STARTING AMOUNT Question 24 of 24 A solution of phosphoric acid (HPO4) with a known concentration of 0.250 M H₂PO4 is titrated with a 0.800 M NaOH solution. How many mL of NaOH are required to reach the third equivalence point with a starting volume of 72.0 mL HsPO according to the following balanced chemical equation: H₂PO4+ 3 NaOH-NasPO4 + 3 H₂O ANSWER N 2 ADD FACTOR x() 7.50 22.5 mol H.PO. 72.0 1000 M NaOH 0.001 1 0.0675 M H.PO. 3 LH.PO. ml. NaOH g H.PO. 43.2 0.250 L NaOH g NaOH RESET 0.800 6.75 x 10 mL. H.PO. mol NaOH 67.5 Subm
STARTING AMOUNT Question 24 of 24 A solution of phosphoric acid (HPO4) with a known concentration of 0.250 M H₂PO4 is titrated with a 0.800 M NaOH solution. How many mL of NaOH are required to reach the third equivalence point with a starting volume of 72.0 mL HsPO according to the following balanced chemical equation: H₂PO4+ 3 NaOH-NasPO4 + 3 H₂O ANSWER N 2 ADD FACTOR x() 7.50 22.5 mol H.PO. 72.0 1000 M NaOH 0.001 1 0.0675 M H.PO. 3 LH.PO. ml. NaOH g H.PO. 43.2 0.250 L NaOH g NaOH RESET 0.800 6.75 x 10 mL. H.PO. mol NaOH 67.5 Subm
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 24 of 24**
**Problem Statement:**
A solution of phosphoric acid (H₃PO₄) with a known concentration of 0.250 M H₃PO₄ is titrated with a 0.800 M NaOH solution. How many mL of NaOH are required to reach the third equivalence point with a starting volume of 72.0 mL H₃PO₄ according to the following balanced chemical equation:
\[ \text{H}_3\text{PO}_4 + 3 \text{NaOH} \rightarrow \text{Na}_3\text{PO}_4 + 3 \text{H}_2\text{O} \]
**Interactive Components and Inputs:**
1. **Input Fields:** There are input fields for the starting amount, factor to convert from H₃PO₄ to NaOH, and the final answer.
2. **Solution Setup:**
- Starting Amount: The initial volume in milliliters of 72.0 mL H₃PO₄.
- Conversion Factors:
- M H₃PO₄ (concentration of phosphoric acid): 0.250 M.
- M NaOH (concentration of sodium hydroxide): 0.800 M.
- Stoichiometric coefficients from the balanced equation: 1 mol H₃PO₄ reacts with 3 mol NaOH.
- Other unit conversions: Necessary volume and molarity calculations.
**Graphical Calculations and Annotations:**
- **Starting Amount Input Box:** (Red Box)
- Value: 72.0 mL of H₃PO₄.
- **Conversion Factors and Units Rows:**
- Different amounts denoted by boxes and arrows showing conversion from volume to moles and then to volume of titrant.
- First Set: 72.0 mL H₃PO₄ x (1 L / 1000 mL) x (0.250 mol H₃PO₄ / 1 L) = 0.018 mol H₃PO₄.
- Second Set: 0.018 mol H₃PO₄ x (3 mol NaOH / 1 mol H₃PO₄) = 0.054 mol NaOH.
- Final Set: 0.054 mol NaOH](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1027c5e0-f235-434a-9c39-9791c1808f61%2F224bb6b6-9030-4f20-acd0-b9818c546cc2%2Fsew42p8_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Question 24 of 24**
**Problem Statement:**
A solution of phosphoric acid (H₃PO₄) with a known concentration of 0.250 M H₃PO₄ is titrated with a 0.800 M NaOH solution. How many mL of NaOH are required to reach the third equivalence point with a starting volume of 72.0 mL H₃PO₄ according to the following balanced chemical equation:
\[ \text{H}_3\text{PO}_4 + 3 \text{NaOH} \rightarrow \text{Na}_3\text{PO}_4 + 3 \text{H}_2\text{O} \]
**Interactive Components and Inputs:**
1. **Input Fields:** There are input fields for the starting amount, factor to convert from H₃PO₄ to NaOH, and the final answer.
2. **Solution Setup:**
- Starting Amount: The initial volume in milliliters of 72.0 mL H₃PO₄.
- Conversion Factors:
- M H₃PO₄ (concentration of phosphoric acid): 0.250 M.
- M NaOH (concentration of sodium hydroxide): 0.800 M.
- Stoichiometric coefficients from the balanced equation: 1 mol H₃PO₄ reacts with 3 mol NaOH.
- Other unit conversions: Necessary volume and molarity calculations.
**Graphical Calculations and Annotations:**
- **Starting Amount Input Box:** (Red Box)
- Value: 72.0 mL of H₃PO₄.
- **Conversion Factors and Units Rows:**
- Different amounts denoted by boxes and arrows showing conversion from volume to moles and then to volume of titrant.
- First Set: 72.0 mL H₃PO₄ x (1 L / 1000 mL) x (0.250 mol H₃PO₄ / 1 L) = 0.018 mol H₃PO₄.
- Second Set: 0.018 mol H₃PO₄ x (3 mol NaOH / 1 mol H₃PO₄) = 0.054 mol NaOH.
- Final Set: 0.054 mol NaOH
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