be aqueous by density: lower layer removed. Upper layer placed into separate flask labeled “A” for acid extract. Lower layer placed into sep. funnel and reextracted with 15 ml 3 M HCl. Combined aqueous layers in flask A Reextracted CH2Cl2 layer containg chemicals with 15 ml 3 M NaOH. Upper layer in flask labeled “B” for base extract. Re-extract organic layer with 15 ml 3M NaOH. Combined base extracted materials in flask “B”. Saw bubbles during mixing‚ heard the evolution of gas while venting
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Name: |Date:| Exp 1: Observations of Chemical Changes|Lab Section: | Data Tables: Part 1: |Chemicals|Well No.|Observations of the Reaction| A.|NaHCO3 + HCl| H12|White and bubbled slightly and settled down to smaller smaller bubbles| B.|HCl + BTB| H11|Golden yellow; looked darker under the black paper| C.|NH3 + BTB|H10 |Dark blue| D.|HCl + blue dye| H9|Greenish color| E.|Blue dye + NaOCl| H8|Blue and lighter than NH3+BTB solution color| | with the 1 drop of HCl| H8|Turned blue green
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Heat of Neutralization for an acid-base reaction Contents: - Abstract - Introduction - Results and Discussions - Conclusion - References Abstract: In the experimental procedure we will measure the heat of neutralization when an acid and base react to form 1 mole of water. This quantity of heat is measured experimentally by allowing the reaction to take place in a thermally insulated Styrofoam cup calorimeter. The heat liberated in the neutralization reaction will
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sodium hydroxide and hydrochloric acid‚ and sodium hydroxide and sulfuric acid will be studied. Beginning Questions When will the maximum extent of the reaction occur? Which will the limiting reagent? Which of the two acid-base combinations will absorb/liberate the greatest amount of heat energy? Hypothesis When NaOH and HCl are mixed‚ the maximum extent of the reaction should occur approximately when the amount of acid is slightly higher than the base. HCl will be the limiting reagent.
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The bronsted-lowry theory is an addition to the Arrhenius theory which defines acids and bases there are many reactions that occur in solvents or without any solvents at all rather than water. The reaction between hydrogen chloride and ammonia can be used to explain it. In aqueous solution‚ hydrogen which is an acid reacts with ammonia‚ a base to form a solution of the salt: ammonium chloride. According to Arrhenius the reaction occurs between the H+ ions formed due to the ionisation of the HCl
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volume changes Chapter 16: Acid-Base Euilibrium Brønsted-Lowry acid Brønsted-Lowry base amphoteric water equilibrium constant pH pOH pH scale weak acid Ka and pKa weak base Kb and pKb oxyacids carboxylic acids polyprotic acids amines conjugate acid conjugate base pH of acidic salt solutions pH of basic salt solutions relate Ka and Kb acid strength (binary acids) acid strength (oxyacids) Lewis acid Lewis base Chapter 17: Additional Aspects
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when we use titration to neutralize a base with acid. The process of the lab was determining the volume of a solution needed to react with a given mass or volume of a sample is called titration. The equivalence point is when the same number of moles of acid and moles of base has been added. Phenolphthalein is used as an indicator because it will have a color change when the equivalence point has been reached. Procedure See AP Chemistry. Chapter 4‚ Acid-Base Reactions‚ Titration Lab for procedure
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Complexometric Determination of Water Hardness 9/12/2013 Abstract: Two sets of acid-base neutralization titrations were conducted for experimental analysis. The first set of titrations was to standardize a solution manufactured in the lab. An approximate solution of Na2EDTA of 0.004 M was titrated against a known solution of 1.000 g CaCO3/L to deter mine to exact molarity of the Na2EDTA. Ca2+ + Na2EDTA → CaEDTA + 2Na+ The second set of titrations was to use the now standardized Na2EDTA
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Chemistry 266 Dominick Armstrong 10/10/2012 Acid-Base Titration Introduction Acid and bases are two important classes of compounds that react to form a salt and water. When mixing acids and bases a precise amount of the base must be added in order to reach the equivalence point. At this point‚ one reactant has been exactly consumed by the addition of the other reactant. When performing chemical reactions chemist use a process called titration to determine the equivalence point of the
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phenolphthalein titration is “a pale pink tint that persists for 30 seconds.” It took Dr. Sweeney 24mL of NaOH to reach his endpoint. 4. HClO4(aq) + NaOH(aq) NaClO4(aq) + H2O(l) 5. This is an acid-base reaction (neutralization reaction). Neutralization reactions involve the reaction of an acid with a base to form a salt. 6. M1V1 = M2V2 (24mL)(0.040M) = (M2)(20mL) (0.96 mL*M) = (M2)(20mL) (0.96 mL*M)/(20mL) = M2 M2 = 0.048M HClO4
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