C5d Titrations Higher
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This document describes the process and principles of acid-base titration. It discusses: 1. The equipment used including burettes, conical flasks, and indicators. 2. The method of slowly adding an alkali to an acid while swirling and monitoring the indicator until the endpoint is reached. 3. Calculations that can be done such as determining moles, concentration, and mass based on the titration results. 4. How a titration curve shows pH changing as a function of alkali added, with the endpoint at neutralization.
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1) The student conducted a titration experiment to determine the concentration of vinegar by titrating 10 mL of vinegar with a 0.1 M NaOH solution.
2) The student repeated the titration experiment three times and found that on average, it took 49.3 mL of the NaOH solution to titrate the 10 mL vinegar sample.
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1) The student conducted a titration experiment to determine the concentration of vinegar by titrating 10 mL of vinegar with a 0.1 M NaOH solution.
2) The student repeated the titration experiment three times and found that on average, it took 49.3 mL of the NaOH solution to titrate the 10 mL vinegar sample.
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This document discusses the titration of hydrated oxalic acid with a sodium hydroxide solution of unknown concentration. The titration reaction is used to determine the molarity of the sodium hydroxide solution. Phenolphthalein indicator is added, which causes the solution to change from colorless to light pink at the endpoint of the reaction. By performing the titration and calculating the moles of sodium hydroxide reacted, the experimenter determined the molarity of the sodium hydroxide solution to be 0.21M. Issues that affected the precision of the results are also discussed, such as using too much acid volume past the endpoint. Recommendations for improving technique include avoiding bubbles in the
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The document describes an acid-base titration lab experiment where students will:
1) Titrate a measured volume of HCl of unknown concentration with a NaOH solution of known concentration to determine the concentration of HCl.
2) Calculate the number of moles of NaOH used in each trial and determine the concentration of HCl from the reaction.
3) Calculate their percent error compared to the accepted HCl concentration value.
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Titration is a procedure to determine the volume of an acid and base solution needed to exactly neutralize each other. By using a standard solution of known concentration, the concentration of another solution can be determined. There are three types of acid-base titrations: strong acid-strong base, strong acid-weak base, and weak acid-strong base titration. The titration curve shows the pH changes at different volumes of titrant added and the suitable indicators correspond to the end point pH range of each titration type.
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1) The document discusses acid-base titration curves and determining the pH at any point during the titration of a strong acid with a strong base or a weak acid with a strong base.
2) Key aspects include calculating the equivalence point and determining the pH in four regions: before, at, and after the equivalence point as well as in the buffer region between initial addition and the equivalence point.
3) Factors that affect the titration curve include the strength of the acid and its concentration - weaker acids and more dilute solutions result in shallower curves without a clear endpoint.
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This document describes a procedure to determine the concentration of acetic acid in vinegar through acid-base titration. Vinegar samples of known volume will be titrated with a sodium hydroxide solution of known molarity. The collected data on titrant volume will be used to calculate the moles of acetic acid present and from that, the molarity and percentage by mass of acetic acid in the vinegar samples. Students will perform the titration, record observations, calculate results, and report the average molarity and percentage of acetic acid determined.
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This document discusses acid-base titrations and summarizes the key steps in standardizing a sodium hydroxide (NaOH) solution and using it to determine the concentration of acetic acid in vinegar. It explains that NaOH is hygroscopic and absorbs moisture, so it must be standardized against a primary standard, potassium hydrogen phthalate (KHP), through titration. The standardized NaOH solution can then be used to titrate vinegar against it and calculate the moles and molarity of acetic acid present. It also discusses concepts like the pH at the equivalence point of a titration involving a weak acid and strong base.
Khpacidbaseneutralization1slideonechm240xxxxxxxxxxxxxxxxxxdontletgo2 14011010...
This document provides instructions for standardizing a sodium hydroxide solution by titrating it with a primary standard of potassium hydrogen phthalate. It describes cleaning and preparing the buret, titrating the potassium hydrogen phthalate sample, and calculating the molarity of the sodium hydroxide solution based on the titration results. It also discusses using potassium hydrogen phthalate as a primary standard due to its stability and ease of accurate weighing, and explains the titration process and calculating concentration from titration data.
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I hope it might be helpful to you.
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- How satellites orbit Earth due to centripetal force balancing gravitational attraction, with examples of low polar orbits and geostationary orbits.
- How planets orbit the Sun due to centripetal force balancing gravitational attraction.
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Determination of carbonates and bicarbonates in water sample
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Carbonate and bicarbonate ions in the sample can be determined by titrating it with against standard sulphuric acid (H2SO4) using phenolphthalein and methyl orange as indicators. Discussion exp 1
This document discusses the titration of hydrated oxalic acid with a sodium hydroxide solution of unknown concentration. The titration reaction is used to determine the molarity of the sodium hydroxide solution. Phenolphthalein indicator is added, which causes the solution to change from colorless to light pink at the endpoint of the reaction. By performing the titration and calculating the moles of sodium hydroxide reacted, the experimenter determined the molarity of the sodium hydroxide solution to be 0.21M. Issues that affected the precision of the results are also discussed, such as using too much acid volume past the endpoint. Recommendations for improving technique include avoiding bubbles in the
Preparation of sodium phosphate buffers
The document provides instructions for preparing sodium phosphate buffers at different pH levels. It describes adding specific volumes of 1M sodium phosphate stock solutions to water according to a table, adjusting the pH with NaOH or phosphoric acid if needed, and diluting the solution to a final volume of 50mL in a volumetric flask. The buffers are intended to be 0.1M solutions of sodium phosphate at pH levels ranging from 5.8 to 8.0 at 25 degrees Celsius.
