What mass of Na2CO3, in grams, is required for complete reaction with 59.9 mL of 0.125 M HNO3 ? Na2CO3(aq) + 2 HNO3(aq) → 2 NaNO3(aq) + CO₂(g) + H₂O(l) g Na2CO3 Mass=
What mass of Na2CO3, in grams, is required for complete reaction with 59.9 mL of 0.125 M HNO3 ? Na2CO3(aq) + 2 HNO3(aq) → 2 NaNO3(aq) + CO₂(g) + H₂O(l) g Na2CO3 Mass=
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...
Related questions
Question
100%
![**Problem Statement:**
What mass of \( \text{Na}_2\text{CO}_3 \), in grams, is required for complete reaction with 59.9 mL of 0.125 M \( \text{HNO}_3 \)?
**Chemical Reaction:**
\[ \text{Na}_2\text{CO}_3(\text{aq}) + 2 \text{HNO}_3(\text{aq}) \rightarrow 2 \text{NaNO}_3(\text{aq}) + \text{CO}_2(\text{g}) + \text{H}_2\text{O}(\ell) \]
**Calculation:**
Mass \( = \underline{\hspace{2cm}} \text{g Na}_2\text{CO}_3 \)
---
**Explanation:**
To solve this problem, follow these steps:
1. **Calculate the moles of \( \text{HNO}_3 \) used:**
- Use the concentration (Molarity) and volume information provided.
\[
\text{Moles of } \text{HNO}_3 = \text{Molarity} \times \text{Volume (in liters)}
\]
2. **Determine the stoichiometric relationship:**
- Based on the balanced chemical equation, 1 mole of \( \text{Na}_2\text{CO}_3 \) reacts with 2 moles of \( \text{HNO}_3 \).
- Use the mole ratio to calculate the moles of \( \text{Na}_2\text{CO}_3 \) needed.
3. **Calculate the mass of \( \text{Na}_2\text{CO}_3 \):**
- Use the molar mass of \( \text{Na}_2\text{CO}_3 \) to convert moles to grams.
\[
\text{Mass of } \text{Na}_2\text{CO}_3 = \text{Moles of } \text{Na}_2\text{CO}_3 \times \text{Molar Mass of } \text{Na}_2\text{CO}_3
\]
Place the computed mass value in the provided space to complete the statement.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7a354f1c-cdfd-41e5-a863-9a86a504af1c%2Fc6af2232-c78e-41d8-aa0a-6b99c8d0f03a%2Fqfxhlse_processed.png&w=3840&q=75)
Transcribed Image Text:**Problem Statement:**
What mass of \( \text{Na}_2\text{CO}_3 \), in grams, is required for complete reaction with 59.9 mL of 0.125 M \( \text{HNO}_3 \)?
**Chemical Reaction:**
\[ \text{Na}_2\text{CO}_3(\text{aq}) + 2 \text{HNO}_3(\text{aq}) \rightarrow 2 \text{NaNO}_3(\text{aq}) + \text{CO}_2(\text{g}) + \text{H}_2\text{O}(\ell) \]
**Calculation:**
Mass \( = \underline{\hspace{2cm}} \text{g Na}_2\text{CO}_3 \)
---
**Explanation:**
To solve this problem, follow these steps:
1. **Calculate the moles of \( \text{HNO}_3 \) used:**
- Use the concentration (Molarity) and volume information provided.
\[
\text{Moles of } \text{HNO}_3 = \text{Molarity} \times \text{Volume (in liters)}
\]
2. **Determine the stoichiometric relationship:**
- Based on the balanced chemical equation, 1 mole of \( \text{Na}_2\text{CO}_3 \) reacts with 2 moles of \( \text{HNO}_3 \).
- Use the mole ratio to calculate the moles of \( \text{Na}_2\text{CO}_3 \) needed.
3. **Calculate the mass of \( \text{Na}_2\text{CO}_3 \):**
- Use the molar mass of \( \text{Na}_2\text{CO}_3 \) to convert moles to grams.
\[
\text{Mass of } \text{Na}_2\text{CO}_3 = \text{Moles of } \text{Na}_2\text{CO}_3 \times \text{Molar Mass of } \text{Na}_2\text{CO}_3
\]
Place the computed mass value in the provided space to complete the statement.
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
Step by step
Solved in 5 steps with 3 images
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY