Investigation 14 Chemistry 113 Lab 10/13/2011 1) Method 1: Adding acid NaHCO3 + HCl → NaCl + CO2 + H2O a) Unknown mixture of NaCl and NaHCO3 Mass of unknown mixture (NaCl + NaHCO3) | 3 g | Mass of HCl | 30 .31g | Mass of products ( NaCl + H2O ) | 26.98 g | Calculate mass of CO2 | 6.33g | Calculate mass of NaHCO3 | 12 .1 g | i) Calculation : Mass of CO2 = [Mass of unknown mixture (NaCl + NaHCO3) + Mass of HCl ] – [Mass of NaCl + H2O] = (3 g + 30.31 g) – 26.98 g = 6.33g Mass of NaHCO3
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Based on my observation CaCl2 is soluble in water. 2. When 15% of HCl was added to CaCl2 as the teacher was performing the experiment I observed and realized some changes took place physically. It was physical change because the color was clear. 3. By adding 15% of HCl of CaCo3 ‚ made it change chemically‚ I would tell this by effervescence and observation. 4. The most obvious difference is that when CaCl2 was mixed with 15% HCl it changed physically and the solid remain on the filter paper is
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to acetone and HCl and find a value for the rate constant‚ k. Since the concentrations of acetone and HCl are much higher than that of I2‚ the concentrations of acetone and HCl will change very little. Thus the rate will be determined by the time needed for iodine to be used up. Iodine has color so you can easily follow changes in iodine concentration visually. The equation‚ rate = k(A)m(H+)n(I2)p‚ can be simplified to rate = k[I2]/t since the values for acetone and HCl essentially remain
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solution was bulked to the mark and mixed again. Finally‚ the solution was transferred to a clean plastic bottle and labeled. The second part was the preparation of ml 100ml of 3.0 M hydrochloric acid (HCl) solution from a more concentrated (12.1 M) HCl solution. Using a pipette‚ ____ ml of concentrated HCl was transferred to a clean Erlenmeyer flask that already contained around 25ml distilled water. Distilled water was then added until the solution
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1411-76426| Data Tables: Part 1: |Chemicals|Well No.|Observations of the Reaction| A.|NaHCO3 + HCl|1 |clear bubbles formed| B.|HCl + BTB|2 |turned orange after BTB was added‚ transparent‚ acidic| C.|NH3 + BTB|3 |turned dark blue after BTB was added‚ opaque‚ basic| D.|HCl + blue dye| |blue dye was missing from kit| E.|Blue dye + NaOCl| |blue dye was missing from kit| | with the 1 drop of HCl| || F.|NaOCl + KI|4 |small white precipitate‚ color changed to black after starch was added |
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Introduction In this chemical reaction‚ the magnesium will dissolve in the hydrochloric acid to produce hydrogen gas. This is because magnesium is higher than hydrogen in the reactivity series. Therefore‚ when the two reactants are combined‚ a displacement reaction occus and the magnesium displaces the hydrogen‚ forming magnesium chloride and hydrogen gas. Mg (s) + 2HCl (aq) -> MgCl 2 (aq) + H 2 (g) Magnesium + Hydrochloric acid -> Magnesium Chloride + Hydrogen
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concluded with 0.54M of NaOH. The results of trial 1 and 3 resemble the most similar and consistent to the expected results of the experiment. Discussion of Theory: The lab as able to determine the concentration of NaOH by neutralizing the solution with HCl‚ a solution which its concentration was already known‚ this process is called titration. It works by neutralizing a solution from a weak acid/base and its
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to prepare 50 mL of buffer dissolve 23.6 g of Guanidine thiocyanate (118.16 g/L) in 25 mL of double-distilled water. Once dissolved add: 2.5 mL of 1 M Tris-HCl pH 7.0 (121.14 g/L)‚ 2 mL of 0.5 M EDTA pH 8.0 (186.12 g/L) and 0.05 mL of Triton X-100. Add double-distilled water to 50mL (final concentrations: 4 M guanidine thiocyanate‚ 50 mM Tris-Hcl pH 7.0‚ 20 mM EDTA and 0.1 % Triton X-100). 36. DNA Binding Solution: First‚ wash diatomaceous earth (silica particles) by resuspending 5 g in 50 mL of water
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Abstract This lab is performed in order to determine the total energy in a reaction between zinc and hydrochloric acid. The reaction is done twice‚ once to measure the heat of the reaction and again to determine the work done in the system. This is because Enthalpy equals heat plus work (∆H= ∆E+W). Heat and work can be broken down further into separate components so the equation used in lab is ∆H=mc∆T + PV. Many calculations are used in the lab to find out what cannot be measured directly (ex:
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acid to cancel out and the weakest will need more acid. Variables: Control | Independent | Dependent | The indicator‚ NaOH | H2SO4 HClHNO3 | The chemical reaction between the acids and alkali. | Materials / Apparatus: * H2SO4 * HCL * HNO3 * Alkali (NaOH) * Stand * Burette * Beaker * Funnel * Bunsen Burner * Crucible * Phenolphyalein Method: 1. Pour the 25 ml of NaOH into a beaker. 2. Drop three drops of phenolphyalein into the beaker
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