Chemical Principles in the Laboratory
11th Edition
ISBN: 9781305264434
Author: Emil Slowinski, Wayne C. Wolsey, Robert Rossi
Publisher: Brooks Cole
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50.00 mL of 0.25 M HNO2 (nitrous acid, Ka = 4.74 x 10^-4) is titrated with 0.25 M KOH solution. What would be the pH of the solution after 25.00 mL of the KOH solution is added?
What is the solubility of Cr(OH)3 in g/l at pH 9.55? Ksp for Cr(OH)3 = 6.30 x 10-31?
Explain why K2CrO4 is used as an indicator in Argentometric titration?
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- Calamine, which is used for relief of skin irritations, is a mixture of zinc and iron oxides. A 1.022-g sample of dried calamine was dissolved in acid and diluted to 250.0 mL. A 50.00 mL aliquot was suitably buffered and titrated with 2.40 mL of 0.002727 M ZnY-2 (Zn-EDTA) solution to allow the following reaction: Fe+3 + ZnY-2 → FeY- + Zn+2. Molecular mass: Fe2O3 = 165.74 a. The weight of sample in the aliquot portion is _________g ? b. the percentage composition of Fe2O3 in the sample is ______ % ?arrow_forwardWhat will be the solubility of Fe(OH)3 (Ksp = 1.6 × 10–39) in:a. 0.0250 M FeCl3 solution?b. a solution buffered at pH 8.00? (First, calculate the OH– concentration at this pH)arrow_forwardEDTA is one of the common reagents used in a complexometric titration.a. Can we use EDTA titrations to determine the concentration of halides in a sample? Givereason for your answer.b. Why is EDTA used to determine concentration of a metal ion in a solution. c. Why is Erichrome black -T used as the indicator in EDTA titrations ?d. Explain hardness of water. Why is it usually expressed in terms of Ca2+ ions?arrow_forward
- 2. The molar solubility of sulfathiazole (weak acid) in water is about 0.001 M. a. What is the lowest pH allowable for complete solubility of a 1% solution of sodium sulfathiazole? (Mw = 277) , pKa = 7.12 b. A 5% solution?arrow_forwardWhat is the concentration of Cd2+ in a 0.016 M Cd(NO3)2 solution that is also 1.0 M NH3? For Cd(NH3)42+, Kf = 1.0 x 107.arrow_forwardAs part of a geological team that studied a local cave, you brought with you a bunch of 1.00 g rock samples to be studied. Each rock was prepared and titrated against 0.050 M EDTA. a. Calculate the percent calcite (CaCO3) content of rock A if it was titrated with 48.0 mL EDTAarrow_forward
- 1) Explain why you can dissolve Ni(OH)2 in aqueous ammonia. 2) Explain how the reaction of Ni(OH)2 with NH3 would enable you to separate a mixture of iron(III) 3) Could you use excess NaOH to separate a mixture of the precipitates of Fe(OH)3 and Ni(OH)2? Explain why or why not.arrow_forwardExplain why addition of NH3 or HNO3 to a saturated solution of Cu(OH)2 in contact with solid Cu(OH)2 increases the solubility of the solid.arrow_forward0.28g 0f MBr is dissolved in distilled water and made up to 250mL mark in a volumetric flask. 25 mL of this solution is titrated against 0.019 M silver nitrate solution using eosin as indicator. The end point was obtained at 12.4 mL of AgNO3 solution . Calculate the molar mass of the metal bromide.arrow_forward
- A buffer solution is made that is 0.392 M in HClO and 0.392 M in NaClO . (1) If Ka for HClO is 3.50×10-8, what is the pH of the buffer solution? (2) Write the net ionic equation for the reaction that occurs when 0.086 mol KOH is added to 1.00L of the buffer solution.arrow_forwardAs part of a geological team that studied a local cave, you brought with you a bunch of 1.00 g rock samples to be studied. Each rock was prepared and titrated against 0.050 M EDTA.a. Calculate the percent calcite (CaCO3) content of rock A if it was titrated with 48.0 mL EDTAb. Calculate the percent brucite (Mg(OH)2) content of rock B if it was titrated with 76.5 mL EDTAarrow_forwardAt 25C, 10.24 mg of Cr(OH)2 are dissolved in enough water to make 125 mL of solution. When equilibrium is established, the solution has a pH of 8.49. Estimate Ksp for Cr(OH)2.arrow_forward
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