/*! 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 102 The \(\mathrm{pH}\) of a \(0.064... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 15: Problem 102

The \(\mathrm{pH}\) of a \(0.0642 \mathrm{M}\) solution of a monoprotic acid is \(3.86 .\) Is this a strong acid?

Short Answer

Expert verified
No, the given acid is not a strong acid.

Step by step solution

01

Identify Known Variables

We know:1. The solution's \(\mathrm{pH}\) is \(3.86\).2. The molarity (\(\mathrm{M}\)) of the solution is \(0.0642 \mathrm{M}\).
02

Calculating the Concentration of Hydronium Ions

First, we calculate the concentration of hydronium ions, \([H^+]\). The pH of a solution is calculated using the negative logarithmic formula \(pH = -\log[H^+]\). Therefore, rearranging the formula to find \([H^+]\), we get \([H^+] = 10^{-pH} = 10^{-3.86}\).
03

Comparing the Concentration of Hydronium Ions with Initial Concentration of Acid

Next, we compare the \([H^+]\) concentration to the initial concentration of the acid. If the \([H^+]\) concentration is equal to the initial concentration of the acid, then the acid is strong because all of it has ionized. If the \([H^+]\) concentration is less than the initial concentration of the acid, the acid is weak because only part of it has ionized.
04

Draw Conclusion

In this case, after calculation we find that \([H^+]\) is significantly less than the initial concentration of the acid, indicating that the acid is weak, not strong.

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.

Monoprotic Acid
A monoprotic acid is a type of acid that can donate only one proton (hydrogen ion, H鈦�) per molecule in an aqueous solution. This characteristic distinguishes monoprotic acids from diprotic or triprotic acids, which can donate two or three protons, respectively. When a monoprotic acid dissolves in water, it releases one H鈦� ion into the solution.
  • The general formula for these acids is written as HA, where 'H' is the hydrogen that ionizes, and 'A' is the rest of the molecule. An example of a monoprotic acid is hydrochloric acid (HCl).
  • Monoprotic acids can be either strong or weak, depending on how completely they dissociate in water. Strong monoprotic acids dissociate completely, releasing all available hydrogen ions, whereas weak monoprotic acids do not.

This distinction becomes crucial when calculating pH or determining how much of the acid dissociates in a solution.
Strong Acid
A strong acid is an acid that completely ionizes or dissociates in a solution. This means that when a strong acid is dissolved in water, it releases all of its hydrogen ions into the solution.
  • This complete ionization leads to a higher concentration of hydronium ions (H鈧僌鈦�) because the acid molecules donate as many hydrogen ions as possible.
  • Strong acids are not only monoprotic; some, like sulfuric acid (H鈧係O鈧�), are diprotic (can release two protons), but they have the same principle of complete ionization for at least one of their protons.

For example, in the case of hydrochloric acid (HCl), a monoprotic strong acid, all HCl molecules ionize to form H鈦� and Cl鈦� ions. This property is why strong acids have low pH values close to or below 1 depending on their concentration.
Hydronium Ions Concentration
The concentration of hydronium ions (\[ [H鈧僌鈦篯 \] or simply \[ [H^+] \]) in a solution is crucial for determining the pH and the strength of an acid. In aqueous solutions, acidic properties arise due to the presence of these ions.
To determine the concentration of hydronium ions, we use the relationship:\[[H^+] = 10^{-pH}\]This expression tells us that the pH of a solution is inversely related to the concentration of hydronium ions: as the concentration increases, the pH decreases, leading to more acidic conditions.
  • A high concentration of \[ [H^+] \] indicates a stronger acidic environment.
  • Conversely, a low concentration would suggest a weaker acid if the pH is higher than expected for a given concentration of acid.

Understanding how to calculate and interpret \[ [H^+] \] is fundamental in acid-base chemistry, helping predict the behavior of acids in solutions.

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

Hemoglobin (Hb) is a blood protein that is responsible for transporting oxygen. It can exist in the protonated form as \(\mathrm{HbH}^{+}\). The binding of oxygen can be represented by the simplified equation $$ \mathrm{HbH}^{+}+\mathrm{O}_{2} \rightleftharpoons \mathrm{HbO}_{2}+\mathrm{H}^{+} $$ What form of hemoglobin is favored in the lungs where oxygen concentration is highest? (b) In body tissues, where the cells release carbon dioxide produced by metabolism, the blood is more acidic due to the formation of carbonic acid. What form of hemoglobin is favored under this condition? (c) When a person hyperventilates, the concentration of \(\mathrm{CO}_{2}\) in his or her blood decreases. How does this action affect the above equilibrium? Frequently a person who is hyperventilating is advised to breathe into a paper bag. Why does this action help the individual?

A typical reaction between an antacid and the hydrochloric acid in gastric juice is \(\mathrm{NaHCO}_{3}(s)+\mathrm{HCl}(a q) \rightleftharpoons\) $$ \mathrm{NaCl}(a q)+\mathrm{H}_{2} \mathrm{O}(l)+\mathrm{CO}_{2}(g) $$ Calculate the volume (in L) of \(\mathrm{CO}_{2}\) generated from \(0.350 \mathrm{~g}\) of \(\mathrm{NaHCO}_{3}\) and excess gastric juice at 1.00 atm and \(37.0^{\circ} \mathrm{C}\).

Calculate the \(\mathrm{pH}\) of a \(0.20 \mathrm{M} \mathrm{NaHCO}_{3}\) solution. (Hint: As an approximation, calculate hydrolysis and ionization separately first, followed by partial neutralization.)

Specify which of the following salts will undergo hydrolysis: \(\mathrm{KF}, \mathrm{NaNO}_{3}, \mathrm{NH}_{4} \mathrm{NO}_{2}, \mathrm{MgSO}_{4}, \mathrm{KCN}\) \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COONa}, \mathrm{RbI}, \mathrm{Na}_{2} \mathrm{CO}_{3}, \mathrm{CaCl}_{2}, \mathrm{HCOOK}\).

Calcium hypochlorite \(\left[\mathrm{Ca}(\mathrm{OCl})_{2}\right]\) is used as a disinfectant for swimming pools. When dissolved in water it produces hypochlorous acid: $$ \begin{aligned} \mathrm{Ca}(\mathrm{OCl})_{2}(s)+2 \mathrm{H}_{2} \mathrm{O}(l) & \rightleftharpoons \\ & 2 \mathrm{HClO}(a q)+\mathrm{Ca}(\mathrm{OH})_{2}(s) \end{aligned} $$ which ionizes as follows: \(\mathrm{HClO}(a q) \rightleftharpoons \mathrm{H}^{+}(a q)+\mathrm{ClO}^{-}(a q)\) $$ K_{\mathrm{a}}=3.0 \times 10^{-8} $$ As strong oxidizing agents, both \(\mathrm{HClO}\) and \(\mathrm{ClO}^{-}\) can kill bacteria by destroying their cellular components. However, too high a HClO concentration is irritating to the eyes of swimmers and too high a concentration of \(\mathrm{ClO}^{-}\) will cause the ions to decompose in sunlight. The recommended pH for pool water is \(7.8 .\) Calculate the percent of these species present at this pH.
See all solutions

Recommended explanations on Chemistry Textbooks

Ionic and Molecular Compounds

Read Explanation

Organic Chemistry

Read Explanation

Nuclear Chemistry

Read Explanation

Making Measurements

Read Explanation

Kinetics

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.