O Calculate the number of milliliters of 0.686 M Ba(OH)2 required to precipitate all of the Cu²+ ions in 171 mL of 0.502 M Cul2 solution as Cu(OH)2. The equation for the reaction is: Cul₂ (aq) + Ba(OH)2 (aq) → Cu(OH)2 (s) + Bal₂ (aq) Volume = mL
O Calculate the number of milliliters of 0.686 M Ba(OH)2 required to precipitate all of the Cu²+ ions in 171 mL of 0.502 M Cul2 solution as Cu(OH)2. The equation for the reaction is: Cul₂ (aq) + Ba(OH)2 (aq) → Cu(OH)2 (s) + Bal₂ (aq) Volume = mL
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
Please answer both questions
![**Precipitation Reaction Calculation**
Calculate the number of milliliters of 0.686 M Ba(OH)₂ required to precipitate all of the Cu²⁺ ions in 171 mL of 0.502 M CuI₂ solution as Cu(OH)₂.
The equation for the reaction is:
\[ \text{CuI}_2(aq) + \text{Ba(OH)}_2(aq) \rightarrow \text{Cu(OH)}_2(s) + \text{BaI}_2(aq) \]
**Volume = [ ] mL**
In this experiment, you are tasked with determining the volume of barium hydroxide solution needed to completely precipitate copper ions from a copper(I) iodide solution, converting them into copper(II) hydroxide, a solid. Use the balanced chemical equation to understand the stoichiometry of the reaction, ensuring proper calculation of milliliters needed.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4295bf62-da14-49f1-b3bf-6e678bc68de3%2F0c533a7c-efd0-4f3c-ab7f-b779a2d6f6ff%2Fa4a4j8r_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Precipitation Reaction Calculation**
Calculate the number of milliliters of 0.686 M Ba(OH)₂ required to precipitate all of the Cu²⁺ ions in 171 mL of 0.502 M CuI₂ solution as Cu(OH)₂.
The equation for the reaction is:
\[ \text{CuI}_2(aq) + \text{Ba(OH)}_2(aq) \rightarrow \text{Cu(OH)}_2(s) + \text{BaI}_2(aq) \]
**Volume = [ ] mL**
In this experiment, you are tasked with determining the volume of barium hydroxide solution needed to completely precipitate copper ions from a copper(I) iodide solution, converting them into copper(II) hydroxide, a solid. Use the balanced chemical equation to understand the stoichiometry of the reaction, ensuring proper calculation of milliliters needed.
![**Problem Statement:**
Calculate the volume (in mL) of a 0.773 M HNO₃ solution required to completely dissolve 8.42 g of MgCO₃.
**Chemical Reaction:**
\[ 2\text{HNO}_3(aq) + \text{MgCO}_3(s) \rightarrow \text{Mg(NO}_3\text{)}_2(aq) + \text{H}_2\text{O}(l) + \text{CO}_2(g) \]
**Solution Blank:**
\[ \boxed{\phantom{0000}} \text{ mL} \]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4295bf62-da14-49f1-b3bf-6e678bc68de3%2F0c533a7c-efd0-4f3c-ab7f-b779a2d6f6ff%2Fis6sne8_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Problem Statement:**
Calculate the volume (in mL) of a 0.773 M HNO₃ solution required to completely dissolve 8.42 g of MgCO₃.
**Chemical Reaction:**
\[ 2\text{HNO}_3(aq) + \text{MgCO}_3(s) \rightarrow \text{Mg(NO}_3\text{)}_2(aq) + \text{H}_2\text{O}(l) + \text{CO}_2(g) \]
**Solution Blank:**
\[ \boxed{\phantom{0000}} \text{ mL} \]
Expert Solution
Step 1
a) given,
CuI2(aq) + Ba(OH)2 -----> Cu(OH)2(s) + BaI2(aq)
For Ba(OH)2 solution:
Concentration of Ba(OH)2 solution = 0.686 M = 0.686 mol/L
Volume of Ba(OH)2 solution = ?
For CuI2 solution:
Concentration of CuI2 solution = 0.502 M = 0.502 mol/L
Volume of CuI2 solution = 171 mL = 0.171 L
Step by step
Solved in 5 steps
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