Investigation Srategy I am ivestigating the reaction of sodium thiosulphate and hydroclohric acid. sodium thiosulphate(aq) + Hydroclohric Acid (aq) --> Sodium cloride (aq) + Sulphur Dioxide (g) + Water (l) + Suplhur (s) Na(2)S(2)O(3) + 2 HCl --> 2NaCl + SO(2) + H(2)O + S The finished reaction of the 2 clear liquids is cloudy.I will use this change from clear to cloudy as an indicator as to when the reaction is finished. By using this change ‚ i can see the effect of changing other factors
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between concentration of hydrochloric acid (HCl) and the rate of diffusion?” My hypothesis for this research question is that change in rate of diffusion will be observed when the agar blocks are placed in solutions of different concentrations of HCl. As the concentration of HCl increases‚ the rate of diffusion will also increase due to the steeper concentration gradient created. To investigate the change in rate of diffusion when different concentrations of HCl are used‚ I used agar blocks that are stained
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Experiment 11.1 Conversion of t-Amyl Alcohol to t-Amyl Chloride Using HCL October 27‚ 2011 Purpose: Alkyl halides can be prepared from alcohols by reacting them with a hydrogen halide‚ HX (X = Cl‚ Br‚ or I). The mechanisms of acid-catalyzed substitution of alcohols are termed SN1 and SN2. The “S” stands for substitution‚ the “N” stands for nucleophilic‚ and the “1” or “2” stand for unimolecular or bimolecular. Secondary alcohols react with hydrogen halides by both SN1 and SN2
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The full strength 1M HCl acid had a pH level of 3.12 (Table 3.1). Sample A2 to A4 remained in the pH 3 level‚ while sample A5 and A6 had a pH range of 4 (Table 3.1). The pH level for 1M HCl dilutions slightly increased between each sample (Table 3.1). The diluted solutions of 1 M NaOH showed a few unexpected results. The original solution of 1 M NaOH was at a pH level of 11.50 (Table 3.1). However‚ the pH of sample B2 increased to 12.81 (Table 3.1). The remaining samples had a decreasing pH pattern
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Determining the Ksp of Calcium Hydroxide by Titration of Saturated Ca(OH)2(aq) with HCl(aq) Abstract: Titration is a technique that has been used in this experiment to identify the Ksp value of calcium hydroxide in order to determine the extent to which the compound is soluble in water. A known volume of 50 mL of hydrochloric acid‚ a concentration of 0.05 M hydrochloric acid‚ a volume of 50 mL calcium hydroxide base‚ an unknown concentration
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1. Gather all the equipments needed. 2. Measure 50ml of HCL in a 250 ml measuring cylinder and pour it into a flask‚ then measure 50ml of HCL again and pour it into the second flask. 3. Measure the 50ml of KOH in a measuring cylinder. Repeat it again in another measuring cylinder. 4. Attach both of the burette clamps to both of the burette stands and clamp the burette at a certain level so that it can fit a flask underneath. 5. Then‚ place a funnel on top of each burette. 6. Place a flask underneath
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eggshells is calcium carbonate‚ CaCO3(s). This analysis is done volumetrically by using a characteristic reaction of carbonate compounds‚ namely their reaction with acids. Calcium carbonate (limestone) is very insoluble in pure water but readily reacts in acid according to the reaction below. 2HCl(aq) + CaCO3(s) → CaCl2(aq) + CO2(g) + H2O(l) + HCl(aq) (in excess) (limiting reagent) (1) (unreacted) This reaction cannot be used directly to titrate the CaCO3 because it is very slow when
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8950g ± 0.002g = 1.657 ± 0.017 mol/dm3 0.0056dm3 ± 0.00005dm3 × 204.23g /mole Concentration of NaOH = 1.657 ± 0.017 mol/dm3 Part B : Standardization of 2M HCl Data Collection : Volume of HCl in a conical flask (ml) ± 0.05ml Burette Reading of NaOH(ml) ± 0.05ml Volume of NaOH solution for neutralization End point of titration - 10ml ± 0.05ml Initial final = final – initial = (10.3 ± 0.05ml) – (0.0 ml ± 0.05) Colorless
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chosen compound Marta Dürrigl 1mmA Chemical reaction: b.) CaCO3 (s) + 2HCl (aq) ----------- CaCl2 (aq) + CO2 (g) + H2O(l) AIM: The aim of this investigation is to experimentally determine the molar mass of carbon dioxide (CO2) by measuring its volume and calculating its mass. CO2 which we will measure will arise as a product of a chemical reaction between Calcium Carbonate (CaCO3) and Hydrochloric acid (HCl) as it is shown in the chemical equation above. Once we find out
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Candidate’s name: Eunika Orłowska Candidate’s number: School’s name: School’s number: Determining the amount of CaCO3 in eggshell of hen’s egg | Design | DCP | CE | Aspect 1 | | | | Aspect 2 | | | | Aspect 3 | | | | Introduction: The back titration is a method used in determining the amount of excess of the reagent. The calcium carbonate is a substance which gives the eggshell stiffness. Research question:
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