14 standardization&titration
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Standardization and titration is a quantitative technique that can produce accurate and precise results when done carefully. It involves standardizing a sodium hydroxide (NaOH) solution by performing multiple titrations of a primary standard potassium hydrogen phthalate (KHP) of known molarity. This allows the determination of an unknown concentration of acetic acid by titrating samples with the standardized NaOH solution. Proper experimental procedure and tips are provided to complete the standardization and acetic acid titrations.
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4) Calculating the acid dissociation constant of acetic acid and obtaining 11.43% relative error.
Acid base titration (1)
This document describes the process of acid-base titration to determine the concentration of an unknown solution. A titration involves using a solution of known concentration (the standard solution) to neutralize a precisely measured volume of the unknown solution. An indicator is used to detect the endpoint of the titration reaction. The concentrations and volumes are then used to calculate the concentration of the unknown solution. The document provides instructions for using titration to determine the concentration of sodium hydroxide and white vinegar solutions. Sodium hydroxide is standardized against a primary standard potassium hydrogen phthalate solution before being used to titrate the vinegar.
Acid base titration
An acid-base titration involves using a solution of known concentration (the standard solution) to neutralize a precisely measured volume of an unknown solution. The titration endpoint is detected using an indicator that changes color at neutralization. The volumes and concentrations are then used to calculate the concentration of the unknown solution. This document describes how to use a standard NaOH solution to determine the concentration of vinegar through titration.
CHE107 - class 07 - Pre lab lecture
This document provides instructions for Lab 7 on water quality testing. It discusses titrating calcium, magnesium, and total hardness in tap water samples using EDTA. Students are instructed on the proper procedure, calculations, and safety precautions for the lab. Key points covered include the 1:1 mole ratio of Ca2+/Mg2+ to EDTA, identifying the color change endpoints, and calculating concentrations and water hardness in terms of ppm CaCO3. Students are also directed to review concepts from previous labs on units, significant figures, percent error, and solution preparation.
Field refguide
The document provides water quality monitoring procedures for volunteers with the Texas Stream Team program. It details the steps to calibrate a conductivity meter, take measurements of air temperature, water transparency, total depth, water temperature, conductivity, dissolved oxygen, and pH at a monitoring site. Contact information is given for environmental assistance organizations in case of spills or other issues. The procedures are intended to guide volunteers in properly collecting and recording water quality field data.
Measuring lab
This document describes procedures for measuring various properties including size distribution, mass distribution, concentration, temperature, and volume. The procedures involve carefully measuring samples and recording the measurements and observations. Key steps include choosing a representative sample, using proper measuring tools, accounting for errors and uncertainties, and recording all relevant data. The goal is to obtain large data sets that can be statistically analyzed to evaluate results and understand sources of error.
Micro chemlab
This document describes a laboratory experiment to determine the concentration of hydrogen peroxide in a commercial antiseptic solution through redox titration. Potassium permanganate is used as the titrant to oxidize hydrogen peroxide. By measuring the volume of permanganate needed to reach the endpoint of the reaction, the concentration of hydrogen peroxide can be calculated. The purpose is to verify if the 3% concentration listed on commercial products is accurate. The procedure involves titrating a sample of the hydrogen peroxide solution with a standard permanganate solution and recording the volumes used in multiple trials to calculate an average concentration.
Micro chem
This document describes a procedure to determine the concentration of hydrogen peroxide in a commercial antiseptic solution through redox titration. Potassium permanganate is used as the titrant to oxidize hydrogen peroxide. By measuring the volume of permanganate needed to reach the endpoint of the reaction, the concentration of hydrogen peroxide can be calculated. The purpose is to verify if the 3% concentration listed on commercial products is accurate. The procedure involves titrating a sample of the product against a standard solution of permanganate while monitoring the color change, and using the reaction stoichiometry and volumes to calculate the concentration.
