SOLUBILITY EQUILIBRIUM OF CALCIUM HYDROXIDE
J.K. DE MATA
NATIONAL INSTITUTE OF PHYSICS, COLLEGE OF SCIENCE
UNIVERSITY OF THE PHILIPPINES, DILIMAN, QUEZON CITY, PHILIPPINES
DATE PERFORMED: OCTOBER 1, 2015
ABSTRACT
The objective of this experiment is to determine the solubility product constant, Ksp, of Ca(OH)2 through the titration of a saturated solution. This experiment also aims to investigate the factors that influence the changes in the Ksp of a partially soluble ionic compound. Different media of varying conditions were prepared and a 25-mL aliquot from each media was titrated with HCl. Volume used in titration was recorded and was used for the calculations. The graph obtained using the data gathered shows the relationship between
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It is also used for reef tanks in saltwater aquaria by making up limewater solutions, and is used as a pH regulating agent. Calcium hydroxide, Ca(OH)2, is an ionic solid that is only slightly soluble in water. A saturated solution of calcium hydroxide has the solid in equilibrium with its ions as shown below.
Ca(OH)2(s) ↔ Ca2+(aq) + 2OH-(aq) (1)
In this experiment, the equation of the Ksp was simplified into
Ksp = [ Ay+]x[Bx-]y (2)
From the expression above, the Ksp of Ca(OH)2 can be written as,
Ksp = [Ca2+][OH-]2 (3) where, [Ca2+] and [OH-] are the equilibrium
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Hence, due to the increase attractions between the participating ions, their effective concentrations become lesser causing a considerable increase in its solubility. This effect is governed by the ionic strength given by µ=1/2 ∑_i▒C_i z_i^2 (5) where ci is the molarity of ion and zi as the ion’s charge.
On the other hand, the common-ion effect is an application of the Le Chatelier’s principle which states that when a common ion is added into the solution of dissociated solids, the tendency of the reaction is to proceed towards the precipitation of the dissolved solid. This solution’s shifting equilibrium balances the reaction system in order to attain and maintain an equilibrium state. In this case, the addition on the product side needs to be balanced by formation of the original solid. [1]
This experiment aims to test a saturated solution of calcium hydroxide and calculate the Ksp of the compound.
METHODOLOGY
Table I. Six media at different conditions
Medium Condition
A : 50 mL distilled water : 28º C
B : 50 mL distilled water : 80º C
C : 50 mL distilled water : 10º C
D : 50 mL 0.10 M CaCl2 : 28º C
E : 50 mL 0.50 M KCl : 28º C
F : 45 mL distilled water + 5 mL 95% thanol : 28º
Goals The primary goal of this experiment was to identify an unknown compound by running various tests to determine the qualitative solubility, conductivity, and pH value of the compound. Tests were also performed for the presence of specific cations and anions in the compound. The second goal was to discover the reactivity of the unknown compound by reacting it with different types of substances. The third goal of this project was to calculate the quantitative solubility of the unknown compound in water.
a=What Jake is copying a=What James is copying a=What Zach is copying a= What Sean is copying Solubility of Sugar Lab Names: James, Jake, Zach, and Sean 2/28/16 5W Purpose: The purpose of this lab is to create crystals of hard rock candy from a supersaturated solution. Material List: hot plate triple beam balance 400 mL beaker clean glass jar Cup String 3 cups of sugar 1 cup of water beaker tongs food coloring (optional) glass stirring rod Procedure: 1.First collect materials listed 2.Use
In the next two paragraphs, I will show you the relationship
Purpose: The purpose of this lab is to titrate an unknown solid acid (KH2PO4) with a standardized sodium hydroxide solution. After recording and plotting the data, the acid’s equivalence point will be recorded once the color changes. Using the equivalence point, the halfway point will be calculated, which is used to determine the acid’s equilibrium constant. The acid’s calculated equilibrium constant will be compared with the acid’s established pKa value.
Standard Sodium hydroxide solution is the alkaline solution that will be used to titrate with soda water as it is a common solution that can be easily found in an ordinary school laboratory. It is a strong base. Carbonic acid is a weak acid which will react with a strong base to form a basic (pH > 7) solution. When Phenolphthalein is added to Soda water, the resultant solution is colourless. After titration with a strong base (sodium hydroxide), the solution will turn to pink as the solution becomes
- A hydrate is a salt that contains water as a part of its crystal structure. The hydrate used in this lab was Copper (ll) Sulfate Pentahydrate. To heat the hydrate in this lab a crucible is needed. A crucible is a heat resistant container used to heat things to high temperatures. In this lab a mole was used to determine the measurements of all substances.
