Redox Titration Lab ABSTRACT: In this lab‚ 0.010 M purple-colored potassium permanganate solution was standardized by redox titration with iron (II) ammonium sulfate hexahydrate (FAS). The average mass of the three flasks of FAS was 0.483 grams. Once the concentration of the standard solution of KMnO4 (aq) was determined‚ it was used to determine the concentration of Fe2+ in iron pills. On average‚ there was 0.01813 L of solution used. With this information and the balanced net-ionic equation
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Silver Nitrate Titration Introduction This experiment was conducted to work out the concentration of the chloride ions in the school swimming pool water and to see if it fits in the required range of concentration of chloride ions in the swimming pool water. This was done by titrating a small sample of the school swimming pool water with silver nitrate‚ which would form a white precipitate of silver chloride. The equation of this process is: The end point of the titration (when all of
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Chemistry 12 12/Oct/2011 Titration- Analysis of Aspirin Tablets Objective: Determine the percentage of aspirin (acetylsalicylic acid) present in two different commercial tablets by titrating the solution with a base. Also determine whether the aspirin is a strong or weak acid according to the Bronsted- Lowry and Lewis theories and deduce the formula of the acid- base reaction. Independent Variable: The amount of base (NaOH) in moles that are needed to neutralize the solution. Dependent Variable:
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Neutralization Titrations: The Determination of Sodium Carbonate from Unknown Soda Ash Unknown # I. Purpose: The goal of this experiment is to determine the weight % of Na2CO3 through the preparation of NaOH and HCl standards. The molarity of the standards will be found through titration of KHP for NaOH‚ HCl vs the known NaOH‚ and the unknown Soda Ash sample vs the known HCl. II. Equations and Sample Calculations: Titration of HCl with NaOH: Complete Equation: HCl (aq) + NaOH (aq)
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Preparation of Sodium Chloride through titration Abstract: acid-base titration is a technique commonly used to determine the moles of acid in a sample by adding a known volume of strong base of a known concentration. The strong base provides the hydroxide ion‚ to react quantitatively with the acid. The point at which the acid is completely and exactly consumed the known quantity of base is called the equivalence end point and is signalled by a colour change in the solution (end point). This colour
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Data‚ Results‚ Calculations and Discussions Preparation of 250-mL 0.1 M NaOH Solution: Wt. of NaOH= (vol. of Sol’n) (M of Sol’n) (MW of NaOH) = (250 mL) (0.1 M NaoH) (40.0g/mol NaOH) Wt. of NaOH= 1.00 g • One gram of NaOH pellets was weighed and dissolved in distilled water. The solution was diluted to 250 mL. Table 1.Weighing of KHP (weighing by difference) |Replicate |Wt. of container -sample‚ g |Wt. of KHP
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Potentiometric Titrations Accuracy The accuracy of a potentiometric analysis is limited by the measurement error for the cell’s potential. Several factors contribute to this measurement error‚ including the contribution to the potential from interfering ions‚ the finite current drawn through the cell while measuring the potential‚ differences in the analyte’s activity coefficient in the sample and standard solutions‚ and liquid junction potentials. Errors in accuracy due to interfering ions
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Title: ACID BASE TITRATION. Objectives: 1. To determine the concentration of acid using titration. 2. Skills of titration techniques. Apparatus: 1. 250 volumetric flask 2. 10mL measuring cylinder 3. 25mL pipette 4. 50mL burette 5. 250mL beaker 6. 150mL conical flask 7. Retord stand 8. White tile 9. Stopwatch 10. Pipette bulb Chemicals: 1. HCl solution 2. 0.1M NaOH solution 3. H2SO4 solution 4. Distilled water 5. phenolphthalein
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12.097 Environmental Chemistry of Boston Harbor – IAP 2006 Lab 1: DETERMINATION OF DISSOLVED OXYGEN BY WINKLER TITRATION 1. Background Knowledge of the dissolved oxygen (O2) concentration in seawater is often necessary in environmental and marine science. It may be used by physical oceanographers to study water masses in the ocean. It provides the marine biologist with a means of measuring primary production - particularly in laboratory cultures. For the marine chemist‚ it provides a measure of
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EXPERIMENT 3: INTRODUCTION TO TITRATION – DETERMINATION OF THE MOLARITY AND CONCENTRATION OF SULPHURIC ACID BY TITRATION WITH A STANDARD SOLUTION OF SODIUM HYDROXIDE INTRODUCTION Reaction of acid and base is one of the most common reaction in chemistry. This reaction is also widely known as neutralization. In this experiment‚ we used titration technique which involves accurately measuring the volume of a solution required to react with another reagent. An indicator must be used to determine the
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