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How many moles of magnesium ions are present in 187 ml of 0.145 M magnesium iodate?

How many moles of magnesium ions are present in 187 ml of 0.145 M magnesium iodate?

Chemistry
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.
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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