10pGasometricNaHCO3

# 10pGasometricNaHCO3 - Gasometric Determination of NaHCO3 in...

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Click to edit Master subtitle style Gasometric Determination Last Update: 2/2/10 07:10:04 AM

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Purpose: Determine the percent of NaHCO3 in a mixture by Gasometry Concepts: Ideal Gas LawHenry’s Law Vapor Pressure Stoichiometry Techniques: Capture Gaseous Product Corrections to volume Apparatus: Syringe Thermometer Barometer
The Exercise is Conceptually Simple . 1. Weigh Sample, wSample . 2. Do Chemistry: NaHCO3 (s) + H+ (aq) Na+ (aq) + H2O (l) + CO2 (g) 3. Capture Liberated Gas and Measure its volume, vCO2 P v = n R T to get number of moles of CO2 nCO2 = P vCO2 / RT 4. Use Ideal Gas Law

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5. From the Stoichiometry of the reaction, get moles, of NaHCO3 nNaHCO3 = nCO2 6. From number of moles, get weight wNaHCO3 = nNaHCO3 * 84.0 g / mol 7. Compute Percent Composition of Sample PctNaHCO3 = 100 * wNaHCO3 / wSample
But - it Involves Some Important Concepts Limiting Reagents Gas Mixtures – Partial Pressure Gas Solubility – Henry’s Law Departure of CO2 from Ideality Reproducibility

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The Basic Experimental Arrangement NaHCO3 HCl Syringe
Suppose the unknown is 100% NaHCO3 You are asked to weigh ~ 0.2 g of the unknown. What is the maximum volume of CO2 we can expect? ( with P = 1.0 atm and T = 25oC = 298oK ) NaHCO3 (s) + H+ (aq) & Na+ (aq) + H2O (l) + CO2 (g) 0.200 g = 200 mg / ( 84.0 mg / mmol NaHCO3) = 2.38 mmol v = n R T / P = 2.98 X 0.0821 X

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## This note was uploaded on 02/01/2010 for the course CHE 133 taught by Professor Robertschneider during the Winter '08 term at SUNY Stony Brook.

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10pGasometricNaHCO3 - Gasometric Determination of NaHCO3 in...

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