**Solubility and Qualitative Analysis: Laboratory Simulation****Problem:**You are given an unknown solution containing both aqueous barium ions, \( \text{Ba}^{2+}(\text{aq}) \), and aqueous lead(II) ions, \( \text{Pb}^{2+}(\text{aq}) \). Which of your six solutions would allow separation of the ions?**Select all that apply:**- A. Ammonium chloride, \( \text{NH}_4\text{Cl}(\text{aq}) \)- B. Nickel(II) nitrate, \( \text{Ni}(\text{NO}_3)_2(\text{aq}) \)- C. Potassium chloride, \( \text{KCl}(\text{aq}) \)- D. Silver nitrate, \( \text{AgNO}_3(\text{aq}) \)- E. Sodium hydroxide, \( \text{NaOH}(\text{aq}) \)- F. Sulfuric acid, \( \text{H}_2\text{SO}_4(\text{aq}) \)**Additional Tools:**- Solubility Table- Methods- My Notes- Lab Data**Instructions:**Select the appropriate reagents that can selectively precipitate one of the ions, allowing for separation based on solubility differences. Consult the solubility table for guidance on which compounds will form precipitates with the given ions.

To separate the given ions, we need to select the solutions with which only one of the ions will…

1) You are given an unknown solution, which contains both aqueous barium ion, Ba²+ (aq), and aqueous lead(11) ion, Pb2+ (aq). Which of your six solutions would allow separation of the ions? Select all that apply. A. Ammonium chloride, NH4Cl(aq) B. Nickel(II) nitrate, Ni(NO3)2(aq) C. Potassium chloride, KCl(aq) lity Table D. Silver nitrate, AgNO3(aq) E. Sodium hydroxide, NaOH(aq) F. Sulfuric acid, H₂SO4(aq)

1) You are given an unknown solution, which contains both aqueous barium ion, Ba²+ (aq), and aqueous lead(11) ion, Pb2+ (aq). Which of your six solutions would allow separation of the ions? Select all that apply. A. Ammonium chloride, NH4Cl(aq) B. Nickel(II) nitrate, Ni(NO3)2(aq) C. Potassium chloride, KCl(aq) lity Table D. Silver nitrate, AgNO3(aq) E. Sodium hydroxide, NaOH(aq) F. Sulfuric acid, H₂SO4(aq)

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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Concept explainers

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.

Arrhenius Acid

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.

Question

**Solubility and Qualitative Analysis: Laboratory Simulation**

**Problem:**
You are given an unknown solution containing both aqueous barium ions, \( \text{Ba}^{2+}(\text{aq}) \), and aqueous lead(II) ions, \( \text{Pb}^{2+}(\text{aq}) \). Which of your six solutions would allow separation of the ions?

**Select all that apply:**

- A. Ammonium chloride, \( \text{NH}_4\text{Cl}(\text{aq}) \)
- B. Nickel(II) nitrate, \( \text{Ni}(\text{NO}_3)_2(\text{aq}) \)
- C. Potassium chloride, \( \text{KCl}(\text{aq}) \)
- D. Silver nitrate, \( \text{AgNO}_3(\text{aq}) \)
- E. Sodium hydroxide, \( \text{NaOH}(\text{aq}) \)
- F. Sulfuric acid, \( \text{H}_2\text{SO}_4(\text{aq}) \)

**Additional Tools:**
- Solubility Table
- Methods
- My Notes
- Lab Data

**Instructions:**
Select the appropriate reagents that can selectively precipitate one of the ions, allowing for separation based on solubility differences. Consult the solubility table for guidance on which compounds will form precipitates with the given ions.

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