The reason as to why inspite of the low solubility of Ca ( OH ) 2 it becomes soluble in acidic solution is to be stated in terms of Le Chatelier’s Principle. Concept introduction: The equilibrium is a state of the chemical reaction in which the rate of the forward reaction and the rate of the backward reaction become the same. There is no net change in the concentration of reactants and products at the equilibrium condition.

Question

3. The following reaction has a Keq = 6.3 × 10–38. 3Fe(OH)3 (s) ⇌ Fe3+(aq) + 3OH3–(aq) Use this information to explain your observations of the position of the equilibrium in the presence of OH–(Part 1b). (HINT: Think about what happens to Fe3+(aq) when there is OH– (aq) present.) 4. As part of the discussion, explain your results from Part 2 within the context of Le Châtelier’s Principle. Look at the cobalt equilibrium and decide which is pink (I or II) and which is blue? Co(H2O)62+ + 2Cl– ⇌ CoCl2(H2O)2 + 4H2O I II As part of the discussion, explain the effect of changing the temperature based upon your observations. Is the cobalt equilibrium exothermic or endothermic, as it is written? Explain your observations with respect to the addition of saturated aqueous sodium chloride solution and the addition of water. (HINT: what is the major component of aqueous sodium chloride?)

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Question

Chapter 18, Problem 39E

Interpretation Introduction

Interpretation:

The reason as to why inspite of the low solubility of Ca(OH)2 it becomes soluble in acidic solution is to be stated in terms of Le Chatelier’s Principle.

Concept introduction:

The equilibrium is a state of the chemical reaction in which the rate of the forward reaction and the rate of the backward reaction become the same. There is no net change in the concentration of reactants and products at the equilibrium condition.

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