Experiment 11: Synthesis of Dibenzalacetone by the Aldol condensation Introduction: The Aldol condensation reaction‚ under basic conditions‚ involves the nucleophilic addition of an enolate ion to another carbonyl group. The resulting product‚ a beta-hydroxy ketone or aldehyde‚ is called an aldol because it contains both and aldehyde group and the hydroxy group of alcohol. Condensations‚ including aldol condensation‚ combine two or more molecules‚ typically with a loss of a smaller molecule (including
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JSUNIL TUTORIAL ‚ SAMASTIPUR‚ BIHAR IX CBSE CHAPTR - ATOMS AND MOLECULES The word atom is derived from the Greek word “Atomos” which means indivisible. John Dalton modelled atoms as hard indivisible spheres. An Indian philosopher Maharishi Kanad‚ postulated that if we go on dividing matter (padarth)‚ we shall get smaller and smaller particles. Ultimately‚ a time will come when we shall come across the smallest particles beyond which further division will not be possible. He named these particles
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which contained 2 drops of orange methyl identifier. Once the titration began‚ the HCl was added until the methyl orange endpoint was reached‚ and as a result the volume of the HCl needed for the endpoint to be reached could be used in determining the moles and in turn the molar solubility and the solubility constant of the Ca(OH)2. For the second part of the experiment a common ion (CaCl2) was added to the calcium hydroxide and the process was repeated to analyze how the common ion would affect the molar
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Hardness of Water by EDTA Titration Introduction Water hardness is caused by natural minerals that are dissolved into the water‚ predominantly calcium and magnesium‚ and is measured as the equivalent concentration of calcium carbonate (in milligrams per litre). Water hardness is usually noticed because of difficulty in lathering soap and the formation of a scum in the bathtub. Ca2+ and Mg2+ form insoluble salts with soaps causing precipitation of the soap scum. Another effect of hard water
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nails. There are 2 different oxidation numbers for iron; that are 2 or 3. We will need to check each of the equations to find out the moles of each element in the equation. Then we can compare the ratio between the mole and the mass of iron and copper; that will be measured during the experiment. Finally because of the balanced equation the ratio of the mass and the mole has to be the same; by this we can check the actual equation and the actual oxidation number of iron in this reaction. This process
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Aim To Find the Number of Moles of Water of Crystallisation in Copper (II) Sulphate salt. Introduction Water of crystallisation is the term given to the molecules of water that are used to build up a crystal lattice in some ionic compounds.In copper II sulphate the blue crystals would be impossible without using water molecules to act as ’scaffolding’ within the structure CuSO4.5H2O. When this is heated the water molecules are driven off and the blue crystals become a white powder. As most
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are needed to visualize the end-points. The first indicator is phenolphthalein which will turn from the pink ionic form while in a base‚ to a colorless form indicating the first end-point in this experiment. At this point exactly one mole of HCl has been added per mole of carbonate. This reaction of phenolphthalein occurs from pH 10 to 8.3 which is within 1 pH of the equivalence point for the carbonate to bicarbonate reaction. The second reaction has an equivalence point at ~ pH 3.7. This is where
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substances taking part in a reaction or forming a compound‚ typically a ratio of whole integers. You need to use numerous conversions‚ atomic weights‚ and mole calculations in order to get the grams of each reactant. Atomic weights are the weight of each element on the periodic table; for example‚ Oxygen is 16.00 grams and Carbon is 12.01 grams. Moles are a standard scientific unit for measuring large quantities of very small entities such as atoms‚ molecules‚ or other specified particles. In all Stoichiometry
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ions in solution. The point at which this mole equivalency occurs is known as the equivalence point. An indicator in the solution will change color to signal that the equivalence has been reached (actually‚ the indicator responds to the slightest excess of OH ions). The color change in a titration is called the endpoint. At the equivalence point of the titration‚ the moles of OH (base) are equivalent to the moles of H+ (acid) in the sample. The moles of OH added to the solution from a buret are
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INTRODUCTION EDTA (H₄Y) is widely used to determine metals in complexometric (a volumetric analysis where the formation of a coloured complex is used to indicate the end point of a titration) titrations as it forms stable complexes with most metal ions. EDTA is a tetracorboxylic acid and in alkaline conditions‚ it exists as Y⁴⁻ ions‚ which form 1:1 complexes with metal ions like nickel(II) ions: Y⁴⁻ + Ni²⁺ NiY²⁻ A metal ion indicator (an organic dye which changes colour when it binds with metal
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