(DOC) Title Of Experiment: Determination Of Acid Content In Vinegar ...

Academia.edu no longer supports Internet Explorer.

To browse Academia.edu and the wider internet faster and more securely, please take a few seconds to upgrade your browser.

×Close

Log In

Log in with FacebookLog in with GoogleorEmailPasswordRemember me on this computeror reset password

Enter the email address you signed up with and we'll email you a reset link.

Need an account? Click here to sign up Log InSign Up

• Log In
• Sign Up
• more
• • About
  • Press
  • Papers
  • Terms
  • Privacy
  • Copyright
  • We're Hiring!
  • Help Center
  • less

download

Download Free PDF

Download Free DOCXTitle of Experiment: Determination of Acid Content in Vinegar -VolumetricANAS HAFIZvisibility

…

description

20 pages

link

1 file

See full PDFdownloadDownload PDF

Related papers

determination of acetic acid in vinegar.docxNovem Ylayron

The experiment was conducted to determine the total acid concentration of a certain brand of vinegar and to determine if that certain brand of vinegar meets the certain amount of acetic acid required and specifies by the commercial law. Acid-base titration was used to determine the acetic acid content.

downloadDownload free PDFView PDFchevron_rightInvestigating the pH Range of IndicatorsMert Inan

Aim: This experiment is intended to experiment on and investigate the transition pH reactivity of acid-base indicators. Because an indicator is also a weak acid or a weak base it has acidic properties and tends to change its colour when the acidity of environment changes. As a result, generally all of the indicators have specific pH levels to provoke the colour change. So, in this experiment, it has been tried to observe the specific pH range of Methyl Orange, Alizarine Yellow, Phenolphtalein, Bromocresol Green and Bromothymol Blue indicators. Research Question: How does the effects of different indicators; Methyl Orange, Alizarine Yellow, Phenolphtalein, Bromocresol Green, Bromothymol Blue with different pH range on the neutralization titration of NH 3 in Burette and HCl in Erlenmeyer Flask occurs under constant pressure and in constant temperature? Hypothesis: As the indicators change, while the titration occurs, the colour of the indicator changes according to the pH level of the solution in the Erlenmeyer flask, thus showing different pH activity. Null Hypothesis: As the indicators change, there will be no colour change interval for different indicators, so all of them will change their colour in the same pH level. Independent Variable: Type of indicator (Methyl Orange, Alizarine Yellow, Phenolphtalein, Bromocresol Green, Bromothymol Blue) Dependent Variable: pH of the colour change interval of the indicator Constant Variables:

downloadDownload free PDFView PDFchevron_rightAcids, Bases and IndicatorsAnthony stamdownloadDownload free PDFView PDFchevron_rightAcid – Base Titration – The Preparation and Standardization Of Sodium Hydroxide Solution Using A Primary Standard and the Determination Of the Total Acidity Of VinegarXiomara Griffith

This lab utilizes the principles to Acid-Base Titration in order to standardize a solution of sodium hydroxide and then use this newly standardized solution to determine the total acidity of acetic acid in vinegar sample and then compare it to the commercial value. The two brands vinegar used in the lab were EHP and Umani.

downloadDownload free PDFView PDFchevron_rightDetermination Of The Concentration Of Acetic Acid In VinegarMuhammad Faris

In this experiment, sodium hydroxide solution is used in order to determine the morality of solution and percent by mass of acetic acid in the vinegar. The method that is used in this experiment is titration. There are 2 parts of the experiment. For the first one is standardization of sodium hydroxide solution. Potassium hydrogen phthalate (KHP) is weighed and stirred until it is completely dissolved then it will be titrated with 250mL of 0.6 sodium hydroxide solution. The neutralization of KHP is repeated thrice. The graph of pH versus NaOH addded is plotted to determine the volume of NaOH required to neutralize the KHP solution in each titration and the morality of the NaOH. The known volume and morality of NaOH is used for the second part of the experiment which is to determine the morality of acetic acid and percent of vinegar. Standardized NaOH solution is titrated the with 10 mL vinegar that has been diluted with 100 mL of distilled water. Both titration for part 1 and 2 are repeated thrice to get more accurate results. The graph of pH vs volume of NaOH added is plotted to determine the volume of NaOH to neutralized vinegar in each titration. Based on results, it can be concluded that the greater the mass of solute in the acid solution, the more concentrated the solution becomes thus, the higher the molarity and more volume of NaOH needed to neutralize the acid. The experiment is completed and successfully conducted.

