they too do not require an active role for the membrane. Osmosis is movement of water across a semipermeable membrane of low concentration to a solution of high concentration. On the other hand diffusion is movement of molecules from a high concentration to a low concentration. Osmosis is a form of diffusion but a distinction would be that it deals essentially with water. Tonicity is what makes the cells either shrink or grow depending on the environment it is placed at‚ it is an osmotic pressure and
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active transport? What is passive transport? How is osmosis related to diffusion? How can we demonstrate active transport? How can we demonstrate Brownian movement? How can we demonstrate diffusion (2 ways)? How can we demonstrate osmosis (3 ways)? In terms of relationships between substances‚ how can we define “hypertonic”‚ “isotonic”‚ and “hypotonic”? What is the relationship between the size of a molecule and its rate of diffusion? ____________________________________________________________________________
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incredibly thin that is very vital in maintaining the integrity of the cell. Not only does the plasma membrane bind the other organelles‚ it also forms a dynamic structure which gives them their remarkable activity and selectivity. (Hickman‚ 2008). Diffusion is the movement of particles from an area of higher concentration to a lower concentration until they reach Equilibrium. (Hickman‚ 2008).Osmosis happens when water diffuses across the membrane from the region of lower solute concentration (higher
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1 Sample 2 Molarity of KMnO4 0.02m 0.02m Weight of Sample 0.237g 0.225g Final Buret Reading 28.5ml 26.3ml Initial Buret Reading 0ml 0ml Volume of KMnO4 dispensed 28.5ml 26.3ml Moles of KMnO4 5.7E-4 5.26E-4 Moles of C2O42- 1.425E-3 1.315E-3 Table 2: (Second Titration) C2O42- Analysis Sample 1 Sample 2 Molarity of KMnO4 0.02m 0.02m Weight of Sample 0.237g 0.225g Final Buret Reading 4.2ml 4.5ml Initial Buret Reading 0ml 0ml Volume of KMnO4 dispensed 4.2ml 4.5ml Moles of KMnO4 8.4E-5 9.0E-5 Moles of
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from this experiment in solving similar problems. Result: N of KMnO4- N KMnO4 = trial 1: M KMnO4= ((0.2492g N2C2O4 x 1000)/ (134g N2C2O4/mol))/ 36.6 ml = 0.051 M N KMnO4= b . M 2eq/mol x 0.051M = 0.1 N KMnO4 Trial 2 M KMnO4= ((0.2389g N2C2O4 x 1000)/ (134g N2C2O4/mol))/35.7 ml = 0.05 M N KMnO4= 2 eq/mol x 0.052M =0.1 N KMnO4 Trial 3 M KMnO4= ((0.2125g N2C2O4 x 1000)/ (134g N2C2O4/mol))/ 32.8ml = 0.048M N KMnO4= 2eq/mol x 0.048M =0.097 N % Fe in razor blade Post lab # 3:
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EXPERIMENTAL Preparation of KMnO4 weight of KMnO4 = ? 300 mL of 0.01 M solution Dissolve in 100 mL distilled water. Dilute to reach 300 mL. Store in a colored container. EXPERIMENTAL Standardization of KMnO4 0.3 g-0.4 g of Fe(NH4)2(SO4)2●6H2O •100 mL beaker: 20 mL distilled water‚ 5 mL 2M H2SO4 voltmeter 2 mL increments of KMnO4 (Vtotal = 20 mL) 1 mL increments of KMnO4 (Vtotal = 30 mL) Measure reduction potentials. Repeat to make 3 trials. EXPERIMENTAL Standardization of KMnO4 10 mL unknown diluted:
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present in a product. If the product contains a substance that can be oxidized‚ then it is possible to determine the number of moles of that substance by titrating the sample with a solution of a strong oxidizing agent. In this lab‚ a solution of KMnO4‚ an oxidizing agent‚ will be standardized by titration with a solution containing a known concentration of iron (II) ions‚ (Fe+). The concentration of oxalic acid solution will be determined by titration with the MnO4- solution that had been standardized
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temperature has on the rate of the reaction 1. In part one‚ the reactants potassium permanganate (KMnO4) and oxalic acid (H2C2O4)‚ three determinations were performed‚ each with different initial concentrations of the reactants. Each initial concentration resulted in a unique reaction rate; these rates were then examined using the method of initial rates to determine the order of the reaction with respect to both KMnO4 and H2C2O4. The rate constant (k)‚ was then calculated‚ and the rate equation for the reaction
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0.1 N KMnO4 solution. In determining the Normality of KMnO4 (FW=158grams/mol)‚ Na2Cr2O4 was used as the primary standard. Na2Cr2O4 was titrated with KMnO4 in three trials. The Normality of KMnO4 computed using the volume of KMnO4 obtained during the three trials on the titration with Na2Cr2O4. The mass of Na2Cr2O4 used (see appendix). The Normality obtained in each trial are slightly close with each other. This may be due to the differences of the masses in Na2Cr2O4 and the volume of KMnO4. Other
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Redox Reaction Lab Practical Luis Suarez and Lukyon Mendrin CHEM 1A Lab‚ Department of Chemistry‚ California State University‚ Fresno‚ CA 93740 Lsuarez054@mail.fresnostate.edu April 13‚ 2016 In This experiment we used potassium permanganate (KMnO4) as our titrant and our titrand was oxalic acid (H2C2O4● 2H2O). The objective of the experiment was to titrate the solutions to determine the molarity of potassium permanganate. We had to dilute the stock solutions to a specific molarity for the experiment
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