of the components of a buffer. For a given addition of acid or base‚ the buffer component concentration ratio change less when the concentration are similar than what they are different. Materials: Acetic acid (MW=60 g/mol)‚ NaOH solution (0.5M)‚ HCl solution (0.001M)‚ calibration buffer (pH3.5 and pH 5.5)‚ 7-UP‚ 100 Plus. Apparatus: pH meter‚ pipettes (10mL)‚ volumetric flask (250mL)‚ beakers (150mL)‚ burettes‚ burette holder and stand‚ funnel‚ graduated
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experiment. Reaction Equation: NaHCO3(s) + HCl(aq) ( NaCl(s) + CO2(g) + H2O(l) Materials: safety glasses baking soda (NaHCO3) 1 M HCl and dropper 500 ml Pyrex flask hot plate Procedure: 1. Find the mass of the 500 ml Pyrex flask. Record this mass in the Data Tables. 2. Add one teaspoon of baking soda to the flask‚ and record the total mass in the Data Table. 3. Use the dropper to drip HCl into the flask. Add HCl until the fizzing ceases. 4. Set the flask
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Discovering the Mystery of Eleven Test Tubes Karen Radakovich Ph.D. Mohammad Farhad Brittany Cina CH 223‚ Spring 08 Abstract: Eleven mystery test tubes labeled from K-1 to K-11 contained: 6M H2SO4‚ 6M NH3‚ 6M HCl‚ 6M NaOH‚ 1M NaCl‚ 1M Fe(NO3)3‚ 1M NiSO4‚ 1M AgNO3‚ 1M KSCN‚ 1M Ba(NO3)2‚ 1M Cu(NO3)2 respectively. The contents of the test tubes were determined by chemical experiments. Solution K-1 contained NiSO4 because when solution K-9‚ ammonia which was identified by its pungent odor
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saturated solutions described above. Since the solution is basic when the phenothelain is added a pink color is observed titrate it with HCL to find the equivalence point‚ which a clear color is shown. In each titration a pink color is observed and once HCL is added the equivalence point is reached the pink color disappears. Results Trial Mg(OH)2 (mL) HCl (mL) HCl (moles) Mg(OH)2 (moles) OH- (moles) Mg2+ (moles) 1 50mL 7.70mL 0.0000154 0.0000077 0.0000154 7.7x10-6 2 50mL 7.95mL 0.0000159
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Experiment # 4: Analysis of Soda Ash Experiment # 5: Volumetric Analysis of a Carbonate – Bicarbonate Mixture Submitted by: Eugenio December 2012 Department of Chemical Engineering University of Santo Tomas España‚ Manila Abstract Soda ash is the common name for sodium carbonate (NaCO3)‚ a chemical salt derived from carbonic acid. It is frequently used in manufacturing‚ industry‚ and in domestic chores. Glass production is one of the primary industrial uses for sodium carbonate. It is also
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number of moles of HCl reacted with the NaOH is 0.00216 moles‚ which is less than Gaviscon. The number of moles of NaOH that were added from the burette is 0.00327 moles (1 tablet of Gaviscon). However‚ for Quick-eze‚ the number of moles is 0.00216 moles (1 tablet). This means the average volume of the NaOH have affected the number of moles as the concentration of the sodium hydroxide is 0.1M. This means that if less NaOH was required to neutralise the acid‚ the number of moles of HCl neutralized by
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This lab will investigate these affects on the rate of a specific reaction. Aim: How does the concentration of HCl affect the rate of the following reaction? CaCO3 (s) + 2HCl (aq) CaCl2 (aq) + CO2 (g) + H2O (l) Variables: Independent variable: Concentration of HCl Dependent variable: Amount of CO2 produced Controlled Variables: Temperature of the room‚ and the HCl No stirring or shaking of the experiment at any times The same type test tube should be used in each trial Try
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Acid | PART I | Solid Acid | Base (NaOH) | Ratio: volume base/ mass acid | Final mass or volume | .70g | 38 ml | 38 ml / .70g | Initial mass of volume | .70g | 0.0 ml | | Mass or volume | .70g | 38 ml | | Titration of HCL | PART II | Acid (HCL) | Base (NaOH) | Ratio: volume base/ volume acid | Final volume | 10 ml | 4.8 ml | 4.8ml / 10ml | Initial volume | 0.0 ml | 0.0 ml | | Volume | 10 ml | 4.8 ml | | Calculations Part I Solid Acid- KHC4H4O6- 188g - .0037mol
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titration of a 25.00 mL sample of H2PO4 buffer solution with 0.1 M HCl and 0.1 M NaOH. The volume of 0.1 M HCl is about double of the amount 0.1 M NaOH used to lower/raise the pH of a blood buffer. In this experiment‚ HCl (a strong acid) and NaOH (a strong base) are used as examples of strong acids/bases‚ and the titration with H2PO4 shows the effect on a buffer solution. The assumption was the addition of large amounts of HCl will lower the pH‚ while the addition of large amounts of NaOH will
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gastric acid (HCl). In order to determine which antacid is the more effective‚ four different brands of antacids were chosen‚ and tested. The purpose of an antacid is to balance out the pH inside a person’s stomach. PH is the measurement of molar concentration of hydrogen ions that are present in the solution (N. Tro‚ 733-735). If this experiment were to be repeated‚ it would be to show which antacid would be more effective to buy as a consumer. In this experiment an antacid is dissolved in HCl‚ and then
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