Hydroxide (NaOH) by titrating it with Hydrochloric Acid (HCl) and to identify any possible sources of error. A colour change from pink to yellow signified the end of each individual titre as the NaOH had been neutralised. Experimental: Method: Firstly two solutions were prepared to show the colour of the Phenol Red indicator in acid and alkaline conditions. These colours were then used to determine the end point of each titre. In the experiment 0.100M HCl (acid) was added‚ from a burette‚ to a solution of
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The unknown soda ash from experiment 3 was used‚ to determine the weight for each trial we used the equation of (M of HCl) x (18 ml x 105.99) / (10 x 2 x Na2CO3 ). Which was equal to (0.01472 M) x ((18 mL X 105.99)(10 x 2 X 2.428 % )= 0.6 g. To start we had to rinse the beakers‚ electrode and the stirring bar with diluted water. The sample we needed was weighted to the closest 0.1 mg which we got was 0.3 for the first trial. The sample was transferred to a 250 mL beaker and dissolved in 70 mL of
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THE EFFECTS OF DIFFERENT FORMULATED ORGANIC PESTICIDES TO THE PREVENTION OF OCCURANCE OF PESTS Reaman S. Balois Paulene Andrea D. Pontela THESIS REPORT Republic of the Philippines ISABELA STATE UNIVERSITY Roxas‚ Isabela THE EFFECTS OF DIFFERENT FORMULATED ORGANIC PESTICIDES TO THE PREVENTION OF OCCURANCE OF PESTS Thesis outline presented to the faculty and staff of Isabela State University‚ Roxas‚ Isabela in partial fulfilment of the requirements
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Effects of pH on the Function of Enzymes Rena Mototani Glen Rock High School Advanced Biology 2014-2015 Effects of pH on the Function of Catalase Rena Mototani Problem: How does the pH of a cell affect the function of the enzyme catalase? Introduction In this lab‚ we experimented the effects of pH on the function of the enzyme catalase. Catalase is an enzyme that brings about the reaction by which hydrogen peroxide is decomposed to water and oxygen (Encyclopedia Britannica). The
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A Strategic management Report On The Laptop Industry in India By: Abhishek Dutta Ayush Palod Amit Jha Aditya Patnaik Debanjan Roy Kanwardeep Singh Mukesh Lohan Pallavi Arora Ravinder Pal Singh Shantanu Sinha Sujay Kher Somdipto Ghosh A brief Introduction on the Laptop Industry of India Computers One industry which continues to hold its head high even in an environment of industrial slowdown is information technology (IT) - with annual growth rates of software value hovering between 20% and 30%
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Group II (conc H2SO4 group) – Cl(chloride)‚ Br- (bromide)‚ I- (iodide)‚ NO3- (nitrate)‚ CH3COO- (acetate)‚ C2O42(oxalate): Salt + conc H2SO4 1. No reaction: Group II anion not present. Continue to group III. 2. Chloride: Colourless white pungent fumes (HCl); intensify when glass rod dipped in NH4OH is brought near mouth of test tube 1. Silver nitrate test: WE + AgNO3 = white ppt soluble in NH4OH 2. Chromyl chloride test: Salt + solid K2Cr2O7 + 2-3 drops conc H2SO4 = orange / red fumes of chromyl chloride
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approx. 0.5 cm × 2 cm‚ or solid marble chips zinc powder or calcium carbonate powder balance 2 test tubes 1M HCl (approx 10 mL per group) Part 2. Effect of Temperature 3 Alka Seltzer tablets 3 250-mL beakers water at three temperatures – with ice‚ room temperature‚ warm (around 70°C) Part 3. Effect of Concentration 1M HCl‚ 5 mL per group 3M HCl‚ 5 mL per group 6M HCl‚ 5 mL per group 3 pieces of zinc metal‚ each approx 1 cm × 1 cm 3 test tubes Part 4. Effect of a Catalyst
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between CuSO4 and NaOH. In this method of experiment‚ the total molar concentration of the two solutions are held constant‚ but their mole fractions are varied. In the second experiment‚ it was observed the reaction of acid-base in solution of NaOH with HCl in different condition of volume for each. An observable that is proportional to complex information is plotted against the mole fractions of these two components. The maximum on the plot correspond to stoichiometry of the solutions or species if sufficiently
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| 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 in color| F.|NaOCl + KI| |See back page| | with 1 drop of starch|
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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 when it dissolved in water. The OH- ion is also formed when ammonia dissolves in water. NH3 + H2O NH4 + OH- HCl + H2O Cl- + H2O- However‚ the reaction between ammonia and hydrogen chloride doesn’t need water or any other solvent to take place. When the gases of ammonia and hydrogen
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