| What is observed | 1. Started with copper‚ Cu (s). | reddish‚ brownish‚ orange-ish‚ powder-like | 2. Added nitric acid‚ HNO3 (aq). | acid turns blue and smells like chlorine. | 3. Added water‚ H2O (l). | stayed the same | 4. Added sodium hydroxide‚ NaOH (aq). | changed consistency‚ gel-like | 5. Heated the mixture | becomes darker‚ dark-brown-like‚ shavings | 6. Filtered the solid and added sulfuric acid‚ H2SO4 (aq)‚ to it. | sulfuric acid cleans off the copper | 7. Added zinc
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the cation of the base mixes with the anion from the acid‚ forming a base‚ and the hydrogen from the acid mixes with the anion from the base‚ forming water. In this reaction‚ the sodium ion from the sodium hydroxide attracts to the acetate ion from the acetic acid‚ and the extra hydride ion bonds with the negative hydroxide ion to form water. The water produced by the reaction had a pH of seven‚ and so when the whole solution was light pink‚ we knew the reaction had fully
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in vinegar by titration with a standardized sodium hydroxide solution. The experiment is divided into two parts where the first one is to prepare standardizing sodium hydroxide solution which will be titrated to potassium hydrogen phthalate‚ solution and the second one is determining the molarity and percentage by mass of the acetic acid in vinegar. 6 g of NaOH solid is used to dilute with distilled water to prepare a 250 mL of 0.6M sodium hydroxide. pH electrode will be immersed into the solution
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Experiment three was divided into three parts; the preparation of the solutions‚ the reaction between Hydrochloric Acid and Ammonium Hydroxide (part b)‚ and the formation of Magnesium Oxide (part c). 200 mL of deionized water were added to a beaker followed by the addition of 100 mL 6 M HCl‚ which reacted to make 300 mL of a 2 M HCl solution used for Part B. Next‚ 50 mL of deionized water were added to a separate beaker and then 100 mL 3 M NaOH were added to the beaker to form 150 mL of a 2 M NaOH
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Experiment 3: ANALYSIS OF UNKNOWN ACID SAMPLE USING TITRATION METHOD Date of Experiment: 4 September 2012 Introduction An acid-base titration is a procedure used in quantitative chemical analysis to determine the concentration of either an acid or a base. Titration is the slow addition of an acid (or a base) of known concentration from a burette (a narrow graduated cylinder) to a base (or an acid) of unknown concentration fin an Erlenmeyer
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Introduction There are three main theories surrounding acids and bases including the Arrhenius‚ Bronsted-Lowry‚ and Lewis theories. The Arrhenius theory of acids and bases states that acids produce hydrogen ions (H+) in solution while bases produce hydroxide ions (OH-) in solution. Arrhenius was able to determine his theory based on his prior knowledge of the behaviour of substances in aqueous solution. Arrhenius went further to describe strong acids as a strong electrolyte that was able to ionize completely
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differences. Apparatus: Test tubes Measuring cylinders Wooden splinter Test tube rack Thermometer Glass rod Materials: Sodium peroxide Silicon (IV) oxide Universal indicator solution Magnesium oxide Phosphorus pentoxide Litmus paper Safety measurements: Safety spectacle **Warning: Phosphorus (V) oxide is corrosive and irritates eyes‚ skin and lungs. Sodium peroxide is also corrosive and a powerful oxidant. Procedure: Part A: Appearance: Examine your oxide samples‚ and in Table
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cleaners and rust removers. A variety of maintenance chemicals contain these compounds. Alkali maintenance chemicals like degreasers‚ oven cleaners and drain openers contain bases such as Sodium Hydroxide (NaOH)‚ Potassium Hydroxide (KOH)‚ Sodium Metasilicate (Na2SiO3)‚ Ammonium Hydroxide (NH3(aq)). Special salts like Sodium Lauryl Sulfate‚ ammonium ethoxysulfate are formulated into carpet shampoos‚ hand soaps and carwash detergents to provide more efficient cleaning. What is a pH buffer? A buffer is a
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Determining the Molarity of Acetic Acid in Vinegar Abstract This experiment was done to determine the molarity of acetic acid in vinegar. The acetic acid in vinegar was titrated with a strong base sodium hydroxide to determine the equivalence point of this chemical reaction. The indicator phenolphthalein was used because the moment it changes color is on the basic side of the pH scale. To insure the experiment was done with the most accuracy‚ the two conductors of this experiment took three
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aqueous and organic layers thoroughly during the NaHCO3 extraction would lead to little to no production of aspirin precipitate. The aqueous layer contains sodium hydroxide and water‚ whereas the organic layer contains the dichloromethane‚ aspirin‚ and the unknown. If the HCl has nothing to react with in the aqueous layer following mixing (i.e.‚ sodium acetylsalicylate)‚ then little to no solid aspirin will be produced. Furthermore‚ more unknown would be produced than expected because aspirin would precipitate
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