downloadDownload free PDFView PDFchevron_rightPlant Extract As Acid Base Indicator: An OverviewAjay K ShukladownloadDownload free PDFView PDFchevron_right20. Thin-layer chromatography of acid-base indicatorsASO LE

Acid-base indicators. Acid-base indicators dyes or pH indicators dyes are substances, which are used in chemistry laboratories to visualize end-points of a acid-base titration experiment through color change(s) in different pH environments [ 1 , 2 ]. They constitute a group of organic compounds, like weak acids or weak bases, which react with water and create acid-base conjugate pairs, where both forms are differently colored. In acidic solution protonated structural forms of the dyes exist, whereas in basic solutions deprotonated forms exist. The key structural feature that varies between the acidic and basic forms for acid-base indicator dyes is change in the electronic conjugation (i.e. alternative resonance structures) throughout these molecules. The change in electronic conjugation in various pH environments provide the color changes to 'indicate' a titration end-point. Highly conjugated systems generally absorb and reflect specific wavelengths of light in visible region of the electromagnetic spectrum. pH indicator dyes can be one-colored (e.g. phenolphthalein), when only one form is colored, second or other forms are colorless, two-colored (e.g. methyl orange) or multicolored (e.g. alizarin red S), when each form of the indicator dye is differently colored. Sometimes mixtures of indicator dyes are used, which gradually change the colors in the broad range of pH -these kinds of indicators are known as universal indicators. Fluorescent indicators also exist, which change the color of fluorescence or start to fluoresce at specific pH of solution.

downloadDownload free PDFView PDFchevron_rightACID-BASE INDICATORSAso Gafury

The first part of this table lists some common acid-base indicators in alphabetical order along with the approximate pH range(s) at which a color change occurs. Following this is a table of the same indicators ordered by pH range, which includes the nature of the color change, instructions on preparation of the indicator solution, and the acid dissociation constant pK, when available.

downloadDownload free PDFView PDFchevron_rightTITRATION OF ACID AND BASES LAB REPORT_CHE142Luqman Nasution

2022

This experiment relies on the titration technique to determine the unknown concentration of monoprotic acid in the solution. There are two types of acids that are used in this experiment which is (1) Potassium Hydrogen Phthalate (KHP) and (2) Unknown Acid. The base that was used in this experiment is Sodium Hydroxide (NaOH) solution. This experiment involves two sections or parts: (i) Standardization of Sodium Hydroxide (NaOH) solution using Potassium Hydrogen Phthalate (KHP) solution, and (ii) Analysis of Unknown acidic solution using standardize NaOH solution.

downloadDownload free PDFView PDFchevron_rightThe Analysis of VinegarUsman AdamdownloadDownload free PDFView PDFchevron_rightSee full PDFdownloadDownload PDF

Loading Preview

Sorry, preview is currently unavailable. You can download the paper by clicking the button above.

