starch (cooled) + 3 ml saliva (cooled) in ice bath; Tube 4 = 3 ml starch + 3 ml saliva 5 drops conc. HCL in water bath. An incubation period of 1 hour was followed and each was tested for starch and maltose. A similar procedure was repeated with pepsin‚ with the test tubes prepared as follows: Tube 1 = 5 ml pepsin 5% soln + 5 ml HCL (0.5)%; Tube 2 = 5 ml pepsin (5% soln)+ water 5 ml; Tube 3 = 5 ml HCL (0.5%) + 5 ml of water; Tube 4 = 5 ml pepsin 5% soln) + 5 ml NAOH (0.5%). Lastly‚ the above procedure
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the acid and the base. In this experiment acid-base titration will be used to determine the concentration of HCl at equilibrium when it reacts with the NaOH H+ (aq)+ Cl- (aq) + Na+ (aq) + OH- →H2O(l) + Na+ (aq)+ Cl- (aq) Procedure When performing this experiment one must first obtain and wear goggles. Next add 40mL of distilled water to a 100mL beaker‚ then add 5.00mL of HCl to the beaker.Then obtain 40mL of 0.1M NaOH. Place the NaOH in a 60mL reagent reservoir and drain a small amount
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determine the quantity of zinc chloride that is produced in a chemical change from a given amount of zinc. Background: We used two important laws of chemistry in this lab. Firstly‚ the Law of Conservation of Mass states that matter is neither created nor destroyed during a chemical reaction and the mass of a system should therefore remain constant during any chemical process. In other words‚ the mass of any one
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and also my merging with a company called AXON. Different Ways Messaging Was Used Instead of holding a live Blueprint meeting‚ HCL decided to have all three hundred of their managers record their business plans‚ which would then be posted on the MyBlueprint portal. Once all of the business plans were posted‚ they’d be open for review by another eight thousand HCL managers. The idea was to transform the planning process into a peer-to-peer review rather than a top-down judgment. (Nayar‚ 2010)
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Prof. T.D. Macasil BSE Physical Science Reactions of amines Reaction of amines with acids – acids and amines form ammonium salts. R – NH2 + HCl → R – NH3+ + OH – Amine acid amine salt Example 1 CH3 – NH2 + HCl → CH3 – NH3 + Cl- Methylamine Methylammonium Example 2 CH3CH2 – NH3 + Cl → CH3CH2NH2 . HCl Ethylammonium Ethylamine Reaction of amine with water – when amines react with water‚ they produce hydroxide ( OH ) R – NH2 + H2O
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5.00 mL HCl soln. x 1.217g HCl soln = 6.085g HCl soln. 1 mL HCl soln 3.0 mol HCl x 36.5g HCl x 1mL soln. = 0.0899g HCl x 5mL = 0.4495 g HCl 1000mL soln mol HCL 1.217g HCl soln mL 6.085g HCl soln. 0.4495 g HCl = 5.63 g H2O 5.63 g H2O x 1 mole H2O = 0.312 moles H2O from HCl solution 18.02 g H2O Then the product amounts at equilibrium were calculated
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H3O+ with NaOH solution can achieve the determination of the amount of acid‚ which has not reacted with the calcium carbonate. There are differences between amount of the acid (HCl) added and the amount left over after the reaction is equal to the amount used by the CaCO3. The reaction used to determine the leftover acid is: HCl (aq) + NaOH (aq) H2O + Na+ (aq) + Cl- (aq) Aim To measure the percent by mass of CaCO3 in an eggshell. Variables Independent variables: Mass of calcium carbonate in
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AgCl(soluble in 12M HCl‚ soluble in sln of good complexing agent‚ 6M NH3) | White ppt‚ PbCl2(soluble in hot water‚ soluble in 12M HCl‚ soluble in sln of xs NaOH) | Soluble – no ppt | Soluble – no ppt | Soluble – no ppt | Na2CO3 | White ppt‚ Ag2CO3(soluble in 6M HCl‚ soluble in sln of good complexing agent) | White ppt‚ PbCO3(soluble in 6M HCl‚ soluble in sln of good complexing agent) | Blue ppt‚ CuCO3(soluble in 6M HCl‚ soluble in sln of good complexing agent) | Green ppt‚ NiCO3(soluble in 6M HCl‚ soluble
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yield versus the theoretical yield of NaCl when HCl is titrated into Na2CO3 and NaHCO3. When 0.15g of both NaHCO3 and Na2CO3 are titrated with HCl‚ then 0.165g of NaCl should form from the NaHCO3‚ and 0.104g of NaCl should form from the 0.15g of Na2CO3. Procedure: Weigh 2 samples of 0.15g of dried unknown each‚ and dissolve each into 50mL of distilled water. Add 0.5 to 1mL of bromocresol green indicator until the solution turns blue. Titrate the HCl until it turns green. Gently heat and boil out
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thermometer so as to not puncture a hole in the calorimeter) to determine the heats of reaction for Magnesium (Mg) with Hydrochloric Acid (HCl) and Hydrochloric Acid with Magnesium Oxide (MgO). Then using mathematical formulas we were able to calculate the heat formation of MgO‚ which is measured in kJ/Mol. Since both reactions are in dilute water solutions of HCl it was necessary to know the heat capacity of water‚ but because some heat would be transferred to the calorimeter whose heat capacity was
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