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FISIOLOGIA DEL MICROAMBIENTE CEREBRAL EDWARD JAVIER A ACERO MONDRAGON M.D.V Biol. Esp cMSc
SOLUTE PLASMA (mM OF PROTEINREE PLASMA)CSF (mM) CSF/PLASMA RATIO Na + 1531470.96 K+K+ 18.104.22.168 Ca 2+ 1.3 (ionized)1.1 (ionized)0.85 Mg 2+ 0.6 (ionized)1.1 (ionized)1.8 Cl - 1101131.03 HCO324220.92 H2PO4, HPO30.75 (ionized)0.91.2 PH7.407.33 Amino acids22.214.171.124 Proteins7 g/dl0.03 g/dl0.004 Osmolality (mOsm) 290 1.00
METABOLISMO NEURONAL Y GLIA
TRASNPORTADORES GLUT Y MONOCARBOXILATO TRANS – MCT-
PH of Weak Acids AP Chemistry Unit 9 Chapter 14. Strengths of Acids and Bases “Strength” refers to how much an acid or base ionizes in a solution. STRONGWEAK.
The reading is 7.38 mm. The reading is 7.72 mm.
A) 80 b) 53 c) 13 d) x 2 = : 10 = 3, x 3 = 309.
[H 3 O + ] Aqueous Solutions Brackets means concentration (Molarity) 1x10 -7 M neutral 1x10 -5 M 1x10 -9 M acidic = > [OH - ] acid base M
Q u a n t u m N u m b e r s M r B o h r w a n t s t o k n o w.
Atomic Radius Paper Plate Model of Carbon Blue = electrons Red = protons Black = neutrons Our scale is: 2 pm : 1 mm If the actual atomic radius of carbon.
Lecture 14. Charge balance Sum of positive charges = sum of negative charges In natural waters: [H + ]+2[Ca 2+ ]+2[Mg 2+ ]+[Na + ]+[K + ]=[HCO 3 - ]+2[CO.
Fluid, Electrolyte, and Acid- Base Homeostasis. Body Fluids Females - 55%, males -60% Interrelationship between intracellular fluid (65%), interstitial.
Periodic Properties of the Elements All Depend on energies of outermost orbitals Atomic Size Ionization Energy Electron Affinity Ion Size.
Given Connections Solution
1 Chapter 3 Electronic Structure and Periodic Law 3.6 Property Trends within the Periodic Table Copyright © 2005 by Pearson Education, Inc. Publishing.
© University of South Carolina Board of Trustees pH K a The pH of a M solution of HNO 2 is Calculate K a for the acid.
IX.Salts and Hydrolysis Salts are simply ionic compounds. Salts can be formed by: 1.A metal reacting with a non-metal. 2 Na (s) + Cl 2(g) 2 NaCl.
Acid-Base Equilibria. Arrhenius acids increase [H + ] when dissolved in water acids can be classified as monoprotic, diprotic or triprotic bases increase.
Lecture 10 Acid-Base Equilibria -II. K a = C = 0.01 M [H + ] = (10 -4 ) ½ = M pH=3 90% acid, 10% base 2 C = M ??
1 Function of the Conjugate Base The function of the acetate ion C 2 H 3 O 2 is to neutralize added H 3 O +. The acetic acid produced by the neutralization.
HSC Chemistry – Acidic Environment R Slider. * The pH of a salt depends upon the relative strength of the ions that make up the salt * Very few salts.
Soil Buffering and Management of Acid Soils. pH pH = - log (H + ) If (H + ) = 1 x mol/L (H + ) = mol/L pH = - log (1 x ) pH = - (-3)
1 Chapter 4 Atoms and Elements 4.6 Electron Energy Levels · Be · · Mg · · Ca · · Sr · · Ba · Copyright © 2008 by Pearson Education, Inc. Publishing as.
Soil Salinity Saline Soil Solution Cation Exchange and Colloidal Phenomena Mineral Weathering Boron Chemistry Irrigation Water Quality.
Electrolytes Pre lab. Electrolytes: a quick review Electrolytes form ions in solution. Ions allow water to conduct electric current Three types of electrolytes:
To calculate the new pH, use the Henderson- Hasselbalch equation: 1141.
1 Chapter 3 Atoms and Elements 3.8 Periodic Trends Copyright © 2005 by Pearson Education, Inc. Publishing as Benjamin Cummings.
6.5- The Strength of Acids and Bases. Strong acids A strong acid is an acid that reacts almost completely ( >99%) with water to form hydronium ions HCl.
1 Acid-Base Reactions Chapter Acid-Base Reactions Reactions always go from the stronger A-B pair (larger K) to the weaker A-B pair (smaller K).
Acids and bases, pH and buffers Dr. Mamoun Ahram Lecture 2.
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Acid/Base Chemistry Part II CHEM 2124 – General Chemistry II Alfred State College Professor Bensley.
Salts product of neutralization reaction 1.00 M NaOH mol OH - L mol1.00 mol L x L x = 0.075L H+H+ + Cl - + Na + + OH - H2OH2O+ Na + + Cl - NaCl.
Oxygen transport by the blood O2 in physical solution O2 in physical solution The O2 in physical solution determines the PO2 in the blood and therefore.
Determining the Strengths of Acids and Bases Objectives: 1. Define the term dissociation constant and explain what it indicates about and acid or a base.
Acetic Acid (HC 2 H 3 O 2 ) has 0.767% dissociation in a 0.300M solution at 25°C. Find the Ka for acetic acid at 25°C and the solution’s pH.
Equine Pathology. Normal equine RBC Equine erythrocytes are about the same size as feline erythrocytes and, similarly, lack central pallor Blood from.
Dr Fatahiya Kashif The Cell. Dr Fatahiya Kashif The Cell.
HAVE A GREAT BREAK! REMINDER: NO LAB Announcements.
Wed / Thurs May 13 Objective: Write the dissociation equation for any acid or base. Checkpoint: – You have 1 L of a 2.0 M solution of KOH. How many mL.
Acids and Bases (Chapter 19): Properties of acids: Taste sour React with metals to form hydrogen gas React with carbonates to form CO 2 gas Form electrolyte.
Strengths of Acids and Bases SCH 11U. Ionization Acid molecules ionize in water; the neutral molecule breaks apart into charged ions HCl H + + Cl –
Dr. Saidunnisa Professor Of Biochemistry Acid-Base regulation.
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Regulation of [H + ] Acid-Base Physiology.. pH vs [H + ]
Review Chapter 19 1.According to Arrhenius, what are the characteristics of acids and bases? ans: acids produce H + and based produce OH - 2.What type.
Acids Lesson 2 Acid and Base Properties. Properties of Acids Neutralize bases Are electrolytes that conduct electricity React with metals such as Mg and.
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Lecture 15 10/05/05 Research Club. What is the charge and mass balance for 0.l5 M phosphoric acid Charge balance: [H + ] = [H 2 PO 4 - ] + 2[HPO 4 -2.
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Created with MindGenius Business 2005® Ion Exchange Chromatography Ion Exchange Chromatography Principles Small K means low affinity – so low RT K is often.
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