Water analysis and testing
This document provides a summary of various laboratory methods for assessing water quality, including tests for inorganic constituents, hardness, arsenic, alkalinity, pH, biological contaminants, and filtration processes. The methods described include tests for fluoride, iron, sulfate, nitrate, and total dissolved solids. Procedures are outlined for assessing arsenic, alkalinity through titration, and testing for total coliform and E. coli bacteria using UV light and growth indicators. The final section briefly describes a water treatment filter house. The document serves as a training aid for learning water quality analysis techniques.
222 l exp lead in soil - spring 2011
This document provides instructions for an experiment to determine the concentration of lead in soil samples using atomic absorption spectroscopy. Students will analyze three related soil samples and develop a hypothesis about the expected trend in lead concentrations between the samples. They will then prepare lead standards, digest the soil samples to extract lead, and use an atomic absorption spectrometer to measure the lead concentration in each sample. The results will be analyzed to compare the expected and measured trends in lead levels across the samples.
Experiment5 chem210
This document describes procedures for potentiometric titration experiments involving aspirin, vinegar, and sodium carbonate samples. Potentiometric titration uses a pH electrode and reference electrode connected to a pH meter to monitor pH changes during titration. For the aspirin experiment, an aspirin tablet is dissolved and titrated with sodium hydroxide while pH is recorded. The vinegar experiment involves titrating a vinegar sample with hydrochloric acid. For sodium carbonate, the sample produces two equivalence points when titrated with hydrochloric acid due to its carbonate ions. Data analysis involves calculating percent composition and errors from the titration curves and derivative plots.
ELISA tips and tricks - March 2016
ELISA is one of the commonly used laboratory techniques. As it is a multi-step manual technique, every step should be carefully monitored. Here is a short presentation on the common things that should be considered when using ELISA.
Ph meter ppt.pptx
The document describes how to calibrate and use a pH meter to measure the pH of samples. It explains that the pH meter must be calibrated using buffer solutions of known pH before taking measurements. The process involves inserting the electrode into the buffer solutions, allowing the reading to stabilize, and calibrating the meter at pH points of 7.0, 4.2, and 9.6. Once calibrated, the electrode can be rinsed and inserted into samples to measure and record the pH values. Accurately measuring pH is important for various industrial and laboratory applications.
determination of acid in juice
This document provides instructions for determining the acidity of fruit juices through titration and calculating the sugar/acid ratio. It describes obtaining juice samples from fruits, preparing samples by filtering out solids, and titrating the samples with sodium hydroxide solution using either a colored indicator or pH meter to find the endpoint. The amount of acid is calculated using titration values and acid factors. The sugar/acid ratio is then calculated using the acid level and measured Brix value, providing an indicator of fruit ripeness. Safety precautions are outlined for handling the sodium hydroxide and phenolphthalein solutions used.
IB Chem HL Internal AssessmentTo what extent does .docx
IB Chem HL Internal Assessment
To what extent does the mass of an antacid affect its ability
to neutralize the stomach’s pH level?
Introduction
Acid indigestion, more commonly known by the term “heartburn” is a stomach problem caused by the regurgitation of gastric (stomach) acid. Gastric acid is a fluid found in our digestive system, normally with a pH of around 2.0 (highly acidic on the pH scale), as it is primarily composed of HCl, KCl and NaCl and contributes to the breaking down of all the foods we digest. Heartburn results in a painful burning feeling in the chest and its duration can vary from person to person. Other symptoms include feeling as if there is food stuck in the throat and/or a burning feeling in the pharynx.
I chose to examine the pH levels of a few store-bought antacids in relation to a home remedy, in order to determine which of the two types are more effective in the neutralization of gastric acid as it undergoes heartburn, whilst evaluating the mass of each antacid. Antacids usually come in the form of a tablet/pill and are taken to help neutralize stomach acid and reduce symptoms of heartburn, as they are composed of weak bases, such as calcium carbonate or certain hydroxides, for example.
Once I was satisfied with my topic, I was able to derive my research question; To what extent does the mass of an antacid affect its ability to neutralize the stomach’s pH level?
