in a color change from yellow to reddish-brown at the end point. Knowing the molarity of the titrant allows for calculation of the chloride concentration. Materials: volumetric pipettes‚ tubes‚ 250 mL Erlenmeyer flasks‚ 50 mL buret‚ 16.7 g/1L of AgNO3‚ CrO4 solution. Weigh out the sample (NaCl + KCl mixture) into a dry tube in a range of 0.150 g to 0.250 g. Dissolve the salt with water to 10 mL/15 mL/20 mL. Pipette a 5 mL aliquot of diluted salt into a 250 mL flask and add distilled to 100 mL
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we hypothesized that when silver nitrate‚ AgNO3‚ reacts with copper‚ Cu‚ the oxidation number of silver (Ag) ions that form will be +1. The unbalanced chemical equation that we used to represent this reaction is Cu + AgNO3 → Ag + Cu(NO3)2. In order to find the approximate masses of reactants needed to produce about 2 grams of silver‚ we found the molar masses of each of the reactants and products: Molar Masses | |AgNO3 |Cu
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cylinder). Reactivity. To determine some chemical properties of the compound‚ precipitate tests were performed. Aqueous solutions of the compound‚ each made with 1 mL distilled water and 0.1 g 643p‚ were mixed in test tubes with aqueous solutions of AgNO3(1 mL of 0.1 M)‚ NaCO3(1 g in 1 mL H2O) and BaCl2 (1mL of 0.2 M)to determine the reactivity of the compound 643p with each compound. These tests were also performed on solutions of possible compounds that the 643p could be‚ in the same way‚ to determine
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increases with temperature‚ favouring less solid and more ions‚ therefore the PbCl2 dissolves in hot water: PbCl2(s) → Pb2+ (aq) + 2 Cl-(aq) (4) Once Pb2+ has been put into solution‚ we can check for its presence by adding a solution of K2CrO4. The chromate ion‚ CrO42-‚ gives a yellow precipitate with Pb2+: Pb2+ (aq) + CrO42-(aq) → PbCrO4(s) (5) Yellow The other two insoluble chlorides‚ AgCl and Hg2Cl2‚ can be separated by adding aqueous ammonia. Silver chloride dissolves‚ forming
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Large test tube • 250 ml beaker • Silver nitrate (AgNO3) powder • Dilute AgNO3 solution • Distilled water • Electronic balance • Glass stir rod • Watch glass PRE-LAB DISCUSSION A single replacement reaction occurs when an uncombined element “replaces” another element that is contained in a compound. You will prepare and observe a single replacement reaction in this lab. Your reactants will be copper (Cu) and silver nitrate (AgNO3). You will weigh the reactants and the products carefully
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Experiment No. 2: Dynamic Equilibrium and Le Chatelier’s Principle December 1‚ 2011 Final Formal Results Le Chatelier’s Principle states that “when a stress is applied to a chemical system at equilibrium‚ the equilibrium shifts in a direction that reduces the effect of stress” (Gross‚ Abenojar‚ and Tan 23). Moreover‚ it helps us “predict the direction of the shift of the equilibrium” (Silberberg 745). Silberberg also stated that there are three kinds of disturbances - concentration‚
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Effect of light on Silver Halide Salts Aim: To investigate the effect of sunlight and UV light on silver salts and to identify an application of this reaction. Hypothesis: The compounds exposed to sunlight (which already contains UV light) will decompose. The compounds which are not exposed to light (put in a dark place) will not decompose. Theory: Equipment: * 4 x petri dishes * 1 x glass stirring rod * 0.1 mol/L silver nitrate in a dropper bottle * 0.1 mol/L Sodium chloride
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And since AgNO3 is a one to one mole ratio the number of moles of Ag ions can be calculated. Then once more the moles of Ag ions equal moles of Cl- because once again there is a one to one mole relationship. From all of that the concentration of Cl- can be found by
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silver nanoparticles. UV–Vis spectra of biomass of Streptomyces spp. 211A treated with 10–3 M AgNO3 aqueous solution for 9 days. The observation of peak at 425 nm in the aqueous silver nitrate – Sp. platensis and silver nitrate – Streptomyces spp. 211A reaction medium indicates the extracellular synthesis of silver nanoparticles. Diffractogram of Sp. platensis biomass after exposure to 10–3 M AgNO3 aqueous solution for 2 days. 4- Extracellular synthesis of silver nanoparticles by the Bacillus
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Name: Kamaal Thomas |Date: January 4‚ 2011 | |Graded Assignment Lab Report Answer the questions below. When you have finished‚ submit this assignment to your teacher by the due date for full credit. (8 points) |Score | | | 1. For Part 2: Single-Displacement Reactions: For each of the four single-displacement reactions‚ describe what happened in each well. If a chemical reaction occurred‚ write a balanced equation for it. Then using the A‚ B symbols‚
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