Table 1: Concentrations of [H3O*] and [OH-] when various amounts hydrochloric acid (HCl, strong acid) or hypochlorous acid (HOCI, weak acid) are dissolved in water to make 1.00 L of solution at 25 Moles of acid added 0.00 0.30 mol HC1 0.75 mol HC1 1.00 mol HCI 0.30 mol HOCI 0.75 mol HOCI 1.00 mol HOCI -1- [H30¹] (M) 1.0 x 10-7 0.30 0.75 1.00 9.3 x 10-5 1.5 x 10-4 1.7 x 10-4 [OH-] (M) 1.0 x 10-7 3.3 x 10-14 1.3 x 10-14 1.0 x 10-14 1.1 x 10-10 6.8 x 10-11 5.9 x 10-11 1. For the strong acid, HCl, in model 1, why are there no HCI molecules present in the beaker? 2. For the weak acid in model 1, why are there mostly HA molecules present in the beaker? 3. From Table 1, what happens to [H3O+] as the number of moles of HOCI increases? 4. From Table 1, how are each of the entries for [OH-] related to the corresponding entries for [H3O+]? 5. If you hadn't been told that HOCI is a weak acid, how could you deduce that from Table 1?
Table 1: Concentrations of [H3O*] and [OH-] when various amounts hydrochloric acid (HCl, strong acid) or hypochlorous acid (HOCI, weak acid) are dissolved in water to make 1.00 L of solution at 25 Moles of acid added 0.00 0.30 mol HC1 0.75 mol HC1 1.00 mol HCI 0.30 mol HOCI 0.75 mol HOCI 1.00 mol HOCI -1- [H30¹] (M) 1.0 x 10-7 0.30 0.75 1.00 9.3 x 10-5 1.5 x 10-4 1.7 x 10-4 [OH-] (M) 1.0 x 10-7 3.3 x 10-14 1.3 x 10-14 1.0 x 10-14 1.1 x 10-10 6.8 x 10-11 5.9 x 10-11 1. For the strong acid, HCl, in model 1, why are there no HCI molecules present in the beaker? 2. For the weak acid in model 1, why are there mostly HA molecules present in the beaker? 3. From Table 1, what happens to [H3O+] as the number of moles of HOCI increases? 4. From Table 1, how are each of the entries for [OH-] related to the corresponding entries for [H3O+]? 5. If you hadn't been told that HOCI is a weak acid, how could you deduce that from Table 1?
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
Related questions
Concept explainers
Ionic Equilibrium
Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
Arrhenius Acid
Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.
Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
Question
![Table 1: Concentrations of [H3O*] and [OH-] when various amounts hydrochloric acid (HCl, strong
acid) or hypochlorous acid (HOC1, weak acid) are dissolved in water to make 1.00 L of solution at 25
Moles of acid added
0.00
0.30 mol HCI
0.75 mol HCI
1.00 mol HCI
0.30 mol HOCI
0.75 mol HOCI
1.00 mol HOCI
- 1 -
[H3O+] (M)
1.0 x 10-7
0.30
0.75
1.00
9.3 x 10-5
1.5 x 10-4
1.7 x 10-4
[OH-] (M)
1.0 x 10-7
3.3 x 10-¹4
1.3 x 10-14
1.0 x 10-¹4
1.1 x 10-10
6.8 x 10-11
5.9 x 10-11
1. For the strong acid, HCl, in model 1, why are there no HCl molecules present in the beaker?
2. For the weak acid in model 1, why are there mostly HA molecules present in the beaker?
3. From Table 1, what happens to [H3O*] as the number of moles of HOCI increases?
4. From Table 1, how are each of the entries for [OH-] related to the corresponding entries for [H3O+]?
5. If you hadn't been told that HOCI is a weak acid, how could you deduce that from Table 1?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F39566a5b-b090-4ce8-ac49-27ee4e8311a1%2Fd90d6a2b-f118-4f7e-80be-449b913b3254%2Fqj6htk2_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Table 1: Concentrations of [H3O*] and [OH-] when various amounts hydrochloric acid (HCl, strong
acid) or hypochlorous acid (HOC1, weak acid) are dissolved in water to make 1.00 L of solution at 25
Moles of acid added
0.00
0.30 mol HCI
0.75 mol HCI
1.00 mol HCI
0.30 mol HOCI
0.75 mol HOCI
1.00 mol HOCI
- 1 -
[H3O+] (M)
1.0 x 10-7
0.30
0.75
1.00
9.3 x 10-5
1.5 x 10-4
1.7 x 10-4
[OH-] (M)
1.0 x 10-7
3.3 x 10-¹4
1.3 x 10-14
1.0 x 10-¹4
1.1 x 10-10
6.8 x 10-11
5.9 x 10-11
1. For the strong acid, HCl, in model 1, why are there no HCl molecules present in the beaker?
2. For the weak acid in model 1, why are there mostly HA molecules present in the beaker?
3. From Table 1, what happens to [H3O*] as the number of moles of HOCI increases?
4. From Table 1, how are each of the entries for [OH-] related to the corresponding entries for [H3O+]?
5. If you hadn't been told that HOCI is a weak acid, how could you deduce that from Table 1?
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 6 steps
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY