0.88g H2O × 0.68% = 0.005984g H2O 0.88g ±0.005984g H2O CuSO4: 63.55 + 32.07 + 16.00(4) = 159.62g1 mol (n)(Hydrated CuSO4): 2.12g CuSO4 ×1 mol CuSO4(s)159.62g CuSO4(s) = 0.01328 mol Hydrated CuSO4 H2O: 16.00 + 1.01(2) = 18.02g1 mol (n)( H2O): 0.88g H2O ×1 mol CuSO4(s)18.02g CuSO4(s) = 0.04883 mol H2O 0.01328 mol CuSO4 0.01328 mol = 1 CuSO4 0.04883 mol CuSO4 0.01328 mol = 4 H2O Presenting Processed
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Introduction The purpose of this lab was to find the theoretical and experimental percentage yields of the double displacement reaction between the solutions Lead (II) Nitrate (PbNO3) and Potassium Iodide (KI). It is important to obtain amounts of Lead (II) Nitrate and Potassium Iodide as close to 1.44g as possible. This reaction creates Lead (II) Iodide and Potassium Nitrate. The precipitate during this reaction is Lead (II) Iodide. The balanced equation is Pb(NO3)2 + 2KI= PbI2 + 2KNO3. In this
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Hot plate Potassium nitrate Distilled water Description of the Object of the Experiment Potassium Nitrate: The chemical compound potassium nitrate is a naturally occurring mineral source of nitrogen. It is a nitrate with chemical formula KNO3. Its common names include saltpetre (from Medieval Latin sal petrae: "stone salt" or possibly "Salt of Petra")‚ American English salt peter‚ Nitrate of potash and nitre. The name salt peter is also applied to sodium nitrate. Description: Potassium
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5O2(4NO + 6H2O Which of the following statements is correct? A. N is reduced‚ NH3 is oxidizing agent B. O is oxidized‚ O2 is reducing agent C. N is reduced‚ O is oxidized D. N is oxidized‚ O2 is oxidizing agent ____ 3. If 145 g of KNO3 were added to water to make 1‚500 mL of solution‚ what would be the molarity of the resulting solution? A. 0.956 M B. 1.43 M C. 0.0967 M D. 10.3 M ____ 4. Calculate the molarity of the solution formed by diluting 50.0 mL of 0.436 M NH4NO3
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NaCl(s) Yellow NaCl Red-Orange NaNO3 Dark Orange LiNO3 Red Sr(NO3)2 Dark Red KNO3 Blue-Indigo Ba(NO3)2 Yellow-Green Cu(NO3)2 Green Ca(NO3)2 Red-Orange Ni(NO3)2 Yellow-Green Materials: Nichrome test wire Bunsen Burner 150 mm test tubes (14) 6.0 mol/L HCl Solid NaCl 0.50 mol/L NaCl 0.50 mol/L NaNO3 0.50 mol/L LiNO3 0.50 mol/L Sr(NO3)2 0.50 mol/L KNO3 0.50 mol/L Ba(NO3)2 0.50 mol/L Cu(NO3)2 0.50 mol/L Ca(NO3)2 0.50 mol/L
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TITLE: Solubility and Thermodynamics PURPOSE: The purpose of the lab was to determine the thermodynamics variables of ∆H‚ ∆S‚ and ∆G for the dissolution reaction of potassium nitrate in water. The solubility of potassium nitrate in mol/L was measured over a range of various temperatures by finding out at what temperature crystallization began for solutions of different molarities. Then‚ the equilibrium constant was calculated and a graphical relationship between the natural logarithm of the
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Water Crystallization and the Chemical Formula of a Hydrate Aim: To determine the percent water of crystallization and the chemical formula of a hydrate Materials * 400 ML beaker * Glass rod * 3 to 5 grams of hydrated copper (II) sulfate CuSO4 (crushed) * Bunsen burner * Spatula * Heating pad * Clamp and stand * Electronic balance Procedures Refer to Lab sheet Observations 1. The powder seems to be very bright and shiny before any heating 2. The blue powder are starting
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placed each solution in that position: NaCH3COO‚ HCl‚ HCN‚ NaOH‚ NH3‚ NaCN‚ KNO3‚ H2SO4‚ NH4Cl‚ H2SO3‚‚ NaHCO3‚ Na3PO4 and CH3COOH. In order of increasing pH: Here are my predictions: ACIDS - H2SO4 – - HCL – - H2SO3 – Weak Acid; - CH3COOH – Weak Acid; - NH4Cl – Weak Acid; - HCN- Weak Acid; NEUTRAL - KNO3 – This is neutral BASES - NaCH3COO – This is a weak base;
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H2O = CO2 + 2 H2O Combination 4. AgBr(s) = Ag (s) + Br2(l) = 2 Ag + Br2 Combination 5. Mg(s) + H2SO4 (aq) = MgSO4 + H2 Decomposition Table Three: Formation of Salt via Double Replacement Reaction 0.1 KNO3 * (NO3)2 0.1 M AgNO3 0.1M NaCl Tube 1: KNO3+NaCl Tube 3: Fe(NO3)3+NaCl Tube 5: AgNO3+NaCl Prediction No change No change No change Observation Change:
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Materials 1. Sand 2. CuSO4 · xH2O salt 3. Evaporating dish 4. Analytical balance 5. Small testtubes 6. Drying flask 7. Thermometer 8. Electrical heater Experimental Procedure Results and calculations Mass of Test tube : 15.8945g Mass of Test tube + CuSO4 ∙ xH2O salt : 17.6698g Mass of Test tube + CuSO4 ∙ xH2O salt after heat for
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