Determination of solubility product of calcium hydroxide by titration. Free Essay: Determination of the Solubility of Calcium Hydroxide 2022-10-12

Determination of solubility product of calcium hydroxide by titration Rating: 5,2/10 1599 reviews

The solubility product of a compound is a measure of the concentration of its ions in solution. It is defined as the product of the ionic concentrations of the ions in the compound, each raised to the power of its respective stoichiometric coefficient in the dissociation reaction.

The solubility product of calcium hydroxide, Ca(OH)2, can be determined by titration. Titration is a laboratory technique in which a known concentration of a reactant, called the titrant, is added to a solution containing an unknown concentration of another reactant, called the analyte. The concentration of the analyte can be calculated from the volume and concentration of the titrant added.

To determine the solubility product of calcium hydroxide, a solution of the compound is prepared by dissolving a known mass of Ca(OH)2 in a known volume of water. The concentration of the Ca(OH)2 solution can be calculated from the mass and volume of the solution.

Next, a titration is performed using the Ca(OH)2 solution as the analyte and a solution of hydrochloric acid as the titrant. The hydrochloric acid solution is added to the Ca(OH)2 solution dropwise, while the pH of the mixture is monitored with a pH meter. The pH of the mixture increases as the hydrochloric acid is added, until it reaches a certain value. At this point, the Ca(OH)2 has been completely neutralized by the hydrochloric acid, and the titration is complete.

The volume and concentration of the hydrochloric acid solution used in the titration can be used to calculate the concentration of the Ca(OH)2 solution. From the concentration of the Ca(OH)2 solution, the solubility product of Ca(OH)2 can be calculated using the dissociation reaction for the compound:

Ca(OH)2 (s) → Ca2+ (aq) + 2 OH- (aq)

The solubility product of Ca(OH)2 can be used to predict the behavior of the compound in solution and to design processes that involve the use of calcium hydroxide. It is an important parameter in the fields of chemical engineering, materials science, and environmental science, among others.

In conclusion, the solubility product of calcium hydroxide can be determined by titration, using a solution of hydrochloric acid as the titrant and a solution of Ca(OH)2 as the analyte. The technique is useful for predicting the behavior of calcium hydroxide in solution and for designing processes that involve the use of the compound.

Determination of the Solubility Product Constant of Calcium Hydroxide

The data that were gathered were used to calculate the Ksp afterwards. Basically, Ksp is the quantification of the relationship of the ionic solid and its constituent ions. It was necessary to remove all of the solid Ca OH 2 before titrating because it would have affected the rate of reaction. This will aid in detecting the colour change. Continue to add the calcium hydroxide until no more will dissolve i.

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Determining Ksp of Calcium Hydroxide Through Titration Lab

The only way I can think of calculating is by trial and improvement. Wash out a 25cm pipette with the calcium hydroxide solution, by drawing up the solution with a pipette filler. This experiment can be improved by accuracy in the saturated solution preparation as well as in titration techniques. Boston: Houghton Mifflin Company. In this experiment, the solubility product constant, Ksp, of calcium hydroxide, Ca OH 2, was obtained using titration. Refill the flask with 25cm of the calcium hydroxide solution using the same process of filling it as before.

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Determination of the Solubility Product Constant of...

Once the titration began, the HCl was added until the methyl orange endpoint was reached, and as a result the volume of the HCl needed for the endpoint to be reached could be used in determining the moles and in turn the molar solubility and the solubility constant of the Ca OH 2. The first of these words is isotonic. Put a few drops of methyl orange into the conical flask. Place in water bath at the appropriate temperature, or heat on a hot plate, stirring occasionally, until equilibrium is achieved, which may be only a few minutes near 100 °C to 24 hr near room temperature. Repeat the titration, this time slowing the stream of the hydrochloric acid when it approaches the expected endpoint. The errors that caused the results could have come mainly from the preparation of the suspension, i.