The neutralization process focuses on the reaction of an acid and a base, resulting in the formation of a salt and water. The reaction would look something like this;
HCl + XOH → XCl + H2O
When the basic reactant, NaOH, is dissolved in water, it becomes an alkali. The products are a result of the acid and base reacting, forming water as the H+ and OH– react. The second product formed is a salt, NaCl, in this case, as the sodium (Na) and the chlorine (Cl) ions reacted. The independent variable in this investigation is the mass of the antacids, because I can choose the mass of TUMS tablets and baking soda I use in the experiment, whilst the dependent variable is the change in pH levels of the antacids; the number of acid drops required to neutralize the solution. This is measured by counting the amount of acid dropped from the burette. Also, I controlled the temperature to be constant because that might have affected the final rate of reaction and as a result, altered my data. The constant, or controlled variable, was the amount of HCl used.
Materials:
· Safety goggles
· Store-bought antacid (TUMS)
· Baking Soda
· Mortar & pestle
· Hydrochloric acid
· Balance
· Distilled water
· 6 different 100mL beakers
· Flask
· Universal pH indicators
· pH buffer solutions
· 50mL graduated cylinder
· Burette
· pH meter
Procedure:
1. Safety goggles were used throughout the entire experiment for safety precautions.
2. TUMS antacid tablet was crushed into a fine powder using the mortar and pestle.
3. The mass of the two antacids were record.
14 titration of h2 o2
1. This experiment involves standardizing a potassium permanganate (KMnO4) solution and then using it to determine the concentration of an unknown hydrogen peroxide (H2O2) solution.
2. To standardize the KMnO4 solution, it is titrated against a precisely weighed amount of oxalic acid. This allows the concentration of the KMnO4 to be calculated using the stoichiometry of the reaction.
3. Then, an unknown H2O2 solution is diluted and titrated with the standardized KMnO4 solution. The concentration of the original H2O2 solution can then be calculated from this titration data and the stoichiometry of the reaction between
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IB Chem HL Internal AssessmentTo what extent does .docx
IB Chem HL Internal AssessmentTo what extent does .docx
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16 buffers sp16
This document provides information about buffers and how to prepare a buffer solution in the laboratory. It defines a buffer as a solution that can maintain a constant pH level when small amounts of acid or base are added. Buffers are composed of an acid and its conjugate base. The key properties that should match the desired pH are the acid's pKa value and that its conjugate base only differs by one hydrogen ion. The document outlines how to calculate the mass of salt needed using the Henderson-Hasselbalch equation and dilute the acid solution, and describes various methods for measuring the pH of buffer solutions. It also defines buffer capacity and how it can be experimentally determined.
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The document provides instructions for students to complete calculations to design a buffer of their assigned pH for a chemistry lab experiment. Students are told to use provided resources to determine the appropriate acid-salt pair to use based on the acid's pKa value relative to the assigned pH. They are then directed to use dilution equations to calculate amounts of acid and the Henderson-Hasselbalch equation to find the conjugate base concentration needed to achieve the target pH with their buffer.
7-EnthalpyOfReaction
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1) Calorimetry involves measuring the temperature change of a reaction to calculate the heat released or absorbed.
2) Reactions can be exothermic (releasing heat) or endothermic (absorbing heat).
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15 buffers
Buffers maintain pH through small additions of acid or base and are composed of an acid and its conjugate base, with the pKa slightly above the desired pH. Dilutions can be calculated using the dilution formula of M1V1 = M2V2. The pH of solutions can be determined through litmus paper, pH paper, indicators, or a pH meter. Calculations must be completed and checked by the TA in advance of the experiment.
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The document discusses acid-base titration, including the analyte, standard, neutralization reaction, equivalence point, and procedure. It explains that an acid-base titration involves titrating an acid with a base until the moles of H+ equal the moles of OH-. It also discusses using a pH sensor and indicator to determine the equivalence point, and using stoichiometry to calculate unknown concentrations from experimental data.
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14 standardization&titration
- 4. Standardization Concentration of unknown acetic acid Concentration of NaOH Accurate mass of KHP