How many mL of 0.098 M HCl is required to completely react with 30.0 mL of 0.150 M K2CO3 solution according to the equation below? What is the molarity of KCl solution formed? 2HCl(aq) + K2CO3(aq) ⟶ 2KCl(aq) + H2O(l) + CO2(g)
How many mL of 0.098 M HCl is required to completely react with 30.0 mL of 0.150 M K2CO3 solution according to the equation below? What is the molarity of KCl solution formed? 2HCl(aq) + K2CO3(aq) ⟶ 2KCl(aq) + H2O(l) + CO2(g)
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter4: Chemical Reactions In Solution
Section: Chapter Questions
Problem 4.61QE
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- How many mL of 0.098 M HCl is required to completely react with 30.0 mL of 0.150 M K2CO3 solution according to the equation below? What is the molarity of KCl solution formed?
2HCl(aq) + K2CO3(aq) ⟶ 2KCl(aq) + H2O(l) + CO2(g)
Expert Solution
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Step 1
It is given that 30.0 mL of 0.150 M K2CO3 is reacting completely with 0.098 M of HCl and the reaction is shown below,
Step 2
To calculate the moles of K2CO3 present,
Step 3
To calculate the moles of HCl present with the help of the balanced equation,
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