Acid

ids Acids, Bases, Buffers and Respiration Darlene E. McDonald WCCC Fall 2012 Ap Lab 071-07 Dr. Roxanne Levandosky August 31, 2012 I. INTRODUCTION: A.PURPOSE: a. To define and understand the key terms. ~acid ~buffer system ~base ~acidosis ~pH ~alkalosis ~pH scale ~hypoventilation ~pH indicators ~hyperventilation b. To determine the acidic or base nature and actual pH of various substances. c. To discuss the formation of the carbonic acid/bicarbonate ion

Background: Acids are known to chemistry as the chemical substances that are below seven on the pH scale and they cause litmus paper to turn red. They are also known to have a sour taste but not all acids should be tasted due to some of them being extremely dangerous and should not be in contact with human body parts. In this lab, we worked with an acid known Hydrochloric Acid (HCl). HCl is a clear liquid that visibly looks no different from water. HCl is known to be very dangerous when in contact

Abstract: In this experiment, it was attempted to purify acid phosphatase from wheat germ in its native confirmation with retention of enzymatic activity. The fraction that would contain the purified acid phosphatase (Supernatant IV), had 4.0mg of total protein, but no enzymatic activity and 0% recovery. The experiment was not successful. Acid phosphatase was not purified in its native confirmation with retention of enzymatic activity. In part 2c of the experiment, an error was made in the amount

determine the molarity of an unknown acid. Moreover, acids and bases react with the known stoichiometric ratios based on the coefficients of the balanced chemical reactions. If the stoichiometric ratio of an acid-base reaction is known the unknown concentration can be determined, however the reaction must have gone through completion and the number of moles of one of the components needs to known. The pH scale can be used to determine the change in concentration of an acid or base. The pH scale is calculated

that a strong acid that is titrated with a strong base will produce a resultant solution has a pH that is slightly over 7. This is because strong acids have a lower pH and solutions that are less basic than weak acids that have been titrated with strong bases. When a weak acid is titrated with a strong base it will produce a resultant solution that is well above 7 because it starts off with a higher pH. Acids and bases with high concentrations result in large changes in pH, while acids and bases with

concentration of NaOH was used to identify the unknown acids, this value is shown is experiment 16.1. This mean standardized concentration was 0.0784 M. By titrating a known amount and concentration of this standardized base to the unknown acid, a titration curve and its derivative could be plotted in order to find the molar mass and acid dissociation constant. The first unknown acid titrated, BGYW, was identified to be Maleic acid, C4H4O4. The identity of the acid was found by taking both the molar mass and

Patterns: The lower a metal is in its group the faster the reaction it will have with water. This is true for both group 1 and group 2. The metals reacted to form Hydrogen gas and a solution that was alkaline. When going down a group the Electronegativity decreases which results in the element losing their valence electrons easier, making them react more quickly. The group 1 elements had similarities in their appearances, Potassium and Lithium were in a cylinder shape, but sodium was white and had

In the lab experiment called Acids and bases; the lab was design for participant to figure out whether certain household chemicals are acids or base and what color they can turn in to when being added to cabbage juice. An acid are a solution that has lose hydrogen ions that usually taste sour. However, some household solutions are acids such as vinegar and citrus fruit juices. Bases are solution that pull hydrogen ions out of solution and into themselves and it usually feels slippery. In this experiment

(a) When dry pH paper was placed over household ammonia, the paper quickly turned a dark blue, indicating that it was a base. (b) When moist pH paper was placed over household ammonia, the paper turned dark blue faster than when dry, still indicating that it was a base. (c) When pH paper was placed over bleach, the paper turned blue, which indicated that it was a base. (d) When pH paper was over ammonium carbonate, the paper turned dark blue even faster than the moist paper over household ammonia

The purpose of this experiment was to test acid-base solutions to determine the absorbance intake they had do to their different pH levels. To do this, four similar samples were recorded with a different amount of NaOH added to each one, which would change the pH level from acidic to basic. Acidic solutions take in less absorbance, while basic solutions will have the most absorbance, as well as higher Ka and pKa values. The acidic solutions would have negative absorbance from 100% or higher transmittance