Lecture 7 post

# Lecture 7 post - Oxyacids REMEMBER, Anion Suffix -ite -ate...

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Oxyacids REMEMBER , Anion Suffix Acid Suffix -ite -ous - ate -ic Oxoanion Oxoacid CO 3 2- Carbon ate ion H 2 CO 3 Carbon ic acid NO 2 - Nitr ite ion HNO 2 Nitr ous acid NO 3 - Nitr ate ion HNO 3 Nitr ic acid ClO - Hypo chlor ite ion HClO Hypo chlorous acid ClO 4 - Per chlor ate ion HClO 4 Per chlor ic acid

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Percent Composition Percentage of each element in a compound By mass Can be determined from 1. the formula of the compound 2. the experimental mass analysis of the compound The percentages may not always total to 100% due to rounding 100% whole part Percentage × =
Example 3.13 – Find the mass percent of Cl in C 2 Cl 4 F 2

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Example 3.14 – Find the mass of table salt containing 2.4 g of Na
Finding an Empirical Formula 1) convert the percentages to grams a) assume you start with 100 g of the compound b) skip if already grams 2) convert grams to moles a) use molar mass of each element 3) write a pseudoformula using moles as subscripts 4) divide all by smallest number of moles a) if result is within 0.1 of whole number, round to whole number 5) multiply all mole ratios by number to make all whole numbers a) if ratio 0.5, multiply all by 2; if ratio 0.33 or 0.67, multiply all by 3; if ratio 0.25 or 0.75, multiply all by 4; etc. b) skip if already whole numbers

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Laboratory analysis of aspirin determined the following mass percent composition. Find the empirical formula. C = 60.00%
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## This note was uploaded on 05/20/2008 for the course CHEM 115 taught by Professor Larkin during the Spring '08 term at Bloomsburg.

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Lecture 7 post - Oxyacids REMEMBER, Anion Suffix -ite -ate...

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