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Week of October 26

by: Notetaker

Week of October 26 Chemistry 100

Default_profile Notetaker
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Preparatory Chemistry
Dr. Ronald See

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The end of Chapter 3 (Ion Concentrations in Solutions, How to Find Concentration of an Ion in a Solution, and Solution Stoichiometry) and the beginning of Chapter 4 (Precipitation Reactions)
Preparatory Chemistry
Dr. Ronald See
Class Notes
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This 3 page Class Notes was uploaded by Notetaker on Thursday October 29, 2015. The Class Notes belongs to Chemistry 100 at Indiana University of Pennsylvania taught by Dr. Ronald See in Fall 2015. Since its upload, it has received 15 views. For similar materials see Preparatory Chemistry in Chemistry at Indiana University of Pennsylvania.

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Date Created: 10/29/15
Week of October 27 2015 End of Chapter 3 and Beginning of Chapter 4 1 Ion Concentration in Solutions a Ionic compound salts strong electrolytes only dissolve as ions in water b Dissociation reaction shows how solid saIt dissolves into ions in aqueous solution i Watch for single atom and polyatomic ions c Examples i CaC2 sCa2 2Cl39 not C239 ii Na2504 2NaSO4239 iii Mg3 PO42 3Mg22PO4339 2 How to Find Concentration of an Ion in Solutions b Examples i What is the concentration of chlorate ion in a solution made with 575g of CaCO32 diluted to 725 ml ii 575g CaCO322071 gmo 00278 mol 1 2071 gmoMoar Mass of CaCO32 iii 725 mL 1L1000mL 725 L iv 00278 mo725 L 00383 M CaCO32 v CaCO32l Ca22 CO339 dissociation reaction vi M of CO3 00383 2 00766 M CIO3 3 Solution Stoichiometry a Given amount or unknown may be expressed as molarity b Use molarity equation MmolL to convert solutions to moles or vice versa c Example i Based on the reaction 2H202 ag 2 H20I 02 g what mass of oxygen gas can be produced from 125mL of 182 M H202 solution ii MmolL182 M xmo125Lx182molL125L 1 X0228 mol H202 iii 1 mol 022 mol H202x moi0228 mol 1 X1228mo2114mo 02 iv 0114mol 02 320g1 mol365g 02 1 320gMoar Mass of 02 Chapter 4 Precipitation Reactions 1 Solubility of Ionic Compounds a Ionic compound salt strong electrolytes dissolve in water only as ions i Dissociate in positive and negative ions ii Occurs if ions are more attracted to water than each other why they dissolve 2 Solubility Rules a Some salts won39t dissolve very well in water bc they39re more attracted to each other than the water i If it does dissolve the salt is more attracted to the water b Function of chanqe attraction between negative ions and positive ions i The quotlargerquot the product of the charges the greater the attraction between ions ii Great attraction between ionslower solubility in water d Examples i NaCI 1 NaCI39 1 1 1soube ii Ca C2 1 Ca2CI391 2 1 2soube iii KNO3DK1NO339139D soluble iv CaCO3 Ca2CO3392Dinsoube 3 Writing Precipitation Reactions a Precipitation when salt solutions are mixed and new combos of positive and negative ions are possible i A solid is formed when new combo is insoluble CI8391K21H ii MgC2KzSO4D b quotNormalquot Equation write compounds and balance i All dissolved species aq ii Precipitate is a solid 5 iii MgC2 aqNa2504 aqMgSO4s2 NaCI aq c Full Ionic Equation aq solutions are really dissociated into ions making it better to write them as ions i Dissociate all aq compounds ii DO NOT dissociate solids actual compounds iii Mg2 2CI391 2NaSO4392DMgSO4s 2Na2 0391 d Net Ionic Equation ions that are unchanged are dropped from the reaction i Only has ions that combine to make precipitate ii Mg2 SO4392D MgSO4s e Example CaCIO32 and K3PO4 are mixed i Write ions ii Look for soluble combos 1 Ca2PO4393D Ca3PO42 5 iii Write and balance quotnormalquot equation 1 3Ca CIO322K3PO4Ca3 PO426KCO3 iv Write full ionic equation 1 3Ca26 CIO33916K12PO4393 CaPO426K16CO3391 v Write net ionic equation 1 3Ca22PO4393Ca3PO42


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