1. Identify the functional group or molecule for each of the following. (3 points) 1. COOH -OH 2. COH -OH 3. COH -OH 1. List whether each of the following substances was positive or negative for reducing sugar‚ as indicated by the Benedict’s test. (6 points) 1. corn syrup (1 point) positive 2. table sugar (1 point) positive 3. unknown 1 (1 point) negative 4. unknown 2 (1 point) negative 5. unknown 3 (1 point) positive 6. unknown 4 (1 point)
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Name Lab Partner Name(s) Thermodynamics‚ Enthalpy of Reaction Lab March 27‚ 2014 I. Purpose The purpose of this lab is to learn how to determine the heat of reaction. II. Safety 1. Wear appropriate safety attire (goggles‚ aprons‚ hair tie‚ etc.). 2. Do not directly inhale or ingest chemicals. 3. Understand safety information regarding the chemicals being handled during the lab (hydrochloric acid‚ sodium hydroxide). 4. Be aware of how to operate all lab equipment. 5. Clean hands
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In the experiment‚ we tested a sodium chloride solution. Along with the tested solution‚ control groups (water and sodium phosphate) were used to be help understand whether or not NaCl was a buffer. Water was the negative control group and sodium phosphate was the positive control group. If NaCl was a buffer than the pH would be stabled as the sodium phosphate buffer. If NaCl was not a buffer than the pH would fluctuate like the negative control‚ water. During the first trial and prior to the drops
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SODIUM DISORDERS * Identify specific types of hyponatremia and hypernatremia using diagnostic criteria and assessment questions * Hyponatremia * Mild: 125-130 * Nausea‚ Malaise * Moderate: 115-125 * HA‚ Lethargy‚ Restlessness‚ Disorientation * Severe: <115 * Seizures‚ Coma‚ Resp/Brainstem damage * Hypernatremia * Mild: 145-160 * Asymptomatic * Moderate: 160-180
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difference in the amount of calcium carbonate in brown versus white chicken eggs. Background: Calcium carbonate (CaCO3) is a component of seashells and eggshells that gives them their strength and hardness. Because calcium carbonate is a base‚ it will react with acids to form a salt and water. The complete reaction of calcium carbonate with hydrochloric acid is: CaCO3 (s) + HCl (aq) ( CaCl2 (aq) + CO2 (g) + H2O (l) The portion of the shell that is not calcium carbonate does not react with acid and
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Hydrogen peroxide and iodide ions Aim: To determine the rate equation for the reaction between Hydrogen peroxide and iodide ions‚ and to investigate the effects of a catalyst and temperatures on the reaction and to derive the activation enthalpy. Background knowledge: 1Hydrogen peroxide reacts with iodide ions producing iodine‚ when in an aqueous acid solution. H2O2 (aq) + 2I- (aq) + 2H3O+(aq) I2 (aq) + 2H2O(l) To detect iodine you can look at the color shown by the addition of starch
Free Chemical kinetics Chemical reaction Reaction rate
SCH 3U0 May 7th 2013 Percent Yield of Calcium Carbonate Introduction: The purpose of this experiment is to examine the percent yield of a precipitate in a double displacement reaction. A solution of calcium citrate and sodium carbonate were mixed together‚ then the products were filtered out as so only the precipitate remained. The filtered paper was then dried and the mass of the precipitate in the experiment divided by the theoretical mass of the precipitate from the calculated gave the
Free Stoichiometry Chemical reaction Sodium
2. An aqueous solution of KCl is colorless‚ KMnO4 is purple‚ and K2Cr2O7 is orange. What color would you expect of an aqueous solution of Na2Cr2O7? Explain. Orange. 3. Explain why hexane will dissolve benzene but will not dissolve sodium chloride. Sodium chloride is an ionic compound. 4. Some drinks like tea are consumed hot or cold‚ whereas others like Coca-Cola are consumed only cold. Why? For taste reasons‚ these drinks can be drunk if the user likes It but having coca cola like tea
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Prior to begin the experiment‚ preparation for some solutions is required to enhance the lab performance. The solutions needed are standardized potassium bromate‚ standardized sodium thiosulfate‚ and starch indicator. First‚ to prepare a starch indicator‚ pulverize 1g of soluble starch and add 15mL of water to make it as a paste-like substance. Dilute it with about 500mL of boiling water‚ and continue to heat until the mixture becomes clear. Cool it to room temperature and save it into a stoppered
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rebound"‚ a condition whereby the gastric acid returns in greater concentration after the drug effect has ceased. Moreover‚ this class of antacids is not suitable for all patients owing to its components. For example‚ the usually high concentration of sodium bicarbonate present in these chemical antacids may be inappropriate for patients afflicted with hypertension or kidney failure. Non Absorbable Antacids The non-absorbable antacids though less prone to cause a rebound effect‚ have their fair
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