Perform all of the following tasks: A. Write the chemical reaction for the CalOH

Question

Perform all of the following tasks: A. Write the chemical reaction for the CalOH) equilibrium system. B. What was the effect (observations) of the addition of HCI? Indicate what the stress was (the 1. librium position shifted reactant or product added or removed) and which way the equil (forward, reverse, no change) What was the effect of the addition of NaOH? Indicate what the stress was (the reactant or product added or removed) and which way the equilibrium position shifted ( reverse, no change). (30 points) C. forward, ilior

Explanation / Answer

1. Calcium hydroxide is a partially soluble base which when added to water stays in an equilibrium with its ionized and unionized form thus appearing as a precipitate.

A. The equilibrium established by calcium hydroxide in water is given as Ca(OH)2 <-----> Ca2+ + 2OH- which shows that the base only partially ionized in the medium.

B. When HCl is added to the suspension of calcium hydroxide in water, a neutralization reaction occurs wherein the hydroxide ions released by the salt is consumed by the protons released by HCl giving water and calcium chloride as the products. In this case, the product side species - hydroxide ions are consumed in the process which is the primary stress to the equilibrium. This results in a greater quantity of calcium hydroxide ionizing as calcium and hydroxide ions which is observed as the dissolution of the precipitate. Thus it can be inferred that the equilibrium moves forward as HCl is added.

C. When NaOH is added to the medium, being a strong base unlike calcium hydroxide, it dissociates completely to give sodium and hydroxide ions in the medium. Now, a greater quantity of the product species - hydroxide ions are added externally which is the stress to the equilibrium. This results in the equilibrium responding by decreased ionization leading to greater quantities of calcium hydroxide forming from the calcium and hydroxide ions in the medium. This results in the appearance of greater quantities of the weak base as a precipitate. Thus the equilibrium moves backward when NaOH is added.

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