the pH level was used to determine which solution it was. The pH scale is 1-14‚ a pH of 7 is neutral‚ less than 7 is acidic‚ and greater than 7 is acidic. Materials: * pH strips * 20 test tubes * Disposable transfer pipettes * Indicators * Methyl Orange * Bromocresol green * Bromocresol purple * Phenol red * Solutions included * Bleach * Lemon juice * Lemon-lime soda * Baking soda solution * One unknown Procedure:
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while in the Phase 1 lab environment. Section 1: You will be testing 4 known solutions for pH levels using a standard wide-range indicator. Based off of the results obtained in the lab room‚ fill in the following table: How many drops of wide range indicator will you use for each test‚ based on industry standards such as the LaMotte field test? One drop per indicator. |Solution Number |pH from Lab |Acid or Base? |Solution Name (from Lab results)
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Part A. Acid-Base Indicators Purpose In this part of the experiment‚ we will find a reagent that will shift the acid-base equilibrium reaction described by Equation (2) in one direction and then a second reagent that will cause the equilibrium position to shift back in the opposite direction. Introduction An acid–base indicator is a substance that changes color as the pH of a solution changes. Consistent with LeChâtlier’s principle‚ if a solution containing the indicator becomes acidic (e
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De Leon‚ Jo-Anna Maria N. 3ChEA Group No. 2 Experiment No. 5 Spectrophotometric Determination of pKa I. Introduction The equilibrium constant of the dissociation of an indicator in water will be determined experimentally using spectroscopic method.This experiment aims to demonstrate the principle of equilibrium and the interaction of matter with light. II. Methodology Figure . UV-VIS Spectrophotometer 10 solutions covering the entire pH range from 1 to 13 were prepared
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Method: First the calibration was completed using an approximately .7340g Na2EDTA/500mL solution. A 1.000g/L calcium ion solution was used as the primary standard with approximately 3mL of ammonium chloride as a buffer and Erichrome Black T as the indicator solution. Three titrations were performed to ensure accuracy of the molarity of the Na2EDTA solution. The 1.000g/L calcium ion solution had to be converted to M so 1g/L/100.1g=.009990M calcium ion solution. Titration 1: 10.00mL CaCO3; .00999MCaCO3X
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base titration means that by using neutralization between acid and base. Abrupt changing of pH says whether procedure is done or not. pH indicators are tools for determining neutralization is reaching end point. When reaction reaches equivalent point‚ one of species‚ titrant or analyte is used up completely and there is no more neutralization. But By pH indicator‚ there is very few possibility to distinguish equivalent point. When‚ neutralization reaches at that point‚ changing pH is too sensitive
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duplicate ~0.15 g samples of previously dried standard Na2CO3 Dissolve samples in ~100-ml distilled water; if it does not dissolve quickly‚ you may warm the solution. 2 - Cool the solution to room temperature and add ~ 0.5 to 1 ml of bromocresol green indicator‚solution turns into blue. Titrate it with HCl until green color is reached. (DO NOT OVER TITRATE) 3 - Heat and boil out CO2gently. You should obtain a blue color again at the end of this step. Cool to room temperature‚ and continue titration until
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that the lower the Ph levels where the more off the milk would be. Equipment * Off full cream P ura milk- had been left out in sun for a week * Fresh full cream Pura milk * Litmus paper * Beaker * Test tubes * Universal indicator Method 1. Put off milk and fresh milk into two separate beakers 2. Pour a small sample of fresh milk into a test tube 3. Pour a small sample of off milk into a new test tube 4. Dip litmus paper into each of the test tubes and remove
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| Gram Negative Unknown | Biology 3444-006 | | Lena Wallace | 11/7/2011 | | Abstract: The purpose of this lab was to identify an unknown bacteria culture using differential tests. The identification of the unknown culture was accomplished by identifying the bacteria based on its specific metabolic characteristics and morphology. It is suggested that culture 11 is a sample of Enterobacter aerogenes. Introduction: This experiment was centered on metabolic and biochemical testing
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1:1 titration. One mole of base will titrate one mole of acid. The endpoint of the titration will be determined by an indicator‚ phenolphthalein. Phenolphthalein is a weaker acid than KHP. It is colorless under acidic conditions and changes to a pink color under basic conditions. Therefore‚ the first persistent presence of color indicates that it is beginning to titrate the indicator and have reached the endpoint; if the solution changes to a dark pink color‚ the solution has overshot the endpoint
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