used the more number of moles are needed to neutralize. To increase the number of moles you can increase the concentration or decrease the volume. If we take an overview of the reaction‚ the protons from the HCl moved to the NaOH or the HCl donated H+ ions to the solution and NaOH gave OH- ions to the solution. And as a result a salt (NaCl) and water were formed. The methods used were quiet precise. The burette and pipette have some limitations due to being less precise. The volume of burette limited
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Experiment: Calorimetry Laboratory Experiment – Heat of Solution Aim: The aim was to use calorimetric measurements to calculate the molar heat of solution of NaOH and NH4NO3. Method: 1. 50g of water was poured into a clean polystyrene calorimeter (Styrofoam cup) and the initial temperature was measured. 2. A teaspoon of 2g of the selected salt was measured and added into the water. 3. The solution was stirred and the final temperature was measured when the solution stabilised and the results
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Synopsis The objective of this experiment is to determine the percentage by mass of calcium carbonate‚CaCO3 in toothpaste using back titration technique. A known weight portion of toothpaste is obtained to react with known volume and concentration of standard acid solution. After completing the reaction‚ the resulting solution containing excess acid is back titrated with known volume and concentration of standard base solution. Determination of excess acid after reaction allow us to calculate the
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specific example of stoichiometric determination‚ which is: “Stoichiometry and limiting reacting”‚ we found out the different mass proportions in which substance react. In this case‚ we used two common acids for this experiment (HCl‚ and H2SO4) and base NaOH Introduction: For this experiment‚ we use Stoichiometry and limiting reactant. The limiting reactant refers to the reactant that controls the amount of product that is
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Carbon Dioxide Understanding and Production in Elodea‚ Snail‚ and Goldfish Introduction This report discusses an experiment to study the rate of aerobic cellular respiration in aquatic organisms which are Elodea (aquatic plant)‚ Snail‚ and Goldfish‚ by measuring carbon dioxide production. Because ectothermic organisms (Elodea‚ snail‚ and goldfish) were placed in completely covered beaker‚ each organism would produce different amount of carbon dioxide. The objective of the experiment is to measure
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Introduction Extraction is a purification technique used in organic chemistry to separate compounds from a mixture of two or more compounds. There are three different extraction techniques: liquid-liquid extraction‚ solid-liquid extraction and chemically active extraction. All three types of extraction follow the same principle. Organic molecules dissolve in organic solvents and polar molecules dissolve in aqueous solvents. This phenomenon is observed because of the intermolecular forces between
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I think we made a mistake because when I calculated the moles for the NaOH and CaCl2‚ we got the same amount of moles for both solutions. That means that from the moles‚ there was no limiting reactant in test tube 3. From this lab‚ I learned how to calculate and find the limiting reactant. I also learned how to use stoichiometry. In my calculations‚ the limiting reactant depended on the test tubes. For test tube 1‚ NaOH was the limiting reactant‚ test tube 2 had no limiting reactant from my
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[Zn 2+][OH –]2 pH 9.35 = pOH 4.65; [OH –] = 10–4.65 = 2.24 x10–5 M Zn2+ = Ksp/[OH -]2 = 7.7x10-17/[2.24 x10-5]2 = 1.5 x10-7 M (ii) At 25˚C‚ 50.0 mL of 0.100-M Zn(NO3)2 is mixed with 50.0 mL of 0.300-M NaOH. Calculate the molar concentration of Zn2+ (aq) in the resulting solution once equilibrium has been established. Assume that volumes are additive. [Zn2+]init = (0.100M )(0.050 L) = 0.0500 M [OH–]init = (0.300M)(0.050 L) = 0.150 M X =
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HCl and others for use with the NaOH. 2. Record the exact molarity as they appear on the stock bottles. 3. Determine the mass of each of you antacid tablets. 4. Dispense 25 mL of HCl solution into the Erlenmeyer flask‚ and then add one of the antacid tablets to the flask. 5. Bring the solution to a boil to dispel any undissolved CO2. 6. Add two or three drops of an indicator to our antacid mixture. 7. Titrate antacid mixture with the NaOH solution until we have reached
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• Fe(NO3)2(aq)+NaOH(aq) → Fe(OH)3(s)+ NO-3(aq)+Na+(aq) • Cu(NO3)2(aq)+NaOH(aq) → Cu(OH)2(s)+ NO-3(aq)+Na+(aq • Ni(NO3)2(aq)+NaOH(aq) → Ni(OH)2(s)+ NO-3(aq)+Na+(aq) • Al(NO3)2 (aq)+NaOH(aq) →Al(OH)(s)+ NO3-(aq)+Na+(aq) • Al(NO3)2 (aq)+NH4OH(aq) →Al(NH4)6+ (s)+ NO3-(aq)+Na+(aq) • Mn(NO3)2 (aq)+NaOH(aq) →Mn(OH)2(s)+ NO3-(aq) +Na+(aq) • Pb(NO3)2 (aq)+H2S(aq)↔PbS2(s)+ S2-2(g)+NO3-(aq) • Ag(NO3) (aq)+H2S(aq)↔
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