Aqueous Solutions, Acids, and Bases: Lecture 3
Aqueous Solutions, Acids, and Bases: Lecture 3 Biol 1107
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This 2 page Class Notes was uploaded by Amanda Notetaker on Wednesday September 9, 2015. The Class Notes belongs to Biol 1107 at University of Connecticut taught by Thomas Abbott in Summer 2015. Since its upload, it has received 26 views. For similar materials see Principles of Biology I in Biology at University of Connecticut.
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Date Created: 09/09/15
Aqueous Solutions Acids and Bases Lecture Notes 0 Basic solution 0 concentration of 0H hydroxide ions molecules is higher than that of H30 hydronium ions 0 changes physical and chemical properties of water 0 Alkaline o solute adds more 0H ions that can be bonded to H ions lowering the concentration of hydronium ions raising pH 0 not being removed from the solution so pH elevates o solute adds more H protons if not removed pH lowers in solution 0 weak acids gt do not readily give up all H ions into solution I carbonic acids used as a buffer in our blood because it doesn t readily give up H transport C02 in respiration back out from cells into environment 0 strong acids gt do readily give up all H ions I think courageous willing to go it alone without Hs strong I stomach uses HCI because it very readily gives up H pumps up acidity in stomach acids to break down food 0 The pH scale 0 xray crystallography atomic accelerators mass spectrometry are use to detect individual atoms 0 logarithmic scale makes it easier mathematically and to detect larger measures in pH to represent at the smaller level 0 How do you know not based on number gt OH concentration would be 10 4 M if H is 10 10M then it is basic OH concentration is larger 0 Sea water is basic gt hydrogen ions being removed carbonate present 0 Buffers stabilize pH 0 average pH in human blood is 74 if it drops to 72 you die 0 carbonic acid is used to offset this change and constantly balance human body 0 various environments in the cell need various pHs I Lysosome breaks down substances slightly acidic I Mitochondria slightly basic for respiration o removing H behaving as buffer gt is reversible especially in red blood cells 0 C7H16 valence electrons would be in between the bonds because they have relatively equal electronegativity I electronegativity attractive forces within the nucleus are relatively equal 0 Number of protons the more you have the more you can attract influences electronegativity o 4 orbitals in 2nd shell each holds 2 electrons o causing shielding which affects electronegativity o Harnessing energy o Septane has more bonds therefore contains a greater source of energy more potential energy stored than LAlanine 0 THE LIVING CONDITION transferring or transforming energy I This is how we LIVE how we have grown and evolved throughout time o Arrangement I shape determines function some encourage a certain chemical reaction some may discourage that same chemical reaction I adding a double bond allows molecules to create more isometric possibilities but they can t rotate around one another I some right handed amino acids will help establish certain structures Notes to be continued NEXT WEEK
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