Joshua Browning and Ian Lobo Purpose:
The accepted Ksp value for this substance is 7. This resulted in a When the solution contained some solids, it was known that it is saturated.
Since this solution was saturated it was implied that it was at equilibrium. Being at equilibrium the forward reaction had to equal the reverse reaction.
This implied that the dissolving and crystallization reactions happened at an equal rate and simultaneously. For these reactions to be equal, some precipitate would have been present, indicating the saturated solution was at equilibrium. It was necessary to remove all of the solid Ca OH 2 before titrating because the it would have affected the rate of reaction.
When the HCl was titrated with Ca OH 2, some of the solid would go down with the liquid because of a minuscule amount of filtering. Since the solids were really concentrated, it would have many reactions with the HCl.
Therefore, the amount of Ca OH 2 had to be only liquid, with no solid pieces going into the burette, which would have neutralized the acid too quickly. Without a pure solution of Ca OH 2 the amount of the solution would change that was needed to titrate the HCl.
The value of solution went up thus giving a different value then was first assumed for Ksp. The less that was filtered lead to a higher value for the Ksp then first thought. Another source of error would have been the measuring of the HCl not being exactly.
The changing masses of HCl would change the results a fair amount since the values theorized in the prelab calculations was for. The more HCl added the higher the Ksp, the less added the lower the Ksp values would have been. One way to minimize the errors in this lab would have been to maintain the temperature of the surroundings at SATP.
A temperature of 25 Celsius would have guaranteed that the assumed Ksp value was the correct one that was assumed in the prelab calculation. This value would have given the most accurate results for theorizing other values.
Another thing that could have minimized the error would be having the exact same mass of HCl. Since values were theorized to be with exactly. This can be shown using the equation:Determining Ksp of Calcium Hydroxide Introduction Aqueous calcium hydroxide, also known as lime water is used to verify the presence of carbon dioxide gas, (carbon dioxide reacts with the calcium hydroxide to produce calcium carbonate) this is achieved by bubbling the gas through the solution, if the solution turns cloudy then the precipitate calcium carbonate has formed, thus carbon dioxide is present.
Calculate the Ksp of calcium hydroxide Ksp = [Ca 2 +] [OH-] 2; Calculate the molarity of a saturated Ca(OH) 2 solution in moles/liter. Calculate the concentration of a saturated Ca(OH) 2 solution in grams/liter.
Determine the concentration of a Ca(OH) 2 saturated solution in grams/ mL Questions. A saturated solution of calcium hydroxide is dilute.
Determining Ksp of Calcium Hydroxide Introduction Aqueous calcium hydroxide, also known as lime water is used to verify the presence of carbon dioxide gas, (carbon dioxide reacts with the calcium hydroxide to produce calcium carbonate) this is achieved by bubbling the gas through the solution, if the solution turns cloudy then the.
A s time goes by, most reef aquarists will encounter a solid precipitate of some sort in conjunction with their reef aquarium. Often these are undesirable particles that cloud the water, coat the glass or clog pumps.
Others are more benign and disappear shortly after forming. Calcium similarly forms ion pairs with carbonate and bicarbonate.
While these comprise a small fraction of the total calcium, the calcium carbonate ion pair comprises a fairly large portion of the total carbonate (together with magnesium, about 2/3 of the carbonate).
A saturated solution of calcium hydroxide (lime water) is titrated with hydrochloric acid of known concentration, and the Ksp of calcium hydroxide is determined from the resulting information. Safety Calcium hydroxide is caustic and hydrochloric acid is corrosive; both can cause blindness.