EXPERIMENT 4 TITLE Complex Formation and Precipitation. INTRODUCTION Precipitation is the formation of a solid in a solution as the result of either a chemical reaction‚ or supersaturating a solution with a salt resulting in solid material collecting on the bottom of the beaker (Housecroft & Constable‚ 2006). When the solution has been supersaturated by a compound and no more material can be supported by the solution‚ it considered as precipitate. Commonly‚ the solid will fall out of the
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A double displacement reaction is a type of chemical reaction in which two compounds react in order to create two new chemicals. The two cations and anions switch places with each other which forms two new compounds. As an example AB+CC can switch to AD+CB. Both sides of these equations must balance out in order to be neutral. So any pairs of compounds (such as A+B) must have a total balanced charge. In this example A could have a charge of positive 2 (+2) and B could have a charge of negative
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Chemical reactions * Chemical reactions occur when substances undergo chemical changes to form new substances * Production of gas and change of color are sings of chemical reactions * Chemical reactions rearrange atoms * A reactant is a substance or molecule that participates in a chemical reaction * A product is a substance that forms in a chemical reaction Energy and Reactions * Energy must be added to break bonds. * Many forms of energy can be used to break bonds:
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IB HL BIOLOGY Dialysis Lab: Exploring Osmosis and Diffusion Through A Membrane Introduction: Dialysis is the flow of certain solutes through a semi permeable membrane. Dialysis is usually used on patients with failing kidneys to clinically purify blood in their kidneys‚ or other regions of their bodies. The dialysate contains waste matter that flows from the blood our of the dialysis tubing. Question/aim of lab: To test the solutions inside and outside the dialysis tubing with Benedict’s
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Silver Nitrate(AgNO3) 1M Potassium Nitrate(KNO2) Calcium Chloride (CaCl2) Barrium Hydroxide Ammonium Hydroxide (NH3OH) Methylene Chloride Test Tube/Test Tube Holder Eye Dropper Eye Dropper Beaker Pipette Pipette Bulb Litmus Paper Hot Plate Observations/Calculations: CO3 + H2SO4 = bubbly reaction‚ little to no colour change. CO3 + 6M HCl = Barrium hydroxide began to go cloudy‚ indicating the presence of BaCO3(Carbonate anions) Chloride Solution + 0.1M AgNO3 =white precipitate
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Ashley Silva Lab 7: Three Stooges in Chemical Reactions Objective: The purpose of this lab is to experimentally determine the equilibrium constant‚ Kc ‚ for the following chemical reaction: Fe3+ (aq) + SCN-(aq) ↔FeSCN2+(aq) Background Information: A system is at equilibrium when the rate of the forward reaction is the same as the rate of the reverse reaction. There is no change in concentration for the reactants or products at chemical equilibrium. When the system is disturbed there
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ofchemicals and some indicators.The following observations were made: NaHCO3 and HCI – CO2 HCI and BTB NH3 and BTB HCI and blue dye Blue dye and NaOCI NaOCI and KI KI and Pb(NO3)2 NaOH and phenolphthalein HCI and phenolphthalein NaOH and AgNO3 AgNO3 and NH3 NH3 and CuSO4 Data Tables: Data Table 1: ReactionsReaction Question/WellNumberA/H12 Chemicals NaHCO3 and HCI - CO2 When I added the hydrochloric acid to the sodium bicarbonate it began to bubble and fizz almostimmediately
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then quantitatively transferred to a 250ml volumetric flask. Proper technique is needed for quantitative analysis. This transfer was done to ensure that there was no detectable KCl left in the beaker. After transferring the solution add 3 drops of AgNO3 to the rinsed beaked to check the completeness of the transfer. Now take the volumetric flask and add deionized water till it is 6mm away from the etched mark on the neck of the flask. Place a stopper on the top of the flask and invert the flask to
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bottom. Yes NaOH + phenolphthalein It had a light odor and turned pinkish red. Yes HCl + phenolphthalein Nothing occurred it remained the same with a slight odor. Yes NaOH + AgNO3 It turned greenish brown with clumps of solid with no odor. Yes AgNO3 + NH4OH – Observation 1 It turned cloudy white‚ with no odor. Yes AgNO3 + NH4OH – Observation 2 It turned a brownish pink color with no odor. Yes NH4OH + CuSO4 It turned dark purple and Yes
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calculated. AgCl(s) => Ag+(aq) + Cl-(aq) Ksp = [Ag+(aq)]·[Cl-(aq)] = 1.6 x 10-10 Since Ksp is so small the dissolved are to be considered negligible. Both ions will precipitate out very quickly to AgCl when the AgNO3 is added to the solution with the Cl- ions until all of these ions are consumed. Small amounts of salt will still remain in the solution because the maximum solubility to be reached when there is no longer excess Ag+. The remaining Cl- can be calculated
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