reactions are reversible, often reaching an equilibrium state where the forward and reverse reactions occur at equal rates. This equilibrium is central to many natural and industrial processes, like acidification of oceans and processes in our bodies. Remember, the strength of acids and bases varies widely, affecting how readily they donate or accept protons.
Proton Transfer
Proton transfer is the essential process that occurs during acid-base reactions. It involves the transfer of a proton from an acid to a base. This proton is essentially a hydrogen ion (H鈦�), which carries a positive charge. This transfer is the main reason why chemical formulas of acids and bases change during reactions. For example, when an acid donates a proton, its formula changes, leaving behind its conjugate base. The base, after accepting a proton, becomes the conjugate acid. This movement of protons is what makes the chemical reactions dynamic and is a key reason why such reactions can shift equilibrium in a solution. Understanding proton transfer helps predict the outcomes of reactions and is fundamental in fields such as biochemistry and pharmacology, where the ability of molecules to donate or accept protons affects their function.
Chemical Formulas
Chemical formulas represent the types and numbers of atoms in a molecule. When identifying conjugate acids, it's essential to alter these formulas to reflect the addition of a proton. For instance, for a base like \(\mathrm{NH}_3\), after accepting a proton, it becomes \(\mathrm{NH}_4^+\). The chemical formula is slightly altered to show the increase in hydrogen atoms and the overall charge change.Chemical formulas serve as a shorthand to convey complex information about the composition and structure of molecules. Understanding them is crucial for predicting how substances will interact in chemical reactions. Each atom's symbol, and any associated charge, provides valuable information about the molecule's potential reactivity and the stability of its conjugate partners. This understanding is especially useful in chemistry labs or industries where predicting reactions is necessary for safety and efficacy.
Charge Conservation
Charge conservation is a fundamental principle in chemistry, stating that the total charge before and after a chemical reaction must remain constant. When a base accepts a proton to form a conjugate acid, its charge typically increases by +1 due to the addition of a positively charged hydrogen ion (H鈦�). For example, when \(\mathrm{CN}^{-}\) accepts a proton, it becomes \(\mathrm{HCN}\), moving from a -1 charge to an overall neutral charge.Ensuring charge conservation is critical for balancing chemical equations correctly. It helps chemists confirm that chemical reactions are balanced not only in terms of atoms but also in terms of charge. This balancing is pivotal when predicting how reactions proceed and ensuring that calculations of reactants and products are accurate. Misunderstanding charge balance can lead to errors in chemical predictions, proving the importance of this concept in both theoretical and practical chemistry.

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Most popular questions from this chapter

Identify each reactant in the following reactions as an acid or a base according to the Br酶nsted-Lowry theory. a. \(\mathrm{HIO}_{3}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{IO}_{3}^{-}(a q)+\mathrm{H}_{3} \mathrm{O}^{+}(a q)\) b. \(\mathrm{F}^{-}(a q)+\mathrm{HClO}(a q) \rightleftharpoons \mathrm{HF}(a q)+\mathrm{ClO}^{-}(a q)\) ?. \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}(a q)+\mathrm{OH}^{-}(a q) \rightleftharpoons \mathrm{HPO}_{4}^{2-}(a q)+\mathrm{H}_{2} \mathrm{O}(l)\) d. \(\mathrm{CO}_{3}^{2-}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{HCO}_{3}^{-}(a q)+\mathrm{OH}^{-}(a q)\)

Explain why the hydrogen phosphate ion \(\left(\mathrm{HPO}_{4}^{2-}\right)\) is amphoteric.

Two solutions are separated by a semipermeable membrane. Solution A contains \(25.0 \mathrm{~g}\) of \(\mathrm{NaCl}\) in \(100.0 \mathrm{~mL}\) of water and solution B contains \(35.0\) g of \(\mathrm{NaCl}\) in \(100.0 \mathrm{~mL}\) of water. a. Which one has a higher concentration? b. Which way will water molecules flow? c. Which volume will increase? d. Which volume will decrease? e. What will happen to the concentration of solution \(\mathrm{A}\) ? f. What will happen to the concentration of solution \(\mathrm{B}\) ?

What does it mean if the \(\mathrm{K}_{\mathrm{eq}}\) is \(<1\) ?

A solution contains \(128 \mathrm{mEq} / \mathrm{L}\) of \(\mathrm{Sr}^{2+}\). What volume of solution is needed to have a total mass of \(3.93\) g of strontium ions?
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