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Chapter 15: Problem 32

Write an equation to describe the proton transfer that occurs when each of these acids is added to water. (a) \(\mathrm{HCO}_{3}^{-}\) (b) \(\mathrm{HCl}\) (c) \(\mathrm{CH}_{3} \mathrm{COOH}\) (d) \(\mathrm{HCN}\)

Short Answer

Expert verified
Proton transfer equations involve donating a proton to water, forming a conjugate base and hydronium ion.

Step by step solution

01

Identify the Proton Donor

Each of the given acids can donate a proton to water. Identify the proton that will be donated from each acid.
02

Write the Reaction for Each Acid

For each acid, illustrate a chemical equation showing the transfer of a proton to water, forming the corresponding conjugate base and hydronium ion, \( ext{H}_3 ext{O}^+\).
03

Equation for \(\mathrm{HCO}_3^-\)

The bicarbonate ion can donate a proton to water: \[\mathrm{HCO}_3^- + \mathrm{H}_2\mathrm{O} \rightarrow \mathrm{CO}_3^{2-} + \mathrm{H}_3\mathrm{O}^+\]
04

Equation for \(\mathrm{HCl}\)

Hydrochloric acid donates a proton to water: \[\mathrm{HCl} + \mathrm{H}_2\mathrm{O} \rightarrow \mathrm{Cl}^- + \mathrm{H}_3\mathrm{O}^+\]
05

Equation for \(\mathrm{CH}_3\mathrm{COOH}\)

Acetic acid donates a proton to water: \[\mathrm{CH}_3\mathrm{COOH} + \mathrm{H}_2\mathrm{O} \rightarrow \mathrm{CH}_3\mathrm{COO}^- + \mathrm{H}_3\mathrm{O}^+\]
06

Equation for \(\mathrm{HCN}\)

Hydrogen cyanide donates a proton to water: \[\mathrm{HCN} + \mathrm{H}_2\mathrm{O} \rightarrow \mathrm{CN}^- + \mathrm{H}_3\mathrm{O}^+\]

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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 a fundamental part of chemistry, often involved in various natural and industrial processes. When an acid is added to water, it typically undergoes a proton transfer reaction. In these reactions, the acid donates a proton, often described as a hydrogen ion ( ext{H}^+), to water. This transfer results in the formation of a new ion and the water molecule being transformed into a hydronium ion ( ext{H}_3 ext{O}^+).

In these reactions:
  • The acid is known as the proton donor.
  • The base, usually water, is known as the proton acceptor.
  • The product is a conjugate base, left after the acid loses its proton.
  • The resulting hydronium ion is a central marker of acidity.
Understanding acid-base reactions helps in predicting the behavior of substances in various chemical environments.
Conjugate Base
The term 'conjugate base' refers to what remains of an acid molecule after it donates a proton in an acid-base reaction. For example, when the bicarbonate ion ( ext{HCO}_3^-), hydrochloric acid ( ext{HCl}), acetic acid ( ext{CH}_3 ext{COOH}), and hydrogen cyanide ( ext{HCN}) donate protons to water, they form the following conjugate bases:
  • Bicarbonate becomes the carbonate ion ( ext{CO}_3^{2-}).
  • Hydrochloric acid becomes the chloride ion ( ext{Cl}^-).
  • Acetic acid becomes the acetate ion ( ext{CH}_3 ext{COO}^-).
  • Hydrogen cyanide becomes the cyanide ion ( ext{CN}^-).
Knowing how to identify the conjugate base in a reaction helps in balancing chemical equations, understanding reaction mechanisms, and recognizing patterns in chemical reactivity.
Hydronium Ion
The hydronium ion is a pivotal player in acid-base chemistry, formed when an acid donates a proton to water. It's denoted by the formula ext{H}_3 ext{O}^+. This ion represents the true nature of hydrogen ions in aqueous solutions.

Let's break down its formation:
  • Upon adding any acid to water, a proton from the acid combines with a water molecule.
  • This creates the hydronium ion, distinguishing acidic solutions by increasing the concentration of ext{H}_3 ext{O}^+ ions.
The presence of hydronium ions is crucial in determining the acidity or pH level of solutions, making it an essential concept in both laboratory and industrial chemistry settings.
Chemical Equations
Chemical equations are the language of chemistry, used to depict the interactions between different molecules in a reaction. For acid-base reactions, these equations show the transfer of ions, especially protons, in a clear and concise manner.

When writing chemical equations:
  • Identify the reactants and products in the reaction.
  • Include the proton donor (acid), proton acceptor (usually water), and the resultant ions, such as the conjugate base and hydronium ion.
  • Ensure the equation is balanced, meaning the number of atoms on each side remains equal.
For instance, in the equations provided for bicarbonate, hydrochloric acid, acetic acid, and hydrogen cyanide, we see a similar pattern:
  • Each acid reacts with ext{H}_2 ext{O}, producing a conjugate base and ext{H}_3 ext{O}^+.
By mastering how to write and interpret chemical equations, one can predict and understand the outcomes of chemical reactions efficiently.

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Most popular questions from this chapter

Like many narcotic drugs, cocaine is a weak base. Its chemical formula is \(\mathrm{C}_{17} \mathrm{H}_{21} \mathrm{NO}_{4} .\) Write the chemical equation for the ionization of this weak base in aqueous solution.

When \(1.00 \mathrm{~g}\) thiamine hydrochloride (also called vita\(\min \mathrm{B}_{1}\) hydrochloride) is dissolved in water and then diluted to exactly \(10.00 \mathrm{~mL},\) the \(\mathrm{pH}\) of the resulting solution is \(4.50 .\) The formula weight of thiamine hydrochloride is \(337.28 .\) Calculate \(K_{\mathrm{a}}\) and \(\mathrm{p} K_{\mathrm{a}}\) for this acid.

Choose from among the labels strongly acidic, weakly acidic, neutral, weakly basic, and strongly basic to estimate the \(\mathrm{pH}\) of the following solutions. (a) \(0.30 \mathrm{M} \mathrm{NH}_{4} \mathrm{Cl}\) (b) \(0.15 \mathrm{M} \mathrm{N}_{2} \mathrm{H}_{5} \mathrm{Cl}\) (c) \(0.50 \mathrm{M} \mathrm{KNO}_{3}\) (d) \(0.50 \mathrm{M} \mathrm{HCOONa}\)

Consider sodium acrylate, \(\mathrm{NaC}_{3} \mathrm{H}_{3} \mathrm{O}_{2} . K_{\mathrm{a}}\) for acrylic acid (its conjugate acid) is \(5.5 \times 10^{-5}\). (a) Write a balanced net ionic equation for the reaction that makes aqueous solutions of sodium acrylate basic. (b) Calculate \(K_{\mathrm{b}}\) for the reaction in (a). (c) Find the \(\mathrm{pH}\) of a solution prepared by dissolving \(1.61 \mathrm{~g} \mathrm{NaC}_{3} \mathrm{H}_{3} \mathrm{O}_{2}\) in enough water to make \(835 \mathrm{~mL}\) of solution.

Calculate the \(\mathrm{pH}\) and \(\mathrm{pOH}\) of the following solutions. (a) \(0.050 M \mathrm{HCl}\) (b) \(0.024 \mathrm{M} \mathrm{KOH}\) (c) \(0.014 \mathrm{M} \mathrm{HClO}_{4}\) (d) \(1.05 \mathrm{M} \mathrm{NaOH}\)
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