How many moles of precipitate are formed when 45.0 mL of 0.450 M CaCl, is mixed with excess K,PO, in the following chemical reaction? 3 СаaCl,(aq) + 2 К,РО.(аq) > Ca:(РО:):(s) + 6 KC(ag)
How many moles of precipitate are formed when 45.0 mL of 0.450 M CaCl, is mixed with excess K,PO, in the following chemical reaction? 3 СаaCl,(aq) + 2 К,РО.(аq) > Ca:(РО:):(s) + 6 KC(ag)
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 7 of 7**
**Chemistry Problem: Stoichiometry and Precipitation Reaction**
**Problem Statement:**
How many moles of precipitate are formed when 45.0 mL of 0.450 M CaCl₂ is mixed with excess K₃PO₄ in the following chemical reaction?
\[ 3 \, \text{CaCl}_2(\text{aq}) + 2 \, \text{K}_3\text{PO}_4(\text{aq}) \rightarrow \text{Ca}_3(\text{PO}_4)_2(\text{s}) + 6 \, \text{KCl}(\text{aq}) \]
**Calculation Input:**
- Volume of CaCl₂ solution = 45.0 mL
- Concentration of CaCl₂ = 0.450 M
- K₃PO₄ is in excess
Below the problem, there is an interactive numeric keypad allowing the input of the calculated moles of Ca₃(PO₄)₂ formed.
**Notes:**
- The reaction involves mixing calcium chloride with potassium phosphate.
- The product of interest is the precipitate calcium phosphate, Ca₃(PO₄)₂.
**Interactive Features:**
- Numeric keypad with digits 0-9, a decimal point, plus/minus sign, and scientific notation (x10) input.
- Clear (C) and backspace (delete/back) buttons for editing the input.
Additional resources can be accessed for more help.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1bafcbb5-b29e-4e04-bd82-dcaa326e84c5%2Ffffb8724-b9be-41f2-a7bc-80c90d495f91%2Fechp4vr_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Question 7 of 7**
**Chemistry Problem: Stoichiometry and Precipitation Reaction**
**Problem Statement:**
How many moles of precipitate are formed when 45.0 mL of 0.450 M CaCl₂ is mixed with excess K₃PO₄ in the following chemical reaction?
\[ 3 \, \text{CaCl}_2(\text{aq}) + 2 \, \text{K}_3\text{PO}_4(\text{aq}) \rightarrow \text{Ca}_3(\text{PO}_4)_2(\text{s}) + 6 \, \text{KCl}(\text{aq}) \]
**Calculation Input:**
- Volume of CaCl₂ solution = 45.0 mL
- Concentration of CaCl₂ = 0.450 M
- K₃PO₄ is in excess
Below the problem, there is an interactive numeric keypad allowing the input of the calculated moles of Ca₃(PO₄)₂ formed.
**Notes:**
- The reaction involves mixing calcium chloride with potassium phosphate.
- The product of interest is the precipitate calcium phosphate, Ca₃(PO₄)₂.
**Interactive Features:**
- Numeric keypad with digits 0-9, a decimal point, plus/minus sign, and scientific notation (x10) input.
- Clear (C) and backspace (delete/back) buttons for editing the input.
Additional resources can be accessed for more help.
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