dissolved and record the highest temperature reached. Data and Observations: CALORIMETRY LAB PART ONE | | Distilled water volume | 205ml | Constant initial temperature | 24.5 degrees C | NaOH mass | 2.535g | Final temperature | 27.8 degrees C | PART TWO | | HCL solution | 105ml | NaOH solution | 105ml | Initial HCL temperature | 25.2 degrees C | Mixed solution temperature | 28.2 degrees C | | In the lab‚ it was hard to get the measurements of the liquids exact‚ so they
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words Observations: (This part is to be completed in class) Part 1: Physical Change- Heat of Solution for Sodium hydroxide (NaOH) 3.2 grams NaOH Result: Temperature of DI water = ____22.8 °C Temperature after addition of NaOH = ______31.8 °C Part 2: Chemical Change- Reaction between acid and base Result: Temperature of HCl = ___21.4 °C Temperature after addition of pellets of NaOH = ____26.4 °C Part 3: Chemical Change- Reaction between stomach acid and antacid Result: Temperature of HCl = __23.3 °C
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__ MATERIALS AND PROCEDURE As per Essential Experiments for Chemistry pages 163–170 RESULTS TABLE 1 Equilibrium involving bromocresol green Initial colour of bromocresol green in water = Reagent added HCl (step 3) more HCl (step 4) NaOH (step 5) more NaOH (step 6) Stress Colour change and # of drops required Direction of shift ver. 02/2012 1 Chemistry 12 Unit 2 Reaction Equilibrium TABLE 2 Equilibrium involving iron(III) thiocyanate ion Colour of FeCl3
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Determination of Percent Potassium & Percent Iron in an Iron Oxalate Salt by Ion Exchange Introduction: This experiment involves determining both the percent potassium (K) and iron (Fe) in a single titration after passing a solution containing a known mass of complex salt through an ion exchange column. Ion Exchange: Certain materials called ion exchange resins consist of rather large molecules which contain ions that can be displaced. The resins are solids‚ insoluble in water‚ usually granular
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Title: Study of Solubility Equilibrium Abstract The effect of temperature on the solubility product constant‚ Ksp‚ of potassium hydrogen tartrate in water was investigated in the temperature range of 285K to 318K at normal atmospheric pressure. It was found that the solubility of potassium hydrogen tartrate decreases with a decrease in temperature and consequently a smaller volume of sodium hydroxide is needed to neutralize it. The molar solubility of potassium hydrogen tartrate was calculated
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filtered solution. It was titrated with 0.1M NaOH until its color turned pink. The procedure was repeated for the second trial. The second part of the experiment was acquiring the pH of solutions using calorimetric measuring tools. First is by using pH paper. The pH paper was dipped into the ten drops of 0.1M HCl then read the pH using the chart. The procedure was repeated using 0.1M NaOH‚ 0.1M CH3COOH‚ and 0.1M NH4OH. Next‚ the pH of 30mL of 0.1M HCl‚ 0.1M NaOH‚ 0.1M CH3COOH‚ and 0.1M NH4OH(placed separately
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____________________________________________________________ ____________________________________________________________ ______ This lab was basically about finding the percentage of acetylsalicylic acid in an aspirin tablet. First‚ the base was created‚ which was made out of 1.00 g of NaOH and D-water. Then the buret was attached to the clamp on the ring stand and the base was poured into the buret. After that‚ one by one‚ an aspirin tablet was dropped into an Erlenmeyer flask filled with 50 mL of D-water so that it could become dissolved
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Duncan 11/24/13 Exothermic and Endothermic Reactions Lab The purpose of this lab is to observe how heat is released or absorbed with different chemicals. Data Table 1 – HCI and NaOH Trial 1 Trial 2 Avg Volume 1.0 M HCI(ml) 25 25 - Volume1.0 M NaOH (ml) 25 25 - Ti of HCI before mixing 20 20 - Ti of NaOH before mixing( 20 20 - Average Ti before mixing( 20 20 - Tf of mixture ) 26 26 - T ) 6 6 - Specific Heat (J/g) 4.184 4.184 - Heat‚ q (J) 1255.2 1255.2 1255
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distilled water then NaOH. 5. Obtain 60 mL NaOH and record exact concentration. Record initial volume. 6. Add 75 mL distilled water to the flask then add 3 drops phenolphthalein to dissolved sample. 7. Allow NaOH to go into the flask 1 mL at a time. When closer to then end point add one drop. When the solution changes color for 20 seconds‚ the titration is done. Record the finial buret reading. 8. Pour solution down the drain with water. Add more NaOH to buret if needed.
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prepared by chemical synthesis from salicylic acid‚ by acetylation with acetic anhydride. The fact that it is an acid allows us to quantify the amount of aspirin in a solution. We would do this by by using an acid-base titration. Sodium hydroxide (NaOH) will be used In this experiment as the base. Preparation • Lab coats should be fully fastened at all times. • Gloves and safety goggles should be worn at all times. Method In all titration experiments careful measurements are very essential
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