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Solubility Product of Calcium Hydroxide

Methodology A precipitate was prepared by mixing 10 mL of 1. This is done using the titration method. Next , when the operating button is pressed to the first stop , the piston is expelled the same volume of air as indicated on the volume setting. The experiment was a failure in the common-ion effect part former , but was successful in the diverse-ion effect latter. About 75 mL of the suspension was then filtered.

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Free Essay: Determination of the Solubility of Calcium Hydroxide

Since the solids were really concentrated, it would have many reactions with the HCl. To compare the solubility would I just say the mass of calcium hydroxide that was not saturated is evidence to suggest that it is sparingly soluble? Approach the endpoint much more slowly and watch the colour of the solution of the flask carefully. The name salt peter is also applied to sodium nitrate. To work out the mass of calcium hydroxide in 1dm we must take the answer from before the amount of mole in 1dm and then multiply this by the formula mass of 74g. Record the temperature of the solution to the nearest degree. This diluted solution is to be used in future titrations. Another thing that could have minimized the error would be having the exact same mass of HCl.

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Determination Of The Solubility Product Constant Of Calcium Hydroxide, Sample of Essays

Ionic Strength Based on the graph, it is observed that the solubility of Ca OH 2 decreased through increasing ionic strength of the solution. Although the experiment yielded a contrary result to the diverse-ion effect, the experiment followed the common-ion effect for the relative solubility of Ca OH 2 in water compared to a solution with Ca2+. With a Pasteur pipette, the supernate was removed, leaving the precipitate behind which was later washed with 3 portions of 5-mL portions of water. Some possible sources of error in this experiment could have been, not reading the buret properly or titrating too much and passing the point where the solution turns yellow. After it is filtered, quickly measure out three 10. The equilibrium reaction of Ca OH 2 is expressed in 5. Place the conical flask containing the calcium hydroxide underneath the burette.

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Determination of the Solubility Product Constant of Calcium Hydroxide in Water

Procedure Temperature Dependence of K sp Place 100. Molar Solubility s , M CONCLUSIONS AND RECOMMENDATIONS 1. Since values were theorized to be with exactly. This experiment also aims to investigate the factors that influence the changes in the Ksp of an partially soluble ionic compound. See the diagram below 12.

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Exp 4 Determining the Solubility Product Constant (ksp) of Calcium Hydroxide

Measure out about 15 mL of the filtered solution into a 250 mL beaker. Purpose The purpose of this experiment is to determine the K sp value of aqueous calcium hydroxide by mixing it with a solution of hydrochloric acid with known molarity until equilibrium is reached. When regarding cells osmosis has three different terms that are used to describe their concentration. Report all results at 95% confidence and perform an error analysis. If you think you might have reached the endpoint, record the volume reading and then add another partial drop.

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Determination Of The Solubility Product Constant Of Calcium Hydroxide [k54677k1e9n8]

The solubility would be 0. Is there evidence for ion pair formation? As well, the molarity of Ca2+, and the Ksp is calculated. If some of the solid comes through the filter paper and is taken up with the pipette and used in the titration, the outcome could have been inaccurate because there would actually be less Ca OH 2 solute. The amount of calcium hydroxide needed should be around the value of 0. Record the precise volume of Ca OH 2 solution that you are using. Unfortunatelly my teacher told me that the titration will have to be done with HCl, he also told me that I have to calculate a reasonable concentration of HCl that needs to be used in the titration. When nearly all of the solution has gone out of the pipette gently tap the pipette on the bottom of the conical flask to get another drop out.

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Chem Lab 8

From it, a Ksp for Ca OH 2 in deionized water was obtained with a value of 1. The ionic strength is another factor that affects the Ksp value. It states that when a common ion is added into the solution of dissociated solids, the tendency would be towards the precipitation of the dissolved solid. Solubility is usually expressed as grams of solute in 100 g of solvent or in 1 dm3 of solution. From these KNO 3 solutions prepare saturated Ca OH 2 solutions at room temperature, as described above. Squeeze the large bulb at the top of the pipette filler and then squeeze valve 1 to draw the liquid up the pipette. Lastly, before it was dried, it was first washed with 95% ethanol.

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