How many moles and numbers of ions of each type are present in the following aqueous solution? 51.7 mL of 1.35 M magnesium chloride: x 10 mol of magnesium x 10 magnesium ions x 10 mol of chloride x 10 chloride ions
How many moles and numbers of ions of each type are present in the following aqueous solution? 51.7 mL of 1.35 M magnesium chloride: x 10 mol of magnesium x 10 magnesium ions x 10 mol of chloride x 10 chloride ions
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
Question
How many moles and numbers of ions of each type are present in the following aqueous solution? 51.7 mL of 1.35 M magnesium chloride:
mol of magnesium
magnesium ions
mol of chloride
chloride ions
![**Educational Content: Calculating Moles and Ion Numbers in a Magnesium Chloride Solution**
---
**Problem Statement:**
How many moles and numbers of ions of each type are present in the following aqueous solution?
51.7 mL of 1.35 M magnesium chloride:
1. \(\_\_\_\_\_\) × 10\(^x\) mol of magnesium
2. \(\_\_\_\_\_\) × 10\(^x\) magnesium ions
3. \(\_\_\_\_\_\) × 10\(^x\) mol of chloride
4. \(\_\_\_\_\_\) × 10\(^x\) chloride ions
---
**Explanation:**
This exercise involves the calculation of the amount of substance in terms of moles and the corresponding number of ions in a given volume of magnesium chloride solution.
- **Magnesium Chloride (MgCl\(_2\))** dissociates completely in solution to produce one magnesium ion (Mg\(^{2+}\)) and two chloride ions (Cl\(^-\)) for each formula unit dissolved.
- The provided molarity (1.35 M) represents the concentration in moles per liter. To calculate the moles present in 51.7 mL, convert the volume to liters and use the formula:
\[
\text{Moles} = \text{Molarity} \times \text{Volume in liters}
\]
- Calculate the number of ions by considering Avogadro's number (6.022 × 10\(^{23}\) ions/mole) for each type of ion produced from the dissociation of magnesium chloride.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fab95b8cd-e92c-4a9e-9ebe-46ce73f4a65e%2Fbab5554d-6e98-41f6-8352-3a7ec68b88b0%2Fem13dm4_processed.png&w=3840&q=75)
Transcribed Image Text:**Educational Content: Calculating Moles and Ion Numbers in a Magnesium Chloride Solution**
---
**Problem Statement:**
How many moles and numbers of ions of each type are present in the following aqueous solution?
51.7 mL of 1.35 M magnesium chloride:
1. \(\_\_\_\_\_\) × 10\(^x\) mol of magnesium
2. \(\_\_\_\_\_\) × 10\(^x\) magnesium ions
3. \(\_\_\_\_\_\) × 10\(^x\) mol of chloride
4. \(\_\_\_\_\_\) × 10\(^x\) chloride ions
---
**Explanation:**
This exercise involves the calculation of the amount of substance in terms of moles and the corresponding number of ions in a given volume of magnesium chloride solution.
- **Magnesium Chloride (MgCl\(_2\))** dissociates completely in solution to produce one magnesium ion (Mg\(^{2+}\)) and two chloride ions (Cl\(^-\)) for each formula unit dissolved.
- The provided molarity (1.35 M) represents the concentration in moles per liter. To calculate the moles present in 51.7 mL, convert the volume to liters and use the formula:
\[
\text{Moles} = \text{Molarity} \times \text{Volume in liters}
\]
- Calculate the number of ions by considering Avogadro's number (6.022 × 10\(^{23}\) ions/mole) for each type of ion produced from the dissociation of magnesium chloride.
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 2 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