The solubility of calcium hydroxide Aim: to find out the solubility of a substance that only partially dissolves in water. Method: place about 100cm3 of distilled water in a flask and add about one spatula of solid calcium hydroxide. Stopper the flask and shake well for one minute. Leave to stand for at least 24 hours. Titrate 10cm3 samples against 0.05 mol dm-3 hydrochloric acid solution using methyl orange as an indicator. Obtain enough results to calculate an accurate average‚ and then
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Experiment 10: Solubility Product for Calcium Hydroxide GOAL AND OVERVIEW A saturated solution of Ca(OH)2 will be made by reacting calcium metal with water‚ then filtering off the solids: Ca(s) + H2O → Ca(OH)2(s) Ca2+(aq) + 2OH-(aq) The concentration of dissolved hydroxide will be determined by acid-base titration with standardized HCl solution. The Ksp for Ca(OH)2 will be calculated from the experimentally determined saturation concentration of hydroxide. Objectives of the data analysis understand
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the Solubility of Calcium Hydroxide Apparatus * Solid calcium hydroxide * 0.4 mol/dm hydrochloric acid * Distilled water * Pipette * Triple valve rubber pipette filler * Conical flask * Beaker * White tile * Clamp and stand * Methyl orange indicator Producing the calcium hydroxide solution 1. Roughly fill a beaker with 200cm³ of distilled water. This does not need to be accurate because samples will be taken from this. 2. Add solid calcium hydroxide‚ a spatula
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DETERMINATION OF THE SOLUBILITY PRODUCT CONSTANT OF CALCIUM HYDROXIDE ABSTRACT This experiment aimed to determine the solubility product constant (Ksp) of Ca(OH)2 as well as to evaluate the effects of common and non-common ions on its solubility. Ca(OH)2 solids were dissolved in eight various media: distilled water‚ 1.0 M KCl‚ 0.5 M KCl‚ 0.1 M KCl‚ 0.05 M KCl‚ 0.005 M KCl‚ 0.001 M KCl‚ and 0.1 M Ca(NO3)2. The concentration of dissociated OH- concentrations was determined by means of titrimetric
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Determination of the Solubility Product Constant of Calcium Hydroxide Introduction The equilibrium constant for the solubility equilibrium between an ionic solid and its ions is called solubility constant [1] ‚ Ksp of the solute. For example‚ the solubility product is defined by MxAy(s) ⇋xM(aq)y++ yA(aq)x- (1) Where M is the metal cation‚ A is the anion‚ x and y are the corresponding charges of the ions. The equilibrium expression is Ksp=[MY+]x[AX-]Y (2)
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unreactive elements. What does this tell you about their electronic structures? (2) 3 When calcium carbonate is heated it decomposes. The equation for this reaction is: CaCO3 → CaO + CO2 a Use numbers from the list to complete the sentences. 2 3 4 5 6 i The number of products in the equation is ....... (1) ii The formula CaCO3 shows that calcium carbonate was made from ....... different elements. iii The equation is balanced because there
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Investigating the solubility of Group II hydroxides Jiyeon Kim Aim: To investigate the solubility of Group II hydroxides (Mg(OH)2‚ Ca(OH)2‚ Sr(OH)2‚ Ba(OH)2) Research Question: What is the trend of solubility of Group II hydroxides going down the group as determined through measuring the volume of hydroxides needed to titrate with a known concentration of hydrochloric acid? Background Information: Solubility is when a solute forms a homogeneous solution by dissolving in solvent. The solubility of any
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CHAPTER 1 INTRODUCTION 1.1 INTRODUCTION Calcium is the largest mineral in the human body‚ where it plays an important role in absorption and the releasing of calcium in the body is through the intestinal and kidney. The calcium in the body is controlled by hormones and vitamins (Takano et al). The three major components that involve in the controller the calcium is parathyroid hormone (PTH)‚ calcitonin and Vitamin D. The consistent the calcium in the body from despite variation in-take and excretion
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Separation of the Components of a Mixture General Chemistry 1 (Chem 101)‚ ISP SCUHS Report 2 January 26‚ 2014 Abstract The analyses of mixture were to distinguish and identify homogeneous mixture by using the techniques of decantation and sublimation. By performing these techniques‚ we examined our solutions such as SiO2 (sand)‚ NH4Cl (ammonium chloride)‚ and NaCl (sodium chloride) and mixed H2O (water) with each solution after being heated. After examining our solutions‚ we made calculations
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In part 1 the results of the solubility do not agree with the with rules of solubility most likely because we put too much solid in the test tubes and not enough water to dissolve it. They should have dissolved because the anything with nitrate should be soluble. With the pH‚ when the mixture where compared with the chart all of them except NaCl where a shade of blue which means that they have a pH of 8-14‚ depending on the darkness of the shade‚ meaning that they are a basic solution. When reacting
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