A 5.850-g sample containing KCl and KClO4 was dissolved in sufficient water to give 250.00 mL of solution. A 50.00-mL portion of the solution required 43.94 mL of 0.0750 M AgNO3 in a Mohr titration. Next, a 25.00-mL portion of the original solution was treated with V₂(SO4)3 to reduce the perchlorate ion to chloride, 8 V³+ (aq) + C1O4 (aq) + 12 H₂O(l) → Cl(aq) +8 VO²+ (aq) + 8 H3O+ (aq) and the resulting solution was titrated with AgNO3. This titration required 38.06 mL of 0.0750 M AgNO3. What is the mass percent of KCl and KC1O4 in the mixture? % KCI % KC1O4
Ionic Equilibrium
Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
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Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.
Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
![### Determining the Mass Percent of KCl and KClO₄ in a Mixture
A 5.850-g sample containing KCl and KClO₄ was dissolved in sufficient water to give 250.00 mL of solution. A 50.00-mL portion of the solution required 43.94 mL of 0.0750 M AgNO₃ in a Mohr titration.
Next, a 25.00-mL portion of the original solution was treated with V₂(SO₄)₃ to reduce the perchlorate ion to chloride. The reaction is as follows:
\[ 8 \, V^{3+} \,(aq) + \, ClO₄^- \, (aq) + \, 12 \, H_2O \, (l) \rightarrow Cl^- \, (aq) + \, 8 \, VO^{2+} \, (aq) + \, 8 \, H_3O^{+} \, (aq) \]
The resulting solution was titrated with AgNO₃. This titration required 38.06 mL of 0.0750 M AgNO₃.
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### Questions:
1. What is the mass percent of KCl in the mixture?
2. What is the mass percent of KClO₄ in the mixture?
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\[ \boxed{ \% \, \text{KCl} } \]
\[ \boxed{ \% \, \text{KClO₄} } \]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F883e3e80-624e-4e0d-88a1-3570ac65b326%2F143940bd-18c4-4edb-b9df-b0f1a061aa94%2Fbc96st4_processed.png&w=3840&q=75)
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