/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 93 What happens to the \(\mathrm{pH... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 10: Problem 93

What happens to the \(\mathrm{pH}\) of a \(1-M\) solution of hydrochloric acid. HCl, as carbon dioxide gas is bubbled into it?

Short Answer

Expert verified
Bubbling CO鈧� does not significantly change the already low pH of the HCl solution.

Step by step solution

01

Understand the Situation

We have a 1-M solution of hydrochloric acid (HCl) and we are bubbling carbon dioxide (CO鈧�) into it. Both HCl and CO鈧� will affect the pH of the solution. HCl is a strong acid and fully dissociates in water, while CO鈧� forms carbonic acid (H鈧侰O鈧�) in water.
02

Role of HCl in Solution

Since HCl is a strong acid, it dissociates completely in the solution: \( \text{HCl} \rightarrow \text{H}^+ + \text{Cl}^- \). It provides a high concentration of hydrogen ions (\( \text{H}^+ \)), which lowers the pH significantly, making the solution very acidic.
03

Reaction of CO鈧� with Water

When CO鈧� is bubbled into water, it reacts to form carbonic acid: \(\text{CO}_2 + \text{H}_2\text{O} \rightleftharpoons \text{H}_2\text{CO}_3\). Carbonic acid can is a weak acid and can further dissociate into hydrogen ions (\( \text{H}^+ \)) and bicarbonate ions (\( \text{HCO}_3^-\)): \( \text{H}_2\text{CO}_3 \rightleftharpoons \text{H}^+ + \text{HCO}_3^- \).
04

Calculate Effects on pH

The major source of \( \text{H}^+ \) ions in this solution is from the dissociation of HCl. Since the contribution of hydrogen ions from carbonic acid addition is minor in comparison, the overall pH is primarily determined by the strong acid (HCl). The CO鈧� addition has a negligible effect on the already low pH.
05

Conclusion

As CO鈧�, a weak acid, is introduced to the strong acidic solution, the small amount of additional \( \text{H}^+ \) ions from carbonic acid formation does not significantly change the overall very low pH caused by the 1-M HCl. The solution remains strongly acidic.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with 91影视!

Key Concepts

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

Hydrochloric Acid
Hydrochloric acid (HCl) is a highly corrosive, strong acid that is widely used in laboratories and industries. When it is dissolved in water, it dissociates completely into hydrogen ions (\(\text{H}^+\)) and chloride ions (\(\text{Cl}^-\)). This dissociation process is what defines HCl as a strong acid.
  • HCl provides a high concentration of hydrogen ions.
  • This results in a significantly lowered pH, making the solution very acidic.
  • The complete dissociation of HCl is represented by the chemical equation: \(\text{HCl} \rightarrow \text{H}^+ + \text{Cl}^-\).
Understanding the nature of strong acids like HCl is crucial because their strong acidic properties have profound effects on the pH of solutions. Hence, even when other components are added to the solution, such as gases or weak acids, their influence on pH remains minimal due to the overwhelming acidic strength of HCl.
Carbon Dioxide
Carbon dioxide (CO鈧�) is a colorless, odorless gas found naturally in the Earth's atmosphere. It plays a significant role in atmospheric and biological processes, such as respiration and combustion. In chemical reactions involving solutions, CO鈧� can interact with water to form carbonic acid.
This reaction is reversible and shown by the equation:
  • \(\text{CO}_2 + \text{H}_{2}\text{O} \rightleftharpoons \text{H}_2\text{CO}_3\).
However, it is important to note:
  • CO鈧� on its own isn't very soluble in water.
  • In solutions with strong acids like HCl, the formation of carbonic acid is relatively minor compared to the dissociation of HCl.
Thus, when CO鈧� is introduced to a solution already containing a strong acid like HCl, its effect on pH is usually minimal.
Carbonic Acid
Carbonic acid (H鈧侰O鈧�) forms when carbon dioxide dissolves in water. Being a weak acid, it partially dissociates in water to produce bicarbonate (HCO鈧冣伝) and hydrogen ions (\(\text{H}^+\)).The dissociation process is represented as:
  • \(\text{H}_2\text{CO}_3 \rightleftharpoons \text{H}^+ + \text{HCO}_3^-\).
Since carbonic acid is much weaker than hydrochloric acid, the addition of CO鈧� and subsequent formation of H鈧侰O鈧� in a solution already containing HCl has little effect on the solution's pH.
Some important points to consider include:
  • The weak dissociation of carbonic acid means it only releases a small amount of hydrogen ions compared to the strong dissociation of HCl.
  • In a very acidic solution, the pH remains predominantly controlled by the strong acid present, regardless of the presence of weak acids like carbonic acid.

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Which should be a stronger base: ammonia, \(\mathrm{NH}_{3}\), or trifluoronitrogen, \(\mathrm{NF}_{3}\) ?

In Pour vinegar onto beach sand from the Carribean and the result is a lot of froth and bubbles. Pour vinegar onto beach sand from California, however, and nothing happens. Why?

A weak acid is added to a concentrated solution of hydrochloric acid. Does the solution become more or less acidic?

Identify the acid or base behavior of each substance in these reactions: a. \(\mathrm{HSO}_{4}^{-}+\mathrm{H}_{2} \mathrm{O} \leftrightarrows \mathrm{OH}^{-}+\mathrm{H}_{2} \mathrm{SO}_{4}\) b. \(\overline{\mathrm{O}^{2-}}+\mathrm{H}_{2} \mathrm{O} \leftrightarrows \mathrm{OH}^{-}+\mathrm{OH}^{-}\)

Why aren't atmospheric levels of carbon dioxide rising as rapidly as might be expected based on the increased output of carbon dioxide resulting from human activities?
See all solutions

Recommended explanations on Chemistry Textbooks

Chemistry Branches

Read Explanation

Chemical Reactions

Read Explanation

Kinetics

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Chemical Analysis

Read Explanation

Inorganic Chemistry

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.