CLAIRE MUNTING 29/01/2018 Criterion C EFFECTS OF SURFACE AREA OF CALCIUM CARBONATE UPON RATE OF REACTION Calcium Carbonate Chips 1 Introduction: Within the current investigation, the effects of the surface area of Calcium Carbonate (CaCO3) in combination with Hydrochloric acid (HCl) upon its rate of reaction. CaCO3, commonly referred to as limestone, is an organic substance and is, in a sense, the crystallised “carbonic salt” of the element, calcium2. In addition to being a salt, the pH level of Calcium Carbonate is 9.91, and it is therefore, a basic substance, due to the fact that it is comprised of a pH level higher than 7, which is neutral3. HCl, however, is the bodily acid found in the stomach of human beings.
Verna Wang Hannah Palmer CHEM 101-069 Lab 11-19-16 Stoichiometry and Limiting Reagents Lab Report Purpose: We are using the reaction of sodium hydroxide and calcium chloride to illustrate stoichiometry by demonstrating proportions needed to cause a reaction to take place. Background: Just like a recipe would call for a specific amount of one ingredient to a specific amount of another, stoichiometry is the same exact method for calculating moles in a chemical reaction. Sometimes, we may not have enough of or too much of one ingredient , which would be defined as limiting and excess reagent, respectively.
Introduction: In this lab, of water in a hydrate, or a substance whose crystalline structure is bound to water molecules by weak bonds, is determined by heating up a small sample of it. By heating, the water of hydration, or bound water, is removed, leaving only what is called an anhydrous compound. Based on the percent water in the hydrate, it can be classified as one of three types: BaCl2O ⋅ 2H20, with a percent water of about 14.57%, CuSO4
Strong acids and strong bases are strong electrolytes and are assumed to ionize completely in the presence of water. Weak acids however, only ionize to a limited extend in water. Any weak or strong acids when in contact with any weak or strong alkali will start to undergo neutralization regardless of their volume. When an indicator which is present in the acid-base mixture and have experienced colour change, it indicates that the mixture is in right proportions to neutralize each other and is also known as the equivalence point.
Since equilibrium cannot be reached, an electrochemical driving force is generated which acts on the ions. It is derived by finding the difference between the membrane potential obtained and the equilibrium potential expected. The sign of the value of this force decides the direction of movement of ions. Since we have cations (positive ions), a positive value shows movement of ions outside the cell membrane and a negative value shows movement of ions inside the cell membrane. If the value is equal to that of the equilibrium potential, the driving force acting on the ion is 0.
Back titration is used for this experiment as Calcium Carbonate is volatile and is an insoluble salt. Therefore they cannot fully dilute with water. As it’s chemical and physical properties are non ideal for a Direct titration, Direct titration cannot be used to determine the Calcium Carbonate content in toothpaste. In Back titration, excess volumes of HCl acids are added to allow for titration with NaOH. Eventually, the moles of CaCO3 can be found via stoichiometric property of the two reactants, and the mass of CaCO3 can be determined.
The calculated value was 1.6 x 10^-5. Conclusions The resulting Ka of the acetic acid from this experiment’s calculations was consistent with the experimental results. The experimental percent of CH3COOH was calculated at 1.6 x 10^-5, while the actual value was 1.8 x 10^-5.
Introduction Solubility is a chemical property that is measured in terms of the maximum amount of solute dissolved in a solvent at equilibrium. The resulting solution is called saturated solution. For example when a sample of sodium chloride solution in water is heated the behavior of the reaction is endothermic obstructing exothermic behavior. Another relationship that can be said about solubility is that the solubility of a solid substance increases as the temperature increases. The solubility of solutes is dependent on temperature.
That is, the higher the temperature of the solvent (water), the more solute (salt) that will dissolve in it. In this experiment, we will study the solubility of potassium nitrate (KNO3) in water. You will dissolve different quantities of this salt in a given amount of water at a temperature close to its boiling point. Which solution will be