Related papers

A Guide to pH Measurement Theory & Practice of Laboratory pH Applications Laboratory environment Practical description of how to measure pHThế Trần MinhdownloadDownload free PDFView PDFchevron_rightLAB REPORT 3 KOTnik muhammad izzatdownloadDownload free PDFView PDFchevron_rightDetemination of Percent of Acetic Acid in VinegarMuhammad Uthman AriffindownloadDownload free PDFView PDFchevron_rightFACULTY OF RESOURCE SCIENCE AND TECHNOLOGY DEPARTMENT OF CHEMISTRY STK1211-Practical Analytical ChemistryNurul SyafiqahdownloadDownload free PDFView PDFchevron_rightThe behaviour and properties of some acid-base indicators: a reviewSOKAINA S A A D HEMDAN

Journal of Science and Humanities Studies , 2020

downloadDownload free PDFView PDFchevron_rightInvestigation of a Simple and Cheap Source of a Natural Indicator for Acid-Base Titration: Effects of System Conditions on Natural IndicatorsDaniel Abugri

Green and Sustainable Chemistry, 2012

downloadDownload free PDFView PDFchevron_rightInvestigation of a simple and cheap source of a natural indicator for acid-base titration: effects of system conditionsDaniel Abugri

2012

downloadDownload free PDFView PDFchevron_rightIdentification of Alkalimetric Levels Using Acid-Base Reaction PrinciplesGayatri Soga

Journal of Health, Technology and Science, 2022

downloadDownload free PDFView PDFchevron_rightExperiment 3 DETERMINATION OF ACETIC ACID CONTENT IN VINEGARFrenche HechanovadownloadDownload free PDFView PDFchevron_rightAcidimetry and AlkalimetryTheresia SembiringdownloadDownload free PDFView PDFchevron_rightLab Report 2Tineka JohnsondownloadDownload free PDFView PDFchevron_rightLab 5: pH TitrationKirsten TurnerdownloadDownload free PDFView PDFchevron_rightNotes & Tips Quantitative pH assessment of small-volume samples using a universal pH indicatorgowdham sdownloadDownload free PDFView PDFchevron_rightIndicator in Acid-Base Titrations Indicator in Acid-Base Titrations Indicator in Acid-Base Titrations Indicator in Acid-Base Titrations Indicator in Acid-Base TitrationsManish Kondawar

2006

downloadDownload free PDFView PDFchevron_rightNATURAL INDICATORS AS ALTERNATIVE TO SYNTHETIC ACID BASE INDICATORSEditor iajpsdownloadDownload free PDFView PDFchevron_rightStandardization of Acid and Base solutionsDARREN WONG ZHENG HAO

2018

downloadDownload free PDFView PDFchevron_rightDetermination of Acetic acid content in VinegarCzaika Kate Irica CervantesdownloadDownload free PDFView PDFchevron_rightChemistry Lab_CHM 116_Sec_C_Spring_2015Dr Mohammad Harun-Ur- RashiddownloadDownload free PDFView PDFchevron_rightLab Report 1 Chemistry 1bekk bekdownloadDownload free PDFView PDFchevron_rightTitaration of Vinegar with NaOHNur Shahida Abu HanifahdownloadDownload free PDFView PDFchevron_rightPhosphoric acidNIK CLAROdownloadDownload free PDFView PDFchevron_rightFIGURE 1. Acids and Bases FIGURE 2. pH Values of Acids and Bases The Theory of pH Measurement Theory Application Data SheetSharef YusufdownloadDownload free PDFView PDFchevron_rightDcapodaca-CHM112L Determination of the Components of a Base Mixture by the Double Indicator MethodMa. Juryst Chelsea ArmasdownloadDownload free PDFView PDFchevron_rightBEHAVIOURE STUDY OF THE ASSOCIATION BETWEEN ACID-BASE INDICATORS IN ACIDIC MEDIUM BY USING SPECTROSCOPY TECHNIQUESOKAINA S A A D HEMDAN

Journal of Natural Sciences, Life and Applied Sciences, 2018

downloadDownload free PDFView PDFchevron_rightPh theory guide ENQingyi WangdownloadDownload free PDFView PDFchevron_right

• About
• Press
• Papers
• Topics
• We're Hiring!
• Help Center

• Find new research papers in:
• Physics
• Chemistry
• Biology
• Health Sciences
• Ecology
• Earth Sciences
• Cognitive Science
• Mathematics
• Computer Science

• Terms
• Privacy
• Copyright
• Academia ©2024