August 28‚ 2009 [PROBLEM SET FROM R. CHANG TEST BANK] Chapter 16 Acid-Base Equilibria and Solubility Equilibria Student: ___________________________________________________________________________ NOTE: A table of ionization constants and Ka’s is required to work some of the problems in this chapter. 1. In which one of the following solutions will acetic acid have the greatest percent ionization? A. B. C. D. 2. Which one of the following is a buffer solution? A. B. C. D. E. 3. 0.40 M HCN and
Free PH Buffer solution Sodium hydroxide
of lead(II) chloride (PbCl2) at 25oC. Ksp = 1.62e–5. A) 1.59e–2 B) 2.53e–2 C) 6.64e–17 D) 2.01e–3 E) 2.01e–2 2. The two salts AgX and AgY have very similar solubilities in water. It is known that the salt AgX is much more soluble in acid than is AgY. What can be said about the relative strengths of the acids HX and HY? A) Nothing. B) HY is stronger than HX. C) HX is stronger than HY. D) The acids have equal strengths. E) Cannot be determined. 3. Solubility Products (Ksp) BaSO4 1
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Selective precipitation of the Barium Magnesium Group Chem 112-004 Abstract The purpose of this experiment is to separate and identify the cations of Ba+‚Sr2+‚Ca2+‚ Mg2+ and NH4+ using differences in solubility and confirming test to identify the unknown solution used in this experiment. In this experiment the methodology used by the group is to perform the tests for both the unknown and the cations (Ba+‚Sr2+‚Ca2+‚ Mg2+ and NH4+) using the known as a control for comparison and identification
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solubility-product constant‚ Ksp‚ for Cu(OH)2 at 25 °C. Ksp = [Cu 2+][OH –]2 = [1.76 x10–7][3.53 x10–7]2 = 2.20 x10–20 (b) The value of the solubility-product constant‚ Ksp‚ for Zn(OH)2 is 7.7 x10–17 at 25 °C. (i) Calculate the solubility (in moles per liter) of Zn(OH)2 at 25 °C in a solution with a pH of 9.35. Zn(OH)2 Zn 2+ + 2 OH – Ksp = [Zn 2+][OH –]2 pH 9.35 = pOH 4.65; [OH –] = 10–4.65 = 2.24 x10–5 M Zn2+ = Ksp/[OH -]2 = 7.7x10-17/[2
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Unur Abdul Kader T.A: Katie Experiment 22: Molar Solubility‚ Common-Ion Effect Abstract The purpose of this experiment was to determine the molar solubility‚ the solubility constant‚ and the effect of a common ion on the molar solubility of calcium hydroxide. To accomplish this the experiment was split into two parts; part A and Part B. in Part A of the experiment a standardized 0.05 M solution of HCl was titrated into a 25 mL solution of saturated Ca(OH)2 which contained 2 drops of orange methyl
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Determination of the Solubility Product Constant of Calcium Hydroxide Austin Raniel Tan Institute of Chemistry‚ College of Science‚ University of the Philippines‚ Diliman‚ Quezon City 1101 Philippines ------------------------------------------------- Christian Tica‚ Ryan Tabernilla‚ Michael Siao‚ Ron Mabunga‚ Jaime Olivares‚ and rest of Team Pogi Abstract ------------------------------------------------- By measuring the concentration of the hydroxide ion from a solution saturated with
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The equation for the reaction between a free calcium ion and an EDTA compound in pH of 10 is a 1:1 reaction which allows to see how many calcium ions were stabilized and therefore dissociated from the CaC2O4. This number of moles can then be multiplied by the molecular mass of CaC2O4 to find the initial weight of the ions that dissociated which
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Aim: To find the solubility and the solubility product of calcium hydroxide. Theory: Define‚ with equation‚ the solubility product. Find‚ from literature‚ the solubility product of calcium hydroxide at 25oC. Experimental: Reagents: solid calcium hydroxide‚ water‚ 0.1 moldm-3 hydrochloric acid Apparatus: Procedure: 1. An empty bottle was weighed. Then the empty bottle was weigh with 1g calcium hydroxide. 2. 100 cm3 of distilled water was added to the bottle. For about
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Measuring the Solubility Product of Ca(OH)2 Purpose: The purpose of this investigation is to find the solubility product (Ksp) of Ca(OH)2 by titrating the hydrochloric acid with calcium hydroxide and using their entities to find the concentration of Ca2+ and OH- ions. Materials: Refer to lab sheet “Measuring the Solubility of Ca(OH)2” (handout) Method (Procedure): Refer to lab sheet “Measuring the Solubility of Ca(OH)2” (handout) Observations Trial 1 Trial 2 Initial burette reading 0mL 17.75mL
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GRAVIMETRIC ANALYSIS OF A CHLORIDE SALT Report Submitted by: Ronald Milner Laboratory partner: Kiesha Mantik Lab Performed: February 16th‚ 2012 Group: Thursday Afternoon‚ Group F Date submitted: March 14th‚ 2012 Purpose: To determine the chloride content of an unknown soluble salt while illustrating the techniques involved in gravimetric analysis. Theory: In order to find the chloride content of an unknown soluble salt‚ that chloride can first be extracted from the
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