Week 5 - Chapter 4
Week 5 - Chapter 4 CHEM 1311
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This 3 page Class Notes was uploaded by carolyn martinez on Sunday October 9, 2016. The Class Notes belongs to CHEM 1311 at University of Texas at Brownsville and Texas Southmost College taught by Vanessa Garcia in Fall 2016. Since its upload, it has received 5 views. For similar materials see General Chemistry I in Chemistry at University of Texas at Brownsville and Texas Southmost College.
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Date Created: 10/09/16
Week 5 – Chemistry I Soluble compounds are compounds that when mix well dissolve and become part of the aqueous solution Insoluble compounds are compounds that when mix will not dissolve and create a precipitate, AKA a solid. Methatheis Reactions (Double displacement reaction) is where a precipitate can occur. AB + CD AD + CB HOW TO CREATE AND BALANCE THIS REACTION: Cn help determine what ions are present 1. Write the formula (Nomenclature rules) 2. Define what state the elements/ compounds are and their solubility 3. Balance 4. This is where you predict the product form, equation given above helps you in finding out. Net Ion Equations are ions and molecules that are involved in a reaction. 1. Write the equation 2. Balance 3. Rewrite the equation, in this case, write the electrolyte and their formation of ions 4. Cancel and identify “spectator” ions Acid- Bases Reactions - + Bronsted acids donate protons look like H acids form H when dissolved in water Bronsted bases accept protons look like OH when dissolved in water. + Monoprotic acid -> one proton to donate HCl and HNO – yiel3 one H Polyprotic donate multiple protons Acid- base reactions acid donates a proton and base accepts the proton = neutralization reaction Neutralization reactions have no acidic or basic properties in the product. To create a salt, you need a ionic compound of cat ion form a base and a anion from an acid. Oxidation- Reduction Reaction = Redox reactions both need to happen in order for the reaction to work. The reaction is where electons transfer from one to another. O XIDATIONLOSESR EDUCTION GAINS Oxidation numbers Loses and gains of electrons Neutral Atom has an oxidation number of zero. Oxidation increases then it loses electrons;lost e- Oxidation number increases it gains electrons gained e- Oxidizing agent is the factor of an element to be oxidized Reducing agent is the factor for a element to be reduced Half reactions are used to balance a redox reaction; electrons must equal the electrons gained 2+ 3+ Example: when Sn and Fe react, Sn +2(aq) + 2 Fe +3 (aq) --> Sn +4 (aq) + 2 Fe +2(aq) +2 +4 - Oxidation: Sn +3q) --> Sn - (aq) + 2+2 Reduction: 2 Fe (aq) + 2e --> 2 Fe (aq) Single Displacement: An oxidation of an element Example: Mg (s) + 2 HCl (aq) --> MgCl (aq)2+ H (g) 2 FIinding molarity: Concentration of a solution Molarity: Molesof solute volumeof solution∈liters Example: What is the molarity of a solution containing 0.32 moles of NaCl in 3.4 liters? 0.32 moles NaCl Molarity = = 0.094 M NaCl 3.4 L Molarity = moles volume Moles (mol) = volume x Molarity moles Volume = Molarity Finding the molarity of a new diluted solution M 1 1 =M 2 2 M 1nd V re1resent the concentrated solution while M and V re2resent2the diluted solution
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