Objective 1. Use the analytical balance to weigh a given hydrated salt as accurate as possible in order to determine the weight of water in the salt Introduction Balances are important laboratory equipment as they are used to determine the mass of materials. Today‚ most balances used in the laboratory are analytical balances which can give readings up to four decimal places or higher. High accuracy is needed in certain experimental work such as material analysis or those involving small change
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math‚ however the calculations did. The harder math calculations included finding moles of the acid‚ moles of the base that was used to neutralize‚ and the molarity of the base. After all calculations‚ below is what we concluded. The molarity you had to be careful with because it was moles/liters and our readings were in milliliters so we had to convert first. In conclusion‚ even though the lab procedure is not about moles‚ most of the calculations are and this is one lab where the concept of
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by the direct titration of a filtered solution with a standard sodium hydroxide solution‚ since it is a slightly soluble salt. Because one mole of sodium hydroxide neutralizes one mole of HT- ions‚ the number of moles of sodium hydroxide used in the titration will equal the number of moles of HT-. The concentration of HT- can be determined by dividing its moles by its volume. The concentration of HT- will be equal to the concentration of K+‚ which in turn will be equal to
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Part a) Legal position enabling expulsion of Annabel from the partnership. Step 1:- The problem at hand deals with Partnership law as governed by the Partnership Act 1895 in the absence of a written agreement. Principles of Common law and Equitable principles also apply. Partnership Act governs the partnership of ‘Health Plus’. Sec. 30 of the Act‚ as it relates to misappropriation of partnership property. The application of Sec. 39 Partnership Act 1895 and the Fiduciary Duty breached. Supreme
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demonstrate the basic laboratory technique of titration 2. To learn to calculate molarity based on titrations INTRODUCTION Molarity (M) or molar concentration is a common unit for expressing the concentration of solutions. It is defined as the number of moles of solute per liter of solution (or millimoles of solute per milliliter of solution). The concentration of a basic solution can be determined by titrating it with a volume of a standard acid solution (of known concentration) required to neutralize
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150g Mass of weigh boat (g) .500g Mass of weigh boat + oxalic acid (g) 3.662g Mass of oxalic acid (g) 3.162g Concentration of 100.00ml .2510M Table 2: NaOH Mass of NaOH + weigh boat 11.336g Mass of weigh boat .500g Calculated mass of NaOH 10.836g Moles of NaOH .2709mol Concentration of 500.0ml NaOH .5418M Table 3: HCl Volume of Concentrated HCl 10.00mL Concentration diluted to 250.00ml .5475M Table 2: Volume of NaOH needed to neutralize 10.00 mL of oxalic acid Trial 1 Trial 2 Initial reading
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using the mole concept. Limiting Reactant: It is the reactant that will deplete or will be used up first during a chemical reaction. Limiting reactant also determine how long the reaction will last for. Balanced Equation: Mg + 2HCl = MgCl2 + H2 The balanced equation is needed to determine the mole ratio between the two reactants. From the equation we know that the equation mole ratio is 1:2. However‚ we need the actual mole ratio to find out the limiting reactant. The actual mole ratio is
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out who a suspected mole is in “the Circus” (British Intelligence Headquarters in London). Through the flashbacks‚ stories that nestle within stories‚
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the reaction has taken place. Therefore‚ the idea is that 50 cm³ of sodium thisoulphate are made to react with 5 cm³ of hydrochloric acid that is of different concentration each time. The concentrations of hydrochloric acid used varied from 0.1 to 5 moles. Afterwards‚ the cross is observed through the top of the conical flask until it because invisible. The time of which this happens is then recorded and monitored using a stopwatch. The symbol equation of this reaction is as follows: The above
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Equilibrium Constant of an Unknown Ester Hydrolysis Reaction Abstract The experiments to follow determined that the equilibrium concentrations of the reaction: ester + water ↔ alcohol + acid‚ are equal to 0.0363 moles of ester‚ 0.2852 moles of water‚ and 0.0268 moles each of alcohol and acid. Using this information the equilibrium constant was determined to be 0.06938. 1. Introduction In this lab the equilibrium constant‚ Kc‚ for the acid catalyzed reaction between an unknown
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