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Using the solubility chart below, identify the cations that would be expected to form a precipitate upon initial addition of sulfate SO4 2- Answer options, Select all that apply: Fe3+ Ni2+ K+ Ba2+ Cd2+ Ag+ Mg2+ Cu 2+ Ca2+ Pb2+ Zn2+ Al 3+

Using the solubility chart below, identify the cations that would be expected to form a precipitate upon initial addition of sulfate SO4 2- Answer options, Select all that apply: Fe3+ Ni2+ K+ Ba2+ Cd2+ Ag+ Mg2+ Cu 2+ Ca2+ Pb2+ Zn2+ Al 3+

Chemistry
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
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Using the solubility chart below, identify the cations that would be expected to form a precipitate upon initial addition of sulfate SO4 2-

Answer options, Select all that apply:

Fe3+

Ni2+

K+

Ba2+

Cd2+

Ag+

Mg2+

Cu 2+

Ca2+

Pb2+

Zn2+

Al 3+

 

The image displays a comprehensive solubility chart for various cations when combined with anions: Cl(−), Br(−), I(−), SO₄(2−), CO₃(2−), PO₄(3−), OH(−), S(2−), and CrO₄(2−). - **Aq** indicates that the compound is soluble in water, forming an aqueous solution. - **I** indicates that the compound is insoluble or poorly soluble in water, forming a precipitate. - **D** stands for decomposition or dissolution under specific conditions. Highlighted sections for different cations are: - **Blue** background for cations including Aluminum Al(3+), Ammonium NH₄(+), Barium Ba(2+), Cadmium Cd(2+), Calcium Ca(2+), Copper Cu(2+), Lead Pb(2+) or (4+), Mercury Hg(2+), Nickel Ni(2+) or (3+), Potassium K(+), Sodium Na(+), Zinc Zn(2+). - **Yellow** background for cations, such as Bismuth Bi(3+), Iron (ferrous) Fe(2+), Iron (ferric) Fe(3+), Magnesium Mg(2+), Manganese, and Silver Ag(+). This chart helps in predicting the solubility behavior of various ionic compounds in water, enabling learners to understand the conditions under which a compound will dissolve or form a precipitate.
Transcribed Image Text:The image displays a comprehensive solubility chart for various cations when combined with anions: Cl(−), Br(−), I(−), SO₄(2−), CO₃(2−), PO₄(3−), OH(−), S(2−), and CrO₄(2−). - **Aq** indicates that the compound is soluble in water, forming an aqueous solution. - **I** indicates that the compound is insoluble or poorly soluble in water, forming a precipitate. - **D** stands for decomposition or dissolution under specific conditions. Highlighted sections for different cations are: - **Blue** background for cations including Aluminum Al(3+), Ammonium NH₄(+), Barium Ba(2+), Cadmium Cd(2+), Calcium Ca(2+), Copper Cu(2+), Lead Pb(2+) or (4+), Mercury Hg(2+), Nickel Ni(2+) or (3+), Potassium K(+), Sodium Na(+), Zinc Zn(2+). - **Yellow** background for cations, such as Bismuth Bi(3+), Iron (ferrous) Fe(2+), Iron (ferric) Fe(3+), Magnesium Mg(2+), Manganese, and Silver Ag(+). This chart helps in predicting the solubility behavior of various ionic compounds in water, enabling learners to understand the conditions under which a compound will dissolve or form a precipitate.
**Accessible Solubility Table** **Header Row:** - **Ion** - **Solubility** - **Exceptions** **Table Body arranged in rows:** 1. **NO₃⁻** - Solubility: Soluble - Exceptions: None 2. **Cl⁻** - Solubility: Soluble - Exceptions: Ag⁺, Hg₂²⁺, Pb²⁺ 3. **I⁻** - Solubility: Soluble - Exceptions: Ag⁺, Hg₂²⁺, Pb²⁺ 4. **SO₄²⁻** - Solubility: Soluble - Exceptions: Ca²⁺, Ba²⁺, Sr²⁺, Hg₂²⁺, Pb²⁺, Ag⁺ 5. **CO₃²⁻** - Solubility: Insoluble - Exceptions: Group IA and NH₄⁺ 6. **PO₄³⁻** - Solubility: Insoluble - Exceptions: Group IA and NH₄⁺ 7. **OH⁻** - Solubility: Insoluble - Exceptions: Group IA, Ca²⁺, Ba²⁺, Sr²⁺ *Note: "IA" refers to Group 1 elements (alkali metals) on the periodic table. "NH₄⁺" refers to the ammonium ion.* **Chart Explanation:** At the top, there's a table listing various ions with their respective solubility and exceptions. It covers a wide array of ions including acetate, bromide, carbonate, chlorate, chloride, chromate, hydroxide, iodide, nitrate, oxide, phosphate, silicate, sulfate, and sulfide. Each ion is labeled with either “Aq” for aqueous (soluble) or “I” for insoluble, along with a brief description of exceptions where applicable. The chart is likely used in educational contexts for quick reference on chemical compound solubility.
Transcribed Image Text:**Accessible Solubility Table** **Header Row:** - **Ion** - **Solubility** - **Exceptions** **Table Body arranged in rows:** 1. **NO₃⁻** - Solubility: Soluble - Exceptions: None 2. **Cl⁻** - Solubility: Soluble - Exceptions: Ag⁺, Hg₂²⁺, Pb²⁺ 3. **I⁻** - Solubility: Soluble - Exceptions: Ag⁺, Hg₂²⁺, Pb²⁺ 4. **SO₄²⁻** - Solubility: Soluble - Exceptions: Ca²⁺, Ba²⁺, Sr²⁺, Hg₂²⁺, Pb²⁺, Ag⁺ 5. **CO₃²⁻** - Solubility: Insoluble - Exceptions: Group IA and NH₄⁺ 6. **PO₄³⁻** - Solubility: Insoluble - Exceptions: Group IA and NH₄⁺ 7. **OH⁻** - Solubility: Insoluble - Exceptions: Group IA, Ca²⁺, Ba²⁺, Sr²⁺ *Note: "IA" refers to Group 1 elements (alkali metals) on the periodic table. "NH₄⁺" refers to the ammonium ion.* **Chart Explanation:** At the top, there's a table listing various ions with their respective solubility and exceptions. It covers a wide array of ions including acetate, bromide, carbonate, chlorate, chloride, chromate, hydroxide, iodide, nitrate, oxide, phosphate, silicate, sulfate, and sulfide. Each ion is labeled with either “Aq” for aqueous (soluble) or “I” for insoluble, along with a brief description of exceptions where applicable. The chart is likely used in educational contexts for quick reference on chemical compound solubility.
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