Observations will be used to determine the halide ion presented in the unknown solution. Hypothesis: If the halide ions react‚ then the production of precipitate and complex ions will be recognizable. Materials: * * 24-well microplate * AgNO3‚ 0.1 M * Ca(NO3)2‚ 0.5 M * Gloves * KBr‚ 0.2 M * KI‚ 0.2 M * Lab apron * Na2S2O3‚ 0.2 M * NaCl‚ 0.1 M * NaF‚ 0.1 M * NaOCl (commercial bleach)‚ 5% * NH3(aq)‚ 4 M * Safety goggles * Starch solution‚ 3%
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=> Ag+(aq) + Cl-(aq) Ksp = [Ag+(aq)]·[Cl-(aq)] = 1.6 x 10-10 While silver chloride will be in equilibrium with its ions in the solution‚ because Ksp is so small‚ the dissolved ions can be considered negligible. When AgNO3 is added to a solution containing containing Cl- ions‚ a displacement reaction is undergone and the Ag+ and Cl- ions will precipitate out quickly as AgCl(s)‚ until all of the Cl- is consumed (assuming Cl- is the limiting reagent). A small amount
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allowed the PbCl2 to dissolve. The supernatant fluid containing the Pb(II) ions was then separated from the solid mercury(I) ions and solid silver ions decanting‚ adding a drop of acetic acid to the supernatant fluid‚ and also adding two drops of K2CrO4 to the test tube. A milky yellow mixture was observed as this indicated the presence of the lead (II) ion. This insoluble yellow precipitate was the insoluble compound of PbCrO4. In part 2 of the experiment‚ after the supernatant
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Salt from green beans Name: Ashni Couprie and Dennise Susanto Class: 5c Introduction From previous experiments we ’ve learned that salt is extracted from green beans. To be more specific: salt is extracted from when the beans are cooked in water in which salt has been dissolved. This experiment is based upon the osmoses theory. According to this theory the cell walls of the green beans are what we call a semi permeable membrane. This membrane only lets water through and not the substance
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the added solutions were also clear and colorless. |AgNO3 (aq) by itself |Colorless solution | |AgNO3 (aq) with NH3 (aq) |Colorless solution | |AgNO3 (aq) with Na2CO3 (aq) |Pale yellow precipitate | |AgNO3 (aq) with NaCl (aq)
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BSc Pharmaceutical Technology Practical - No 5 Preparation of a Primary Standard Solution Aim: to prepare a standard solution of pure silver nitrate and use it to determine the concentration of chloride ions in a sample of tap water and another sample of bottled water. Chemicals: * High grade purity silver nitrate * Potassium chromate indicator * Tap water * Bottled water * Distilled water Apparatus: * Laboratory oven * Dessicator * Conical flask
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Chemical Reactions Lab Introduction Four different types of chemical reactions were observed in this lab. Synthesis reactions occur when two different elements or compounds form a more complex compound as shown by equation (1). Single replacement occurs when one element replaces another to form a new compound as shown in equation (2). Double replacement occurs when two different atoms in different compounds trade places with one another to form two new compounds as shown in equation (3).Combustion
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Lab chemisty 03/27/2011 Five unlabeled bottles Set 1: A) colorless B) colorless C) blue D) blue E) colorless A: Ba(NO3)2 B: AgNO3 C: CuSO4 D) CuCl2 E) KCl Description how to identify solution: _ We have two blue solution which are CuSO4 and CuCl2 or C and D‚ according to chemical reaction experiment‚ C didn’t have any reaction with other solution like B and D beside A‚ so if we look at the solubility
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are all more reactive than copper. ● (2) I believe this solution to be Sodium Sulfate because of the following reasons: ○ Blah blah blah ○ Blah blah ○ blah blahhh Unknown 1 ● NaCl ○ ○ ○ ○ ○ Unknown 2 yellow flame 7 ph precip with agno3 therefore one of the halides (cl‚ br‚ i) white solid from evaporation conductive ● Water ○ no residue when evaporated ○ almost neutral ph ■ ^my group got pH 9 tho?? ○ no conductivity there was conductivity for 2 contamination could have been present causing the conductivity
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halide‚ we are adding drops of Ca(NO3)2‚ AgNO3‚ AgNO3 + Na2S2O3‚ and NaOCI + Starch to the halides. Each halide will be separated from each other and the drops of each compound will be added to the halides‚ but it is one compound for one of the four halide rows‚ each compound will be in a different column. Hypothesis: If I mix drops of different compounds with halides found in
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