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what volume in l of 1.6 m na3po4 would be required to obtain 0.60 moles of na+ ions?

what volume in l of 1.6 m na3po4 would be required to obtain 0.60 moles of na+ ions?

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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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.
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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