solids hydrates‚ and we call the bound water the water of hydration. A hydrate has a definite number of water molecules bound to each anhydrous salt unit. The formula of the hydrate copper(II) sulfate pentahydrate is CuSO4 · 5 H2O The dot indicates that the molecules of water are attached to the ions in CuSO4 by weak bonds. We can drive off the water of hydration by heating the hydrate. If blue CuSO4 · 5 H2O is heated‚ the water of hydration is released as water vapor‚ and solid white anhydrous CuSO4
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water were also converted into moles and utilized to compute the molar ratio of the unknown sample. The ratio for these samples were calculated at a low 2:1 and a high of 12:1‚ water to calcium sulfate; the empirical formulas were CaSO4·2H2O and CaSO4·12H2O respectively. The determined percent mass of hydration was 19.85% and
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Reactions which release energy are described as exothermic and those which absorb energy are endothermic. The energy released in chemical reactions was previously stored as chemical potential energy in the reactants; this stored energy is called enthalpy. The aim of this practical is to observe and classify chemical processes as endothermic or exothermic‚ based on the changes in temperature measured and the observations made. If a chemical reaction produces products with more chemical potential
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THE s-BLOCK ELEMENTS 291 UNIT 10 THE s -BLOCK ELEMENTS The first element of alkali and alkaline earth metals differs in many respects from the other members of the group After studying this unit‚ you will be able to • describe the general characteristics of the alkali metals and their compounds; • explain the general characteristics of the alkaline earth metals and their compounds; • describe the manufacture‚ properties and uses of industrially important sodium and calcium
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IONIC COMPOUNDS In chemistry‚ an ionic compound is a chemical compound in which ions are held together in a lattice structure by ionic bonds. Usually‚ the positively charged portion consists of metal cations and the negatively charged portion is an anion or polyatomic ion. Ions in ionic compounds are held together by the electrostatic forcesbetween oppositely charged bodies. Ionic compounds have high melting and boiling points‚ and they are hard and very brittle. Ions can be single atoms‚ as the sodium and chlorine in
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the formula Ccal = -(ΔHwater * nLR) / ΔT (eq 1) where ΔHwater is the enthalpy change of water. This is equal to -55.81 kJ/mol. nLR is the number of moles of the limiting reactant‚ and ΔT is the change in temperature associated with the reaction. The Ccal obtained was later used to determine the experimental values of the enthalpy change of the reactions (ΔHrxn). Six other reactions were also used to determine its enthalpy change. The reactions are: Neutralization: a. Ammonia and hydrochloric
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materials using cheesecloth. A clean‚ cotton cloth was then subjected to a series of procedures from pretreatment and mordanting down to dyeing with the rnangosteen extract. Alum and copper sulfate were used as mordants. Results revealed that the mangosteen extract was stabilized by both mordants‚ but copper sulfate was a better fixing agent than alum‚ because it intensified the color of the extract. It can be concluded that the mangosteen husk extract can effectively be used as an alternative‚ environment-friendly
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materials using cheesecloth. A clean‚ cotton cloth was then subjected to a series of procedures from pretreatment and mordanting down to dyeing with the rnangosteen extract. Alum and copper sulfate were used as mordants. Results revealed that the mangosteen extract was stabilized by both mordants‚ but copper sulfate was a better fixing agent than alum‚ because it intensified the color of
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2014 Purpose: To determine the identity of an unknown hydrated salt calculating the percent water loss after heating and also to determine the empirical formula of magnesium oxide. Results: Table 1: Determination of the mass of waters of hydration of an unknown hydrated compound. Hydrated Compound code: C-14 Mass (g) Crucible + Lid 30.581g Crucible + Lid + Hydrated compound 31.590g Hydrated Compound 1.004g Crucible + Lid + contents (after 1st heating) 31.122g Crucible + Lid + contents
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could measure the density of atoms with crude experiments. The second part of the experiment dealt with Solubility of large ions and their Hydration enthalpy. Hydration enthalpy is the enthalpy change when 1 mole of an ionic substance dissolves in a solution to give a solution of infinite dilution. (Jim Clark‚ 2010). (Jonathan Hopton‚ 2011) Hydration Enthalpy decreases (gets less negative) down a group‚ the Solubility of the group 2 metals also decreases down the group. Methods The method was followed
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