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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Question
what volume in l of 1.6 m na3po4 would be required to obtain 0.60 moles of na+ ions?
![**Question 5 of 13**
What volume (in L) of 1.6 M Na₃PO₄ would be required to obtain 0.60 moles of Na⁺ ions?
**Answer:**
0.40 L
----
This interactive question displays an input field where students can enter their answer in liters along with a virtual number pad to facilitate this input.
**Explanation:**
Each molecule of Na₃PO₄ contains three Na⁺ ions. To find the volume of the solution needed:
1. **Determine the moles of Na₃PO₄ needed:**
Since each mole of Na₃PO₄ provides 3 moles of Na⁺, you need \(\frac{0.60 \text{ moles Na}^+}{3} = 0.20 \text{ moles of Na}_3\text{PO}_4\).
2. **Calculate the volume:**
Use the formula \( \text{Volume} = \frac{\text{Moles of solute}}{\text{Molarity}} \)
Substitute \( \text{Molarity} = 1.6 \text{ M} \) and \(\text{Moles} = 0.20\):
\[
\text{Volume} = \frac{0.20}{1.6} = 0.125 \text{ L}
\]
The answer shown as 0.40 L allows students to reconsider the computations, as it appears the final calculation in the image might not align with this step-by-step approach in the explanation section.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff5fef3a0-e6fd-445e-9e70-c8351f019035%2F74aaca61-158a-42d1-9f73-79ec2c7719d5%2Fyxlzex_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Question 5 of 13**
What volume (in L) of 1.6 M Na₃PO₄ would be required to obtain 0.60 moles of Na⁺ ions?
**Answer:**
0.40 L
----
This interactive question displays an input field where students can enter their answer in liters along with a virtual number pad to facilitate this input.
**Explanation:**
Each molecule of Na₃PO₄ contains three Na⁺ ions. To find the volume of the solution needed:
1. **Determine the moles of Na₃PO₄ needed:**
Since each mole of Na₃PO₄ provides 3 moles of Na⁺, you need \(\frac{0.60 \text{ moles Na}^+}{3} = 0.20 \text{ moles of Na}_3\text{PO}_4\).
2. **Calculate the volume:**
Use the formula \( \text{Volume} = \frac{\text{Moles of solute}}{\text{Molarity}} \)
Substitute \( \text{Molarity} = 1.6 \text{ M} \) and \(\text{Moles} = 0.20\):
\[
\text{Volume} = \frac{0.20}{1.6} = 0.125 \text{ L}
\]
The answer shown as 0.40 L allows students to reconsider the computations, as it appears the final calculation in the image might not align with this step-by-step approach in the explanation section.
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