Ch1 - mass of total solution or mixture X 100 wt% = Can...

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Quantitative Chemical Analysis Quantitative Chemical Analysis Chapter 1: Measurements Measurements
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2 * * Système International d’Unités
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5 (per molecule) § 1 Å = 100 pm 1 nm = 10 Å ………. § 1 eV/mole = 23.06 kcal/mole = 96.48 kJ/mole
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6 Concentration Molarity moles/liter of solution (temperature dependent) Molality moles/kg of solvent (temperature independent ) Formality –usedfor electrolytes moles*/liter of solution *moles = molar amount of a substance put into solution regardless of how much dissociates to ions 1.34 F HCl = 1.34 M H 3 O + + 1.34 M Cl (acid is 100% dissociated) 0.010 F CH 3 CO 2 H = 0.0096 M CH 3 CO 2 H + 0.00041 M H 3 O + + 0.00041 M CH 3 CO 2 (acid is 4.1% dissociated)
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7 Composition Percent composition : If not specified, is percent by weight (wt%) mass of solute
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Unformatted text preview: mass of total solution or mixture X 100 wt% = Can also use volume percent (vol%) (typical for gases) volume of solute volume of total solution or mixture X 100 vol% = 8 Parts-per-Million, Parts-per-Billion mass of solute mass of total solution or mixture X 10 6 ppm = mass of solute mass of total solution or mixture X 10 9 ppb = Dilute aqueous solution ~ H 2 O 1 mL H 2 O @ 4.0 C = 1.00 g 1 g / mL = 1 ppm (wt%) 1 mg / L = 1 ppm (1mg / 1000g) 1 g / L = 1 ppb 9 Dilution Molarity x Volume = moles When a solution of a given molarity and volume is diluted, the number of moles of solute present remains constant Therefore, M conc x V conc = M dilute x V dilute And, Dilution factor...
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This note was uploaded on 03/28/2011 for the course CHEM 300L at USC.

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Ch1 - mass of total solution or mixture X 100 wt% = Can...

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