Copper Sulfate Pentahydrate

The use of sofid supports in conjunction with permanganate reactions leads to modification of the reactivity and selectivity of the oxidant. The use of an inert support, such as bentonite (see Clays), copper sulfate pentahydrate, molecular sieves (qv) (151), or sifica, results in an oxidant that does not react with alkenes, but can be used, for example, to convert alcohols to ketones (152). A sofid supported permanganate reagent, composed of copper sulfate pentahydrate and potassium permanganate (153), has been shown to readily convert secondary alcohols into ketones under mild conditions, and in contrast to traditional permanganate reactivity, the reagent does not react with double bonds (154). 

ChemicalDesignations-Synonym Blue Vitriol Copper Sulfate Pentahydrate Cupric Sulfate Sulfate of Copper Chemical Formula CuS04-5Hj0. 

Tanimoto, A.K., Kobayashi, K. and Fujita, S., 1964. Overall crystallization rate of copper sulfate pentahydrate in an agitated vessel. International Chemical Engineering, 4(1), 153. 

A large number of inorganic compounds crystallize as hydrates. One of the most familiar examples is copper sulfate pentahydrate, CuS04-5H20. Like most hydrates, when this material is heated it loses water, but because all of the H20 molecules are bound in different ways, some are lost more easily than others. Therefore, as the solid is heated the reactions observed first are... 

Most solvents have unshared pairs of electrons, and they are polar. Therefore, they have the ability to attach to metal ions or interact with anions. As a result, when many solids crystallize from solutions, they have included a definite number of solvent molecules. When this occurs in water, we say that the crystal is a hydrate. An example of this is the well-known copper sulfate pentahydrate,... 

Sodium Nitrotetrazolate Dihydrate (NaNT) Anhydrous aminotetra-zole (8.48 g, 0.10 mol) and copper sulfate pentahydrate (0.2 g, 0.8 mmol) were added to a solution of nitric acid (9 mL, 65 %) in distilled water (60 mL). This was added to a pre-cooled solution of sodium nitrite (20.8 g, 0.30 mol) and cupric sulfate pentahydrate (11 g, 0.044 mol) in distilled water (100 mL). The solution was maintained at 15 to 18 °C during the addition by means of a cool water bath. After addition, the solution was stirred for 30 min at the same temperature... 

Fig. 72. Photometer curves of X-ray photographs taken during the decomposition process of copper sulfate pentahydrate...

Zinc. Next to sodium, zinc is the most used reductant. It is available in powder, dust, and granular (mossy) forms. Zinc gets coated by a l er of zinc oxide which must be removed to activate it before it can reduce effectively. It can easily be activated by shaking 3 to 4 min. in a 1% to 2% hydrochloric acid solution. This means for every 98 ml of water volume, add 2 ml of coned hydrochloric acid. Then wash this solution with water, ethatiol, acetone, and ether. Ot activation can be accomplished by washing zinc in a solution of anhydrous zinc chloride (a very small amount) in ether, alcohol, or tetrahydrofuran. Another way is to stir 180 g of zinc in a solution of 1 g copper sulfate pentahydrate. Personally, I like the HCl acid method. 

Zinc dust is frequently covered with a thin layer of zinc oxide which deactivates its surface and causes induction periods in reactions with compounds. This disadvantage can be removed by a proper activation of zinc dust immediately prior to use. Such an activation can be achieved by a 3-4-minute contact with very dilute (0.5-2%) hydrochloric acid followed by washing with water, ethanol, acetone and ether [/55]. Similar activation is carried out in situ by a small amount of anhydrous zinc chloride [156 or zinc bromide [157 in alcohol, ether or tetrahydrofuran. Another way of activating zinc dust is by its conversion to a zinc-copper couple by stirring it (180g) with a solution of 1 g of copper sulfate pentahydrate in 35 ml of water [/55]. 

For assay solution B Dissolve 624 mg copper sulfate pentahydrate (CuS04 5H20) and 631 mg L-serine with stirring. Bring to 500 ml with distilled water in a volumetric flask. Store in a dark bottle up to 1 month at 4°C. 

Prepare a solution of 12 g sodium potassium tartrate and 24 g anhydrous sodium carbonate in 250 ml distilled water. Add a solution of 4 g copper sulfate pentahydrate and 16 g sodium hydrogen carbonate in 200 ml distilled water. Separately, prepare a solution of 180 g anhydrous sodium sulfate in 500 ml of boiling distilled water. Combine the two solutions in a volumetric flask and dilute the final solution to 1 liter. Store up to 1 year at room temperature. 

Timeliness and duration certain control methods are effective only in earliest stages of a bloom, and the effect is short-lived. Copper sulfate pentahydrate, has been found to be effective in killing off small patches of G. breve in early stages of a bloom, but copper sulfate cannot be used to control the organism when blooms cover many square miles of the sea. The cost estimates vary, but a value of about 1050 per square mile was reported. Using activated charcoal to absorb hormones and vitamins required by G. breve has been suggested, and cost estimates (based on 3 tons of activated charcoal) are 150-810 per square mile (34). 

A These blue crystals of copper sulfate pentahydrate contain the Cuy+ cation and the polyatomic SO42- anion. 

Potassium permanganate adsorbed on copper sulfate pentahydrate oxidizes dithiol 112 into 1,2-dithiepane 113 (Equation 35) <1998S1587>. 

Copper sulfate pentahydrate CuS04-5H20 Insecticide, medicinal battery cells... 

Potassium phosphate monobasic Magnesium sulfate heptahydrate Calcium chloride dihydrate Zinc sulfate heptahydrate Ferric sulfate heptahydrate Copper sulfate pentahydrate Cobalt(II) chloride hexahydrate Perchloric acid Potassium hydrocarbonate... 

A student repeated the experiment you just finished and recorded the following data for copper sulfate pentahydrate ... 

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