which cation present in the unknown soluble ionic compound has to be predicted. Concept introduction: When the cations and anions switch partners, they result in the arrangement of two new ionic compounds one of which is in the solid state. The hard product is an insoluble ionic compound called a precipitate . The rules for salts to be soluble in water are as follows 1. Most of the Nitrate salts are soluble 2. Salts containing the cation as alkali metal such as Sodium, Magnesium, Rubidium etc and Ammonium are said to be water soluble. 3. Salts of Bromide, Chloride and Iodide are said to be water soluble except in case of cations such as silver, Lead and Mercury. 4. Most of the Sulphate salts are soluble except Barium sulphate, Mercury sulphate, Lead sulphate and Calcium sulphate. 5. Most of the hydroxides are sparingly soluble except Sodium hydroxide and Potassium hydroxide. 6. Most of the Sulphide, Carbonate, Chromates and Phosphates are less soluble except those include in the rule 2.

Question

> You are trying to decide if there is a single reagent you can add that will make the following synthesis possible without any other major side products: 1. ☑ CI 2. H3O+ O Draw the missing reagent X you think will make this synthesis work in the drawing area below. If there is no reagent that will make your desired product in good yield or without complications, just check the box under the drawing area and leave it blank. Click and drag to start drawing a structure. Explanation Check ? DO 18 Ar B © 2025 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility

Answer 1

Question

Chapter 6, Problem 56E

(a)

Interpretation Introduction

Interpretation: which cation present in the unknown soluble ionic compound has to be predicted.

Concept introduction: When the cations and anions switch partners, they result in the arrangement of two new ionic compounds one of which is in the solid state. The hard product is an insoluble ionic compound called a precipitate.

The rules for salts to be soluble in water are as follows

1. Most of the Nitrate salts are soluble

2. Salts containing the cation as alkali metal such as Sodium, Magnesium, Rubidium etc and Ammonium are said to be water soluble.

3. Salts of Bromide, Chloride and Iodide are said to be water soluble except in case of cations such as silver, Lead and Mercury.

4. Most of the Sulphate salts are soluble except Barium sulphate, Mercury sulphate, Lead sulphate and Calcium sulphate.

5. Most of the hydroxides are sparingly soluble except Sodium hydroxide and Potassium hydroxide.

6. Most of the Sulphide, Carbonate, Chromates and Phosphates are less soluble except those include in the rule 2.

(b)

Interpretation Introduction

Interpretation: which cation present in the unknown soluble ionic compound has to be predicted.

Concept introduction: When the cations and anions switch partners, they result in the arrangement of two new ionic compounds one of which is in the solid state. The hard product is an insoluble ionic compound called a precipitate.

The rules for salts to be soluble in water are as follows

1. Most of the Nitrate salts are soluble

2. Salts containing the cation as alkali metal such as Sodium, Magnesium, Rubidium etc and Ammonium are said to be water soluble.

3. Salts of Bromide, Chloride and Iodide are said to be water soluble except in case of cations such as silver, Lead and Mercury.

4. Most of the Sulphate salts are soluble except Barium sulphate, Mercury sulphate, Lead sulphate and Calcium sulphate.

5. Most of the hydroxides are sparingly soluble except Sodium hydroxide and Potassium hydroxide.

6. Most of the Sulphide, Carbonate, Chromates and Phosphates are less soluble except those include in the rule 2.

(c)

Interpretation Introduction

Interpretation: which cation present in the unknown soluble ionic compound has to be predicted.

Concept introduction: When the cations and anions switch partners, they result in the arrangement of two new ionic compounds one of which is in the solid state. The hard product is an insoluble ionic compound called a precipitate.

The rules for salts to be soluble in water are as follows

1. Most of the Nitrate salts are soluble

2. Salts containing the cation as alkali metal such as Sodium, Magnesium, Rubidium etc and Ammonium are said to be water soluble.

3. Salts of Bromide, Chloride and Iodide are said to be water soluble except in case of cations such as silver, Lead and Mercury.

4. Most of the Sulphate salts are soluble except Barium sulphate, Mercury sulphate, Lead sulphate and Calcium sulphate.

5. Most of the hydroxides are sparingly soluble except Sodium hydroxide and Potassium hydroxide.

6. Most of the Sulphide, Carbonate, Chromates and Phosphates are less soluble except those include in the rule 2.

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> You are trying to decide if there is a single reagent you can add that will make the following synthesis possible without any other major side products: 1. ☑ CI 2. H3O+ O Draw the missing reagent X you think will make this synthesis work in the drawing area below. If there is no reagent that will make your desired product in good yield or without complications, just check the box under the drawing area and leave it blank. Click and drag to start drawing a structure. Explanation Check ? DO 18 Ar B © 2025 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility

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Consider a solution of 0.00304 moles of 4-nitrobenzoic acid (pKa = 3.442) dissolved in 25 mL water and titrated with 0.0991 M NaOH. Calculate the pH at the equivalence point