Calculations Mass percent of water in CuSO4·5H2O using experimental data: (mass of water lost / mass of hydrated salt) x 100 (0.658 / 2.009) x 100 = 32.75 % Mass percent of water in CuSO4·5H2O using theoretical data: (90 / 249) x 100 = 36.14 % Percent error using experimental and theoretical mass percentages: (experimental value – theoretical value / theoretical value) x 100 (32.75 – 36.14 / 36.14) x 100 = 9.38 % Average percent water in CuSO4·5H2O using experimental values: (trial 1 % water +
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Experiment 3: Solution Calorimetry: Thermodynamics of Potassium Nitrate II. Abstract A determination of thermodynamic variables of KNO3 is presented. KNO3 was heated and dissolved in varying volumes of distilled water. Upon dissolution‚ the KNO3 solution was removed from heat and the temperature was recorded once crystals formed. For each solution‚ ∆G the Ksp were found with the temperature and molarity values. ∆H and ∆S were found through the linearization of the data with
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The investigation was designed to determine the effect of the addition of increasing concentrations of a miscible liquid (ethanol) on the solubility of KNO3 in water. The results of the investigation support the hypothesis that water‚ which exhibits greater polarity‚ is able to dissolve a greater mass of KNO3 at lower temperatures compared to tested concentrations of Ethanol ranging from 12.5% to 30%. Furthermore‚ the results of the graph 1 show correspondence to the dielectric constant of each solvent
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Copper (II) Sulfate Purpose: The purpose of this lab is to find out how many moles of water there are in one mole of Copper Sulfate (CuSO x HO) and the percent by mass of water in the hydrate. This will be accomplished by heating a determined mass of the hydrate to remove the water‚ and by measuring the salt left over. Introduction: This laboratory experiment will be done to find out how many moles of HO are present per one mole in the hydrate CuSO. A hydrate is a compound that has a fixed number
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F6/7 Chemistry Practical: Enthalpy of hydration of copper(II) sulphate Objective: To determine the enthalpy of hydration of copper(II) sulphate Group size: Individual Introduction This experiment enables an approximate determination of the enthalpy of hydration of copper(II) sulphate to be made. The enthalpy change when one mole of anhydrous copper(II) sulphate is dissolved in water is first determined. Secondly‚ the enthalpy of solution of copper(II) sulphate pentahydrate in water is determined
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water. An example can be hydrated copper (II) sulfate. Exactly this salt is used in the described experiment. RESEARCH QUESTIONWhat is the number of moles of water of crystallization associated with one mole of copper (II) sulfate‚ in the hydrate CuSO4 * xH2O (s)? The independent variable in this experiment is sample thermal treatment ( heating and cooling) and the dependent variable is the number of moles of water of crystallization. A number of other variables can affect the final result of the
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Experiment 9/5 Voltaic cells AIM How the change the concentration of the electrolyte CuSo4 (solution of ions) affect the voltage of the electrochemical cell BACKGROUND An electrochemical cell is also called a voltaic cell‚ which derives electrical energy from redox reaction taking place within the cell. It consists of two different metals that are connected by a salt bridge. Eletrons always flow from anode to cathode‚ where anode is negative (reduction) and cathode is positive (oxidation)
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physical process es. The enthalpy and entropy changes of a system undergoing such processes are interrelated by the change in free energy‚ ªG‚ according to the equation ªG = ªH - T ªS (1) This investigation focuses on the reaction Zn(S ) + CuSO4(aq) Y ZnSO4(aq) + Cu(S ) (2) ªG will be calculated from the ªH and ªS values obtained electrochemically. The validity of Equation (1) will be tested by comparing the value of ªH obtained electrochemically with the value of ªH obtained
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2H2O 2NH4+ + OH- + 2H+ + SO4-2 → 2NH4+ + SO4-2 + 2H2O OH- + 2H+ → 2H2O(l) Aqueous ammonia is ammonia in water. Aqueous ammonia reacts with sulfuric acid‚ which then forms the salt ammonium sulfate and water. This is a neutralization reaction. 7. CuSO4 + Zn(NO3)2 → Cu(NO3)2 + ZnSO4 Cu+2 + SO4-2 + Zn+2 + 2NO3- → Cu+2 + 2NO3- + Zn+2 + SO4-2 All are cancelled out as spectator ions‚ so as observed there was no reaction that took place. 8. Na2CO3 + CaCl2 → 2NaCl + CaCO3(s) 2Na+ + CO3-2 + Ca+2 + 2Cl-
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procedure similarities with redox titration INTRODUCTION Determining the endpoint from a potentiometric redox titration curve: EXPERIMENTAL Preparation of Cu/Cu2+ Reference Electrodes 5 cm Pasteur pipet: plugged with cotton saturated KCl/KNO3‚ 0.1 M of CuSO4 solution Copper wire voltmeter Modelling clay EXPERIMENTAL Preparation of KMnO4 weight of KMnO4 = ? 300 mL of 0.01 M solution Dissolve in 100 mL distilled water. Dilute to reach 300 mL. Store in a colored container. EXPERIMENTAL Standardization
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