Herschel Walker’s Victory over D.I.D. Micah Holtgraves Ivy Tech Community College PSYC101-HAF September 27‚ 2012 Herschel Walker was one of the most important running backs in NFL and college history. Because he contained great speed and strength‚ he soon became one of the greatest football players of all time. In 1982 at the age of only 20‚ he became the Heisman trophy winner (Brown‚ 2009). He went on to play 15 years of professional football. This was all before he became diagnosed with
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"Jesus Christ‚ what in the fuck did you do to my face? Where the fuck is my face" (Identity) the main actor in the movie Identity by Columbia Pictures presenting a Konrad Pictures production a film by James Mangold. and shows his discomfort and his misunderstanding of what is going in his life when he is face to face with many lawyers and a judge; along with the Doctors trying to convince them that this man is not the killer of the people‚ but instead that was just one of his identities that should
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In the Faces of Eve‚ the main character‚ Eve experiences episodes of Dissociative identity disorder. However‚ in the film‚ she was diagnosed with its former name multiple personality disorder. Faces of Eve is based on a true story of women in the 1920s to 50s who had at least 3 different personalities that would come with certain triggers. Someone diagnosed with Dissociative identity disorder is the presence of two or more distant personality. Each personality has it own name and characteristics
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The purpose of the Weak Acid Dissociation experiment is to determine the dissociation constant of a weak acid experimentally by using acid-base titration with a strong base and stoichiometry. An acid-base titration is a method by which a basic (or acidic) solution of unknown concentration is reacted with an acidic (or basic) solution of known concentration. (1) The pH in acid-base titration is measured using a pH meter or color changing indicator‚ such as phenolphthalein‚ as the known solution is
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E r J. Biochem. 40‚177-185 (1973) u. Intracellular Titration of Cyclic AMP Bound to Receptor Proteins and Correlation with Cyclic-AMP Levels in the Surviving Rat Diaphragm Lien DO KHAC‚Simone HARBON Hubert J. CLAUSER and lnstitut de Biochimie‚ Universit6 de Paris-Sud‚ Orsay (Received April 9/July 17‚ 1973) Extracts prepared from rat diaphragms incubated with or without theophylline and/or epinephrine have been tested for their total cyclic AMP content and for their ability to bind exogenously
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Ka‚ Acid Dissociation Constant and Kb‚ Base Dissociation Constant (Lesson Recap) Ka‚ Acid Dissociation Constant Ka- is the Keq for the dissociation for a weak acid. e.g Acetic Acid‚ when dissolved in H2O CH3COOH (aq) + H2O (l) (ACID) (BASE) CH3COO (aq) + H3O(l) (CONJ BASE) (CONJ ACID) CH3COOH (aq) + H2O(l) ↔ CH3COO (aq) + H3O(l) *ONLY weak acid and back can be reversible Equation for Ka : Keq= [CH3COO(aq)] [H3O(l)][CH3COOH(aq)] [H2O(l)] Keq x [H2O
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= 55.56 M K = 1.8 x 10-16 ; pKa = 15.74 pKa is the acid dissociation constant; low pKa (strong acid‚ high pKa (weak acid we can also write Kw = [H3O+][OH-] Kw = 10-14 In water‚ pH + pOH = 14 pH scale Strong Acids: Complete dissociation of the acid in water: HA ( H+ + A- note: H+ in H2O is hydrated (H3O+) K (Ka since it is an acid) is large (For complete dissociation‚ K = infinity; however there is some very tiny amount that is not
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Acid Rain Introduction: Titrations are often recorded on graphs called titration curves‚ which generally contain the volume of the titrant as the independent variable and the pH of the solution as the dependent variable (because it changes depending on the composition of the two solutions). The equivalence point on the graph is where all of the starting solution (usually an acid) has been neutralized by the titrant (usually a base). One can easily find the pKa of the monoprotic acid by finding
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gradually neutralizing the acid. The volume of base added can be determined by the difference in the initial and final volume marks on the buret. At a certain volume of added NaOH‚ all the KHP acid will be neutralized due to the large equilibrium dissociation constant (Kb) of the base. This point of titration is referred to as the equivalence point. Considering the 1:1 stoichiometry of this acid-base reaction NaOH(aq) + C6H4(COOH)(COOK) (aq) C6H4(COONa)(COOK)(aq) + H2O(l) the point of equivalence
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the acid dissociation constant (Ka) for the weak acid HX in aqueous solution is 3.01 × 10–5 mol dm–3. (i) Calculate the value of pKa for HX at this temperature. Give your answer to 2 decimal places. ............................................................................................................... ............................................................................................................... (1) (ii) Write an expression for the acid dissociation constant
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