Jacob Hernandez October 23‚ 2014 Hima Lahari Marneni CHEM 1411. 114 Post Lab Report 6 Introduction The purpose of this lab is to determine the concentration of HCl when titrated with a standardized NaOH solution‚ through means of the titration method. My hypothesis is When an unknown concentration of HCl is titrated with a known volume of standardized NaOH solution‚ one can gather enough data to determine the concentration of the unknown (HCl). My prediction is If an unknown concentration of HCl
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------------------------------------------------- Purpose: The purpose of this lab was to use acid-base titrations to find the mass percent of ascorbic acid in a Vitamin C tablet. A known concentration of sodium hydroxide was used and the value found was compared to the stated amount of ascorbic acid listed on the vitamin container. Also in this lab the acidity of different salt solutions were tested using different indicators including litmus paper. Procedure: (titration) 1. Weigh a vitamin C tablet‚ record it’s mass‚ then use a
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of aspirin aspirin present in different commercial preparations and to find out‚ which the best value is‚ using a neutralization reaction followed by a direct titration with NaOH. Chemicals Used: 100 ml of distilled water in a wash bottle 50 ml of 0.100 M NaOH 40 mL of 96% ethanol phenolphthalein as an indicator (3 drops per titration) 325 mg non buffered aspirin tablets Materials Used: One spatula Two Erlenmeyer flasks‚ 250 ml One weighing scale (with uncertainly +-0.005g) 1000 ml graduated
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disorders and kidney stones. (Food Science and Technology Strand 2015) L-ascorbic acid L-dehydroascorbic acid (Sánchez 2013) In this experiment‚ we use titration method (volumetric analysis) to determine the centration of vitamin C in packaged fruit juice samples such as the mango‚ apple‚ passion fruit and orange juices in this experiment. Titration is a commonly used method of quantitative analysis which can determine the concentration of a known analyte (reactant). In this case the reactant is vitamin
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EXPERIMENT 10 POTENTIOMETRIC REDOX TITRATION BAUTISTA ‚ Anne Judith LARIN‚ Michelle V. OBJECTIVES At the end of the experiment‚ the student should be able to: 1.Construct a potentiometric redox titration curve 2.Determine the % Fe in a sample by potentiometric redox titration INTRODUCTION Potentiometry definition indicator electrode reference electrode Potentiometric titration applications general procedure similarities with redox titration INTRODUCTION Determining the endpoint
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Water Hardness 9/12/2013 Abstract: Two sets of acid-base neutralization titrations were conducted for experimental analysis. The first set of titrations was to standardize a solution manufactured in the lab. An approximate solution of Na2EDTA of 0.004 M was titrated against a known solution of 1.000 g CaCO3/L to deter mine to exact molarity of the Na2EDTA. Ca2+ + Na2EDTA → CaEDTA + 2Na+ The second set of titrations was to use the now standardized Na2EDTA solution to determine an unknown water
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Abstract Water “hardness” was analyzed in this experiment‚ through the determination of CaCO3 concentration. This was achieved by the titration of an unknown solution using a standardized 0.1M EDTA‚ and addition of Eriochrome Black T to the unknown‚ to indicate the endpoint of the titration. The average concentration of CaCO3 obtained was 1034 ppm‚ with a standard deviation of 2.4495. The results indicate that the unknown solution can be considered as hard water. Introduction The
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indicate the end point of a titration) titrations as it forms stable complexes with most metal ions. EDTA is a tetracorboxylic acid and in alkaline conditions‚ it exists as Y⁴⁻ ions‚ which form 1:1 complexes with metal ions like nickel(II) ions: Y⁴⁻ + Ni²⁺ NiY²⁻ A metal ion indicator (an organic dye which changes colour when it binds with metal ions) shows the end of an EDTA complexometric titration. However‚ for a metal ion indicator to be suitable in n EDTA titration‚ it must not bind as strongly
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Title: Determination of chloride by the Mohr Method Objective: To determine chloride by using Mohr Method. Introduction: The Mohr method is the method used to determine the chloride ion concentration of a solution by titration with silver nitrate. As the silver nitrate solution is slowly added‚ a precipitate of silver chloride forms. Ag+ + Cl- AgCl(s) (Ksp for AgCl is 1.810-10) The chloride ion (Cl-) is an important anion found in solids and solutions. Chloride is the predominant anion
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quantitative analysis using the technique of titration. You are going to analyse an iron tablet to find out how much iron is actually present in it. Titrations involving potassium manganate(VII) may form part of your Practical Assessment. Intended lesson outcomes By the end of this practical you should be able to: • perform a titration involving potassium manganate(VII); • read a burette and use a pipette; • use a volumetric flask; • record your titration results appropriately in tables you have drawn
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