Third Weeks of Chemistry Lecture Notes

Third Weeks of Chemistry Lecture Notes - Strong acids- just...

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Third Weeks of Chemistry Lecture Notes February 5, 2008 Where do equations go to equilibrium? The following reaction delta G =s -542 kJ per mol at 298K. If I start out with a container that has a pressure of 1 atm of F2(g), at equilibrium what will the partial pressure of HF be? When H2 + F2 = 2 HF Answer= 2 atm The following reaction delta G = +740 kJ per mol at 298K. If I start out with a contain that has a pressure of 1 mole of Fe2O3, at equilibrium how much solid Fe will I have? When Fe2O3 = 2Fe + (3/2) O3. Answer= 0 atm Acids and Bases= Bronsted-Lowry Definition Acid is a proton donor (H+), Base is a proton acceptor (H+) electron acceptors and donors works too. For example Hydrochloric Acid February 7, 2008 pH slide I missed Strong Acids and Bases= “strong” means one thing. The substance dissociates 100% in water. Strong electrolytes fall apart completely. Aqueous means the ion is completely surrounded by water. Ka justs cause it is an acid still constant of equilibrium.
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Unformatted text preview: Strong acids- just memorize them= HCL Hydrochloric HBr Hydrobromic HI Hydroiodic HClO4 Perchloric All Dissociate 100% HClO3 Chloric H2SO4 Sulfuric HNO3 Nitric What is the pH of a 0.5M solution of HBr? Answer is 0.3 should have used a calculator… We can ignore the conjugate base of a strong acid. Strong acids are completely dissociated, you cannot make them go back together. For this reaction which side has a higher entropy? One molecule breaks into two so the products has higher entropy. Look at his examples in his lecture. Liquid water will dissociate only to a small extent. Kw is the water equilibrium, spontaneous dissociation of water. If something has an H+ concentration equal to an OH- concentration we have a neutral solution. If H+ is greater than OH- we have a negative solution. If H+ is less than the OH- solution we have a basic solution. Look at his example slides....
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This note was uploaded on 06/09/2008 for the course CHE 302 taught by Professor Davidvandenbout during the Spring '08 term at University of Texas.

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Third Weeks of Chemistry Lecture Notes - Strong acids- just...

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