**Solubility Rules for Some Ionic Compounds in Water****Soluble Ionic Compounds**1. All sodium (Na⁺), potassium (K⁺), and ammonium (NH₄⁺) salts are SOLUBLE.2. All nitrate (NO₃⁻), acetate (CH₃CO₂⁻), chlorate (ClO₃⁻), and perchlorate (ClO₄⁻) salts are SOLUBLE.3. All chloride (Cl⁻), bromide (Br⁻), and iodide (I⁻) salts are SOLUBLE — EXCEPT those containing: lead, silver, or mercury (I) (Pb²⁺, Ag⁺, Hg₂²⁺) which are NOT soluble.4. All sulfate (SO₄²⁻) salts are SOLUBLE — EXCEPT those containing: calcium, silver, mercury (I), strontium, barium, or lead (Ca²⁺, Ag⁺, Hg₂²⁺, Sr²⁺, Ba²⁺, Pb²⁺) which are NOT soluble.**Not Soluble Ionic Compounds**5. Hydroxide (OH⁻) and oxide (O²⁻) compounds are NOT SOLUBLE — EXCEPT those containing: sodium, potassium, or barium (Na⁺, K⁺, Ba²⁺) which are soluble.6. Sulfide (S²⁻) salts are NOT SOLUBLE — EXCEPT those containing: sodium, potassium, ammonium, or barium (Na⁺, K⁺, NH₄⁺, Ba²⁺) which are soluble.7. Carbonate (CO₃²⁻) and phosphate (PO₄³⁻) are NOT SOLUBLE — EXCEPT those containing: sodium, potassium, or ammonium (Na⁺, K⁺, NH₄⁺) which are soluble.**Additional Notes:**- *Soluble compounds* are defined as those that dissolve to the extent of 1 g or more per 100 g water.- *NOT soluble compounds* are further classified as: - Slightly soluble, which dissolve to the extent of 0.01 to 1 g per 100 g water. - Difficulty soluble or Insoluble, for which less than 0.01 g per **Write the dissolution reaction for calcium sulfide in water.**Be sure to specify the state of each reactant and product.[Blank rectangle] → [Blank rectangle] + [Blank rectangle]---**Is calcium sulfide considered soluble or not soluble?**A. Soluble B. Not soluble [a]---**Based upon this, the equilibrium constant for this reaction will be:**A. Greater than 1 B. Less than 1 [a]---**Note:**- The diagram consists of empty rectangles representing reactants and products, separated by an arrow. The layout prompts users to fill in specific chemical formulas with their physical states.- Two multiple-choice questions ask about the solubility of calcium sulfide and the relative size of the equilibrium constant, with placeholders for responses.

Calcium sulphide is an ionic compound which is sparingly soluble in water which dissociates into its…

Write the dissolution reaction for calcium sulfide in water. Be sure to specify the state of each reactant and product. Is calcium sulfide considered soluble or not soluble ? A. Soluble B. Not soluble Based upon this, the equilibrium constant for this reaction will be: A. Greater than 1 B. Less than !

Write the dissolution reaction for calcium sulfide in water. Be sure to specify the state of each reactant and product. Is calcium sulfide considered soluble or not soluble ? A. Soluble B. Not soluble Based upon this, the equilibrium constant for this reaction will be: A. Greater than 1 B. Less than !

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 Rules for Some Ionic Compounds in Water**

**Soluble Ionic Compounds**

1. All sodium (Na⁺), potassium (K⁺), and ammonium (NH₄⁺) salts are SOLUBLE.

2. All nitrate (NO₃⁻), acetate (CH₃CO₂⁻), chlorate (ClO₃⁻), and perchlorate (ClO₄⁻) salts are SOLUBLE.

3. All chloride (Cl⁻), bromide (Br⁻), and iodide (I⁻) salts are SOLUBLE — EXCEPT those containing: lead, silver, or mercury (I) (Pb²⁺, Ag⁺, Hg₂²⁺) which are NOT soluble.

4. All sulfate (SO₄²⁻) salts are SOLUBLE — EXCEPT those containing: calcium, silver, mercury (I), strontium, barium, or lead (Ca²⁺, Ag⁺, Hg₂²⁺, Sr²⁺, Ba²⁺, Pb²⁺) which are NOT soluble.

**Not Soluble Ionic Compounds**

5. Hydroxide (OH⁻) and oxide (O²⁻) compounds are NOT SOLUBLE — EXCEPT those containing: sodium, potassium, or barium (Na⁺, K⁺, Ba²⁺) which are soluble.

6. Sulfide (S²⁻) salts are NOT SOLUBLE — EXCEPT those containing: sodium, potassium, ammonium, or barium (Na⁺, K⁺, NH₄⁺, Ba²⁺) which are soluble.

7. Carbonate (CO₃²⁻) and phosphate (PO₄³⁻) are NOT SOLUBLE — EXCEPT those containing: sodium, potassium, or ammonium (Na⁺, K⁺, NH₄⁺) which are soluble.

**Additional Notes:**

- *Soluble compounds* are defined as those that dissolve to the extent of 1 g or more per 100 g water.
- *NOT soluble compounds* are further classified as:
- Slightly soluble, which dissolve to the extent of 0.01 to 1 g per 100 g water.
- Difficulty soluble or Insoluble, for which less than 0.01 g per

**Write the dissolution reaction for calcium sulfide in water.**

Be sure to specify the state of each reactant and product.

[Blank rectangle] → [Blank rectangle] + [Blank rectangle]

---

**Is calcium sulfide considered soluble or not soluble?**

A. Soluble
B. Not soluble [a]

---

**Based upon this, the equilibrium constant for this reaction will be:**

A. Greater than 1
B. Less than 1 [a]

---

**Note:**

- The diagram consists of empty rectangles representing reactants and products, separated by an arrow. The layout prompts users to fill in specific chemical formulas with their physical states.
- Two multiple-choice questions ask about the solubility of calcium sulfide and the relative size of the equilibrium constant, with placeholders for responses.

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