Chapter 4, Problem 4.86QP

(a)

Interpretation Introduction

Interpretation: The affect on the ionic concentrations of the given aqueous mixtures is to be stated.

Concept introduction: Ionic compounds are those compounds in which a cation is bounded to anions through the bond. In ionic compounds, the negative charge is balanced with the positive charge. Ionic compounds dissociate into their respective ions in water.

Some examples of ionic compounds are sodium chloride, potassium nitrate and potassium chloride.

Some solubility rules for ionic compounds are,

• The alkali metal $\left(\text{group}\text{1}\text{A}\right)$ salts are soluble. Examples are Sodium chloride, potassium chloride.
• The salts in which nitrates are present are soluble.
• Ammonium salts are soluble.
• Sulfides, carbonates and phosphates are insoluble but sulfides, carbonates and phosphates of the alkali metal and ammonium sulfides, carbonates and phosphates are soluble.

To determine: If the ionic concentration of sodium chloride and iron $\left(\text{II}\right)$ chloride dissolved in $\text{100}\text{ml}$ of water will decrease or remain the same.

(b)

Interpretation Introduction

To determine: If the ionic concentration of the reaction of sodium carbonate with sulfuric acid in equimolar amounts will decrease or remain the same.

(c)

Interpretation Introduction

To determine: If the ionic concentration of potassium sulfate and barium nitrate dissolved in $\text{100}\text{ml}$ of water will decrease or remain the same.