halogens’ (NaF‚ NaCl‚ NaBr‚ and KI) reactions with the chemicals Ca(NO3)2‚ AgNO3‚ and NH4OH and use these observations to identify an unknown halogen. Data: (see next page) TABLE 1: REACTIONS OF HALOGENS WITH CA(NO3)2‚ AGNO3‚ AND NH4OH REACTION NAF NACL NABR KI REACTION W/ CA(NO3)2 solution turns cloudy and precipitate forms clear precipitate formed slightly cloudy precipitate formed no reaction REACTION W/ AGNO3 no reaction white‚ cloudy precipitate formed thick white/yellow
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Barium Chloride (BaCl2) * 8 -grams of Silver Nitrate (AgNO3) * Analytical Balance * 2- Volumetric Flasks; one 50 mL flask‚ and one 100 mL flask * 2- Scoopulas * 10- Weigh Boats * 5- Filter paper * 5- 250 mL beakers * 2- 25 mL pipets * Distilled water * 2- 100 mL Erlenmeyer flasks * 2- glass funnels Procedure: 1. To the best of your ability‚ weigh out 3.75 grams of BaCl2 and 6.125 grams of AgNO3 on separate weigh boats 2. Pour the BaCl2 into the
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is a very insoluble solid‚ yet still does have some solubility. Because of these traits‚ the following reaction is able to occur: Ag+(aq) + Cl−(aq) → AgCl(s) . This reaction is able to occur in both directions. When a soluble silver salt such as AgNO3 is added to a solution containing Cl−(aq) ion‚ then the added Ag+(aq) precipitates as AgCl(s) until all the chloride is consumed. For this particular reaction K sp = 1.6 x 10−10. The reason why the solution is precipitated in an acidic medium become
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containing AgNO3 (Table 1). Graph one depicts the correlation of percent change in weight for each sucrose concentration with AgNO3 added. The initial length of the potato cylinders were 2cm as depicted in table two. Graph two depicts the correlation of percent change in length in different sucrose concentrations. The initial weights for the solutions lacking AgNO3 ranged from 1.0-1.7grams (Table 3). Graph three displays the correlation for the percent change in weight for a solution lacking AgNO3 in different
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Last Name ____________________First Name _______________________ Ignore: 5‚ 7‚ 19‚ 30 1. | How many grams of CaCl2 (molar mass = 111.0 g/mol) are needed to prepare 4.44 L of 0.500 M CaCl2 solution? | | A) 369 g B) 271 g C) 258 g D) 296 g E) 246 g | 2. | An aqueous solution of ammonium sulfate is allowed to react with an aqueous solution of lead(II) nitrate.The complete ionic equation contains which of the following species (when balanced in standard form)? | | A)
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reaction occurs where the balance equation is then 2AgNO3 + Cu(s) 2Ag + Cu (NO3) 2 III. Materials * 1 pair of gloves * 1 pair of safety glasses * 1 (10 cm) Copper Wire * 1 Plastic container * 1 bottle of 0.50 AgNO3 * 1 bottle of distilled water * 1 Weighing tray * 1 square of hard‚ rough paper (to sand wire) * 1 electronic balance * 1 pipet * 1 pair of forceps * 1 beaker * 1 pencil * 1 marker
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Slowly turned darker | Rapidly turned darker red | Slowly turned into Brown (yellowish) | [Part 2] Procedure: The solutions that we used were: * 5 ml of 0.1 mol dm-3 of K2CrO4 * 5 ml of 0.1 mol dm-3 of K2Cr2O7 1. We named 4 test tubes as #5‚ #6‚ #7 and #8. 2. We put 5 ml of 0.1 mol dm-3 of K2CrO4 into tubes #5 and #6 3. We put 5ml of 0.1 mol dm-3 of K2Cr2O7 into tubes #7 and #8 4. We added 1.0 mold
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and then weighed. For this lab‚ lead (II) nitrate (Pb(NO3)2) and potassium chromate (K2CrO4) will be reacted together to demonstrate double replacement reaction between 2 ionic compounds. This was shown when chromate replaced the nitrate and formed lead (II) chromate‚ and when the nitrate replaced the chromate and formed potassium nitrate‚ which is shown in the following equation: Pb(NO3)2 + K2CrO4 PbCrO4 + 2KNO3 In this experiment‚ I found that when two ionic compounds that are
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Techniques: A Microscale Approach‚ 5th edition by Pavia‚ Lampman Kriz‚ and Engel pages: 186-189 Experiment 21: Reaction of some Alkyl Halides See carbon copy pages: 33-35 Observations See carbon copy pages: 33-35 Results: Compounds AgNo3 (RT) AgNO3 (50°C) 2-Chlorobutane No reaction No reaction 2-Bromobutane cloudy ------ 1-Chlorobutane No reaction Cloudy‚ precipitate 1-Bromobutane cloudy ------ t-butyl Chloride Cloudy ------ Crotyl Chloride cloudy ------ Benzyl Chloride cloudy ------
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Fe(NO2)2 11. A chemist has 4.0 g of silver nitrate and needs to prepare 2.0 L of a 0.010 M solution. Will there be enough silver nitrate? If so‚ how much silver nitrate will be left over? 2.0 L soln x 0.010 mol AgNO3 x 169.88g AgNO3 = 3.4g AgNO3 Used/Needed 1 L soln 1 mol
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