PPT-Acid, Base and Buffer Arrhenius Acid base theory

Acid is defined as a substance which when dissolved in water gives hydrogen ions H Examples Base is defined as a substance which when dissolved in water gives hydroxyl ions OH Examples. of Acids and Bases. Acids are substances which produce hydrogen ions H. +. , in solution.. Bases are substances which produce hydroxide ions OH- in solution.. Neutralization . happens because hydrogen ions and hydroxide ions react to produce water.. Determination of Buffer Capacity . Purpose . Students will determine the buffer capacity of several acetic acid / acetate buffer solutions using a pH probe. . Buffers. A buffered solution is a solution that resists a change in pH.. BLB. Additional Aspects of Acid / Base . Equilibria. Use a weak acid HC2H3O2 along with a soluble salt of the acid like NaC2H3O2. HC2H3O2 – . NaC2H3O2 - . HC2H3O2 . NaC2H3O2 . Equilibrium shift?. 17.1 The Common Ion Effec t. HNO. 2. HNO. 3. Which is the stronger base?. N. O. 2. -. N. O. 3. -. Acid-Base Reactions. strong acid + strong base. strong acid + weak base. weak acid + strong base. weak acid + weak base. Extent of Weak Acid-Weak Base Reactions. Common household acids. Citric acid. Ethanoic acid. Lactic acid. Stearic acid. Acetylsailicylic Acid. Common laboratory acids. Hydrochloric acid - HCl. Nitric acid - HNO. 3. Sulfuric acid - H. MLAB 2401: Clinical Chemistry. Keri Brophy-Martinez. Terms. Acid. Any substance that can yield a hydrogen ion (H. +. ) or hydronium ion when dissolved in water. Release of proton or H. +. Base. Substance that can yield hydroxyl ions (OH. Solutions made from a weak acid plus a soluble ionic salt of the weak acid.. Solutions made from a weak base plus a soluble ionic salt of the weak base. Solutions made of weak acids plus a soluble ionic salt of the weak acid. Acid-base balance . (H. . production = loss). Normal plasma pH: 7.35–7.45. H. . gains: many metabolic activities produce acids. CO. 2. (to carbonic acid) from aerobic respiration. Lactic acid from glycolysis. Done By:. Assistant Lecturer . Zeina. . Dawood. Assistant Lecturer . Sura. . Zuhair. Assistant Lecturer . Hiba. Sabah. Buffers. :. are . compounds or mixtures of compounds that, by their presence in solution, resist changes . Learning Objectives. Describe . what is meant by acids, bases and . buffers. List . normal pH of the body fluids. . Describe . the processes involved in maintenance of normal blood pH. .. Describe . various types of acidosis and alkalosis. By. Dr. . Jamal Ahmed Abdul-Barry. . Professor in Clinical biochemistry. Buffering Systems. Buffers are aqueous systems that tend to resist changes in pH when small amounts of strong acid [H. Schedule. Intro. Why the pH value of body fluids must be “defended”. Defining pH. Logarithms . (see appendix). Acidosis and alkalosis. Biological Buffers and the Henderson-. Hasselbalch. equation. This lecture presents the basic concepts of pharmaceutical inorganic chemistry with emphasis on the description, mechanisms and uses of various pharmaceutical products which are clinically used to correct various body disorders. The major topics to be covered are acids and bases, intra and extra cellular electrolytes, the gastrointestinal agents and topical agents frequently employed in the conversion of drugs to chemical forms convenient to their product formulations.. Acid-base balance.  . * Acids are electrolytes that release hydrogen ions (H+) when they are dissolved in water.. * Bases are electrolytes are release hydroxide ions (OH-) when they are dissolved in water..