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...
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![### Calculation of Magnesium Ions
**Question:**
How many moles of magnesium ions are present in 187 ml of 0.145 M magnesium iodate?
**Details:**
To find the number of moles of magnesium ions in the given solution, we follow these steps:
1. **Determine the Volume in Liters:**
- Given: 187 ml of solution
- Convert ml to liters:
- \( 187 \, \text{ml} = 0.187 \, \text{L} \)
2. **Use the Molarity to Find the Moles:**
- Molarity (M) is defined as moles of solute per liter of solution.
- Given: The solution has a molarity of \( 0.145 \, \text{M} \) (which means 0.145 moles of solute per liter).
- Calculate the moles of magnesium iodate using the formula:
- \( \text{Moles} = \text{Molarity} \times \text{Volume\,(L)} \)
- \( \text{Moles} = 0.145 \, \text{M} \times 0.187 \, \text{L} \)
- \( \text{Moles} = 0.027115 \)
Thus, **0.027115 moles** of magnesium ions are present in 187 ml of a 0.145 M magnesium iodate solution.
**Note:**
The solution contains a textbox prompt for the answer. Students would typically enter the calculated moles in this box as part of an online educational exercise.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F19b0aed3-745e-4879-8577-ea35399669d0%2F6259b38e-9080-4cde-b157-28b85768d23c%2F2srvuff_processed.png&w=3840&q=75)
Transcribed Image Text:### Calculation of Magnesium Ions
**Question:**
How many moles of magnesium ions are present in 187 ml of 0.145 M magnesium iodate?
**Details:**
To find the number of moles of magnesium ions in the given solution, we follow these steps:
1. **Determine the Volume in Liters:**
- Given: 187 ml of solution
- Convert ml to liters:
- \( 187 \, \text{ml} = 0.187 \, \text{L} \)
2. **Use the Molarity to Find the Moles:**
- Molarity (M) is defined as moles of solute per liter of solution.
- Given: The solution has a molarity of \( 0.145 \, \text{M} \) (which means 0.145 moles of solute per liter).
- Calculate the moles of magnesium iodate using the formula:
- \( \text{Moles} = \text{Molarity} \times \text{Volume\,(L)} \)
- \( \text{Moles} = 0.145 \, \text{M} \times 0.187 \, \text{L} \)
- \( \text{Moles} = 0.027115 \)
Thus, **0.027115 moles** of magnesium ions are present in 187 ml of a 0.145 M magnesium iodate solution.
**Note:**
The solution contains a textbox prompt for the answer. Students would typically enter the calculated moles in this box as part of an online educational exercise.
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