When 17.1ml of unknown molarity of potassium chloride solution is reacted in excess lead (11) nitrate solution, 6.53 g lead (II) chloride was produced ? Assuming 100% yield, what is the molarity of KCI? (some possibly useful molar masses: PbCl2= 278.1 g/mol; KCI= 74.55 g/mol; Pb(NO3)2 = 331.2 g/mol) 2 KCI(aq) + Pb(NO3)2 (aq) → PbCl2(s) + 2 KNO3(aq)
When 17.1ml of unknown molarity of potassium chloride solution is reacted in excess lead (11) nitrate solution, 6.53 g lead (II) chloride was produced ? Assuming 100% yield, what is the molarity of KCI? (some possibly useful molar masses: PbCl2= 278.1 g/mol; KCI= 74.55 g/mol; Pb(NO3)2 = 331.2 g/mol) 2 KCI(aq) + Pb(NO3)2 (aq) → PbCl2(s) + 2 KNO3(aq)
Chemistry
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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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![**Chemical Reaction Problem: Determining Molarity**
**Problem Statement:**
When 17.1 mL of an unknown molarity of potassium chloride (KCl) solution is reacted in excess lead (II) nitrate (Pb(NO₃)₂) solution, 6.53 g of lead (II) chloride (PbCl₂) was produced. Assuming 100% yield, what is the molarity of KCl?
**Molar Masses (possibly useful):**
- PbCl₂ = 278.1 g/mol
- KCl = 74.55 g/mol
- Pb(NO₃)₂ = 331.2 g/mol
**Chemical Equation:**
\[ 2 \text{KCl (aq)} + \text{Pb(NO}_3)_2 \text{ (aq)} \rightarrow \text{PbCl}_2 \text{ (s)} + 2 \text{KNO}_3 \text{ (aq)} \]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6501bcec-69f0-41c7-aaf6-9d4563ecc7cd%2F887104ac-06fa-4498-9635-d09c1292acfc%2F5n5zl2d_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Chemical Reaction Problem: Determining Molarity**
**Problem Statement:**
When 17.1 mL of an unknown molarity of potassium chloride (KCl) solution is reacted in excess lead (II) nitrate (Pb(NO₃)₂) solution, 6.53 g of lead (II) chloride (PbCl₂) was produced. Assuming 100% yield, what is the molarity of KCl?
**Molar Masses (possibly useful):**
- PbCl₂ = 278.1 g/mol
- KCl = 74.55 g/mol
- Pb(NO₃)₂ = 331.2 g/mol
**Chemical Equation:**
\[ 2 \text{KCl (aq)} + \text{Pb(NO}_3)_2 \text{ (aq)} \rightarrow \text{PbCl}_2 \text{ (s)} + 2 \text{KNO}_3 \text{ (aq)} \]
Expert Solution
Step 1
The balanced reaction taking place is given as,
Given : Volume of KCl solution used = 17.1 mL = 0.0171 L (since 1 L = 1000 mL)
And mass of PbCl2 produced = 6.53 g
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