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Chapter 6: Problem 33

Identify the Br酶nsted-Lowry acids among the reactants in the following reactions: (a) \(\mathrm{KCN}+\mathrm{HI} \rightleftharpoons \mathrm{HCN}+\mathrm{KI}\) (b) \(\mathrm{PO}_{4}^{3-}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{HPO}_{4}^{2-}+\mathrm{OH}^{-}\)

Short Answer

Expert verified
(a) HI; (b) H鈧侽.

Step by step solution

01

Understanding Br酶nsted-Lowry Acids

A Br酶nsted-Lowry acid is a substance that can donate a proton (H鈦� ion) to another substance. To identify the acids, look for reactants that lose a proton in the reaction.
02

Analyzing Reaction (a)

In the reaction \(\mathrm{KCN} + \mathrm{HI} \rightleftharpoons \mathrm{HCN} + \mathrm{KI}\), we identify \(\mathrm{HI}\) as the reactant that donates a proton to form \(\mathrm{HCN}\). Thus, \(\mathrm{HI}\) is the Br酶nsted-Lowry acid in this reaction.
03

Analyzing Reaction (b)

For the reaction \(\mathrm{PO}_{4}^{3-} + \mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{HPO}_{4}^{2-} + \mathrm{OH}^{-}\), \(\mathrm{H}_{2} \mathrm{O}\) donates a proton to \(\mathrm{PO}_{4}^{3-}\) to form \(\mathrm{HPO}_{4}^{2-}\). Thus, \(\mathrm{H}_{2} \mathrm{O}\) is the Br酶nsted-Lowry acid in this reaction.

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Key Concepts

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

Understanding Proton Donors
In the world of chemistry, a proton donor is a crucial concept, especially in the realm of acid-base reactions. Simply put, a proton donor is a substance that gives away a proton, which is represented as an \( \text{H}^+ \) ion, during a chemical reaction. This process is essential for identifying Br酶nsted-Lowry acids, as these are the substances that act as proton donors in reactions.
  • To identify a proton donor in any reaction, look for the molecule or ion that loses an \( \text{H}^+ \) ion.
  • The substance that receives this \( \text{H}^+ \) ion is known as the Br酶nsted-Lowry base.
  • This transfer of a proton is what characterizes the interaction between an acid and a base in Br酶nsted-Lowry theory.
Without these proton transfer processes, many fundamental chemical reactions would not occur, making proton donors vital to numerous scientific and practical applications.
Essentials of Chemical Reactions
Chemical reactions are processes where substances, called reactants, are transformed into different substances, known as products. These reactions are driven by the breaking and forming of chemical bonds, leading to changes in the chemical composition of the involved substances.In the context of acid-base reactions, particularly under the Br酶nsted-Lowry theory, chemical reactions involve the transfer of protons (\( \text{H}^+ \) ions).
  • A notable aspect of these reactions is the equilibrium state, where both reactants and products coexist, typically denoted by the double arrow \( \rightleftharpoons \).
  • The direction of the reaction can shift based on various factors such as concentration, pressure, and temperature.
  • An example includes the reactions provided: \( \text{KCN} + \text{HI} \rightleftharpoons \text{HCN} + \text{KI} \) and \( \text{PO}_4^{3-} + \text{H}_2 \text{O} \rightleftharpoons \text{HPO}_4^{2-} + \text{OH}^- \).
Through understanding chemical reactions, one can predict and explain the outcomes of mixing different substances, which is foundational knowledge in chemistry.
Insights into Acid-Base Theory
Acid-base theory has evolved over time, with various definitions helping chemists to classify and understand these substances. The Br酶nsted-Lowry acid-base theory is one of the most widely accepted frameworks. It defines acids and bases based on their ability to donate or accept protons.
  • A Br酶nsted-Lowry acid is a proton donor, as seen with \( \text{HI} \) donating a proton to form \( \text{HCN} \).
  • A Br酶nsted-Lowry base, on the other hand, accepts a proton, as depicted by \( \text{PO}_4^{3-} \) accepting a proton to become \( \text{HPO}_4^{2-} \).
  • One important aspect of this theory is that water, \( \text{H}_2\text{O} \), can act as both an acid and a base, depending on the reaction context, exemplifying its amphoteric nature.
The simplification of acids and bases to their capacitiy to donate or accept protons makes the Br酶nsted-Lowry theory instrumental in understanding a diverse range of chemical reactions.

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Most popular questions from this chapter

Write the \(K_{\mathrm{a} 2}\) reaction of phosphoric acid \(\left(\mathrm{H}_{3} \mathrm{PO}_{4}\right)\) and the \(K_{\mathrm{b} 2}\) reaction of disodium oxalate \(\left(\mathrm{Na}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\right)\).

For the reaction \(\mathrm{HCO}_{3}^{-} \rightleftharpoons \mathrm{H}^{+}+\mathrm{CO}_{3}^{2-}, \Delta G^{\circ}=+59.0 \mathrm{~kJ} / \mathrm{mol}\) at \(298.15 \mathrm{~K}\). Find the value of \(K\) for the reaction.

Fill in the blanks: (a) The product of a reaction between a Lewis acid and a Lewis base is called (b) The bond between a Lewis acid and a Lewis base is called or (c) Br酶nsted-Lowry acids and bases related by gain or loss of one proton are said to be (d) A solution is acidic if . A solution is basic if

Write the \(K_{\mathrm{a}}\) and \(K_{\mathrm{b}}\) reactions of \(\mathrm{NaHCO}_{3}\).

Write the autoprotolysis reaction of \(\mathrm{H}_{2} \mathrm{SO}_{4}\).
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