PDFchem_353_2020-2021_final.pdfDosya | C:/Users/Asus/Downloads/chem_353_2020-2021_final.pdfSolubility of KNO370Answer the following 3 questions by using this sohubility graphof KNO3.O 6050O 4030201010 20 30 40 50 60 70 80 90Temperature (c)a) What happens to a solution of KNO3 that is saturated at 50°C when it is cooled quickly to10°C? EXPLAIN.b) How would you describe a solution of KNO3 at 80°C if there are about 45 g of KNO3dissolved in 100 g of water? EXPLAIN.c) How many grams of KNO3 need to be dissolved in 300 g of water in order to have asaturated solutionSolubility (g/100 g)of

(a) From the graph it is clear that at 50°C,solubility ofKNO3is 20 gm/100 gm 10°C solubility of KNO3…

Solubility of KNOs 70 Answer the following 3 questions by using this solubility graph of KNOs. 60 50 40 30 20 10 O 10 20 30 40 s0 60 70 80 90 Temperature (C) a) What happens to a solution of KNO; that is saturated at 50°C when it is cooled quickly to 10°C? EXPLAIN. b) How would you describe a solution of KNO, at 80°C if there are about 45 g of KNO, dissolved in 100 g of water? EXPLAIN. (8 0OL6) Aamanjos

Solubility of KNOs 70 Answer the following 3 questions by using this solubility graph of KNOs. 60 50 40 30 20 10 O 10 20 30 40 s0 60 70 80 90 Temperature (C) a) What happens to a solution of KNO; that is saturated at 50°C when it is cooled quickly to 10°C? EXPLAIN. b) How would you describe a solution of KNO, at 80°C if there are about 45 g of KNO, dissolved in 100 g of water? EXPLAIN. (8 0OL6) Aamanjos

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter7: Statistical Data Treatment And Evaluation

Section: Chapter Questions

Problem 7.26QAP

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The following evidence was obtained from an experiment to determine the solubility of calcium chloride at room temperature. A sample of saturated calcium chloride solution was evaporated to dryness, and the mass of solid residue was measured.EvidenceVolume of solution (mL) = 15.0Mass of empty beaker (g) = 90.54Mass of beaker and residue (g) = 101.36The solubility of calcium chloride is g/100 mL
1.1The Ksp of Ca3 (PO4 ) 2 is 1.3 × 10−26 . Estimate the solubility of this salt in units of g. L −1 . You must show any reaction equation(s) that you may think are necessary. 1.2 If a sample of solid Ca3(PO4)2 is stirred into exactly one litre of a 0.550M solution of Na3PO4, how will the solubility of the salt compare with the answer that you have obtained in question 1.1? Explain you answer in a short sentence.
A solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Find the freezing point of the solution(in C to 2 decimal places)
A solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Find the osmotic pressure in atm to three decimal places
A solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Determine the boiling point of the solution(in C to 2 decimal places)
A solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Determine the following: Boiling point of solution (in °C to two decimal places) Freezing point of solution (in °C to two decimal places) Vapor pressure of the solution (in atm to three decimal places) Osmotic pressure (in atm to three decimal places)
1. The Ksp of Ca3(PO4)2 is 1.3 × 10−26. Estimate the solubility of this salt in units of g. L−12. If a sample of solid Ca3(PO4)2 is stirred into exactly one litre of a 0.550M solution of Na3PO4, how will the solubility of the salt compare with the answer that you have obtained in question 2.1? Explain you answer in a short sentence.
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