and 3 drops of phenolphthalein indicator was added to the flask and then titrated with the standard NaOH solution. Finally‚ the 2 infinity samples were titrated in the same way and the [HCl] was calculated. [HCl]t was calculated from each aliquot sampling. Lastly‚ Excel software was used to plot ([HCl] -[HCl]t) vs. time(t). The slope of the straight line through the points enabled the calculation for the rate of the reaction. Results
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quantities of NaHCO3 was added in order to adjust the pH of the solutions until effervescence ceased. About 2 mL of K2Cr04 was added and the solution was titrated with 0.1 M AgNO3 solution to the first permanent appearance of red Ag2Cr2O4. B. Determination of Cl- in solid sample The unknown was dried at 110 for 1 hour and cooled in a desiccator. Individual samples were weighed into each of three 250 mL Erlenmeyer flasks and dissolved in about 100 mL of distilled water. Small quantities of NaHCO3 was added
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Making sure to place only 2 drops of the first chemical then adding only 2 drops of the second chemical the observation of the reaction can be made. To properly observe the titrations move them between a dark background and a white background. a. NaHCO3 & HCI- bubbles form b. HCI & BTB c. NH3 (Ammonia) & 1 drop of BTB- record expected color & actual result. d. HCI & blue dye e. Blue dye & NaOCI. Record findings‚ then add 1 drop of HCI f. NaOCI & KI. Observe‚ then
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account statements and calculating different ratios related to Profitability‚ Liquidity‚ Asset Management and Long-Term Debt Paying Ability. Also‚ I will be doing a comparative analysis of Wipro with its nearest competitor Hindustan Computer Limited (HCL). I will also be doing a sector outlook of the IT industry and the government policies related to the IT industry‚ the Holding pattern & ownership of shareholders‚ FII’s‚ Financial Institutions‚ public‚ etc.‚ the price trend of the Wipro’s stock in
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EQUILIBRIUM CONSTANT OF A REACTION Methodology The following stock solutions were prepared: 1.0 M HCl‚ 0.1 M HCl‚ 0.1 M KSCN‚ 0.002 M KSCN (in 0.1 M HCl)‚ 0.2 M FeCl3 (in 0.1 M HCl)‚ and 0.002 M FeCl3(in 0.1 M HCl). Using the prepared stock solutions‚ the standard (Table 1) and Unknown (Table 2) solutions were prepared. Table 2. Preparation of Standard Solutions 0.10 M KSCN 0.002 M FeCl3 0.1 M HCl Blank 2.0 ml 0.0 ml 8 ml S1 2.0 ml 0.1 ml 7.9 ml S2 2.0 ml 0.25 ml 7.75 ml S3 2.0 ml 0.5 ml
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objective of the Get Charged Up lab was to determine the charge on a metal ion reacting with HCl by determine the mole ratio in a reaction by determining the amount of excess reactant‚ amount of product‚ and amount of hydrogen gas produced as well as finding the best research method to determine the charge. To accomplish this‚ three different methods were used. Titration was used to react NaOH with HCl to determine the amount of H+ left over after the reaction is complete. Crystallization was
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Discussion 2mol of HCL * V = 50 cm3 * 1 mol 50/2=V V=25 cm3 Volume needed to neutralise 50 cm3 of 1 mol dm-3 of NaOH is 25 cm3 of HCL b) Independent variable: Volume of HCL Dependent variable: Temperature of mixed solution Controlled variables: Volume of alkaline‚ Concentration of acid‚ Concentration of alkaline c) Burette d)Fix the burette into a burette holder securely. Pour HCL into the burette with a funnel until it reaches the 0.0cm3 mark. e)The risk of using plastic cup
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acid. Magnesium reacts with magnesium is react with hydrochloric acid to form hydrogen gas. The aim of this experiment is to determine the value of x in the following equation: Mg + X HCl → MgCl2 + X/2 H2 A known amount of magnesium is reacted with a large excess of HCl‚ and the volume of H2 evolved is measured. As HCl is in excess‚ all the magnesium will be consumed‚ and the yield of both MgCl2 and H2 is dependent on the amount of magnesium used. A comparison of the amount of hydrogen produced with
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normality) of the standard solution and the measured volume of unknown solution used‚ the unknown concentration can be calculated. For example‚ standard base solution (NaOH) is added from a burette to an accurately known volume of the acid solution (HCl). HCl(aq) + NaOH(aq) ------------> H 2 O(l) + NaCl(aq) This reaction (neutralization) can be written as a NET IONIC equation as follows: H+(aq) + OH-(aq) ----------> H 2 O(l) (2) (1) When sufficient NaOH has been added to react with all of the acid
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Chemistry Lab Report Stoichiometry Design Experiment Percentage Yield of Calcium Carbonate and HCl I. Background Information When marble chips and hydrochloric acid are added together‚ they form sodium chloride‚ water‚ and carbon dioxide. This reaction can be displayed by the balanced equation below; CaCO3 (s) + HCl (l) NaCl(s) + H2O(l) + CO2 (g) As the carbon dioxide is formed‚ it will leave the open beaker as a gas. This will result in a loss of mass. The mass change can then be
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