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The document outlines how to write a plan and design experiment for testing which color of lime (yellow or green) has a higher level of acidity. It includes sections for the problem statement, hypothesis, aim, apparatus and materials, method, variables, expected results, treatment of results, chemical principles, and sources of errors/assumptions/limitations. The hypothesis is that yellow limes have the highest acidity. The aim is to measure and compare the pH levels of lime juice from each color lime. Yellow lime juice is expected to give a lower pH reading, supporting the hypothesis that it has a higher acidity.
Report 1 prepare and standardize a 0.1 M NaOH solutions
This document describes an experiment to prepare and standardize a 0.1 M sodium hydroxide (NaOH) solution through titration. The student measured and diluted a 3 M NaOH solution to make an approximate 0.1 M NaOH solution. This solution was then standardized through titration against a 0.104 M sulfamic acid standard solution. The student determined the concentration of the NaOH solution to be 0.092 M on average, with a percent error of -9% due to imprecise measurement of the initial 3 M NaOH solution. The student concluded the procedure was successful in standardizing the NaOH solution and learning the titration technique.
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The document discusses volumetric analysis techniques for determining the concentration of acids and bases through titration. It provides examples of calculating molarity from moles and volume. An experiment is described where students determine the concentration of an unknown sodium hydroxide solution by titrating it with hydrochloric acid of a known concentration.
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.
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The document summarizes an experiment titrating 7-Up and Sprite with 1.0 M NaOH to determine the concentration of citric acid in each drink. The average volume of NaOH needed to neutralize the citric acid was 0.4 mL for both drinks, indicating they have the same concentration of 0.04 M citric acid. The error in the experiment was 0.1 mL due to inaccurate measurements and overshooting during titration. More precise equipment and using different acids could improve the experiment.
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This document outlines a procedure to estimate the concentration of potassium permanganate (KMnO4) and copper sulfate (CuSO4) solutions using a colorimeter. Standard solutions of varying concentrations of each compound are prepared. The absorbance of each standard solution is measured using different colorimeter filters to select the filter with the highest absorbance. A calibration curve of absorbance versus concentration is plotted for each compound. The absorbance of unknown solutions is then measured and the concentrations are determined using the calibration curves. The procedure aims to estimate the unknown concentrations of KMnO4 and CuSO4 colorimetrically based on the Beer-Lambert law relationship between absorbance and concentration.
Sample lab
The document describes an acid-base titration lab experiment where students will:
1) Titrate a measured volume of HCl of unknown concentration with a NaOH solution of known concentration to determine the concentration of HCl.
2) Calculate the number of moles of NaOH used in each trial and determine the concentration of HCl from the reaction.
3) Calculate their percent error compared to the accepted HCl concentration value.
Acid base titration
Titration is a procedure to determine the volume of an acid and base solution needed to exactly neutralize each other. By using a standard solution of known concentration, the concentration of another solution can be determined. There are three types of acid-base titrations: strong acid-strong base, strong acid-weak base, and weak acid-strong base titration. The titration curve shows the pH changes at different volumes of titrant added and the suitable indicators correspond to the end point pH range of each titration type.
Acid base titrations
1) The document discusses acid-base titration curves and determining the pH at any point during the titration of a strong acid with a strong base or a weak acid with a strong base.
2) Key aspects include calculating the equivalence point and determining the pH in four regions: before, at, and after the equivalence point as well as in the buffer region between initial addition and the equivalence point.
3) Factors that affect the titration curve include the strength of the acid and its concentration - weaker acids and more dilute solutions result in shallower curves without a clear endpoint.
Estimation of sodium bicarbonate and carbonate in mixture
This document provides instructions for estimating the amounts of sodium carbonate and sodium bicarbonate present in a mixture using acid-base titration with hydrochloric acid and pH indicator dyes. The mixture is titrated with standardized HCl using methyl orange and phenolphthalein indicators to differentiate between the neutralization of carbonate and bicarbonate ions. Methyl orange is used to fully neutralize both species while phenolphthalein only indicates the neutralization of carbonate. The procedure involves standardizing HCl and then titrating aliquots of the mixture with HCl using the two indicators to determine the amounts of each species present.
Preparation of p h buffer solutions
The document provides instructions for preparing pH buffer solutions using various salts including phosphates, acetates, and borates. It lists the different names that phosphate salts can be referred to and provides recipes for making standard pH 4 and pH 7 buffer solutions using potassium dihydrogen phosphate and disodium hydrogen phosphate. Tables are included showing the volumes of acid or base needed to be added to primary salt solutions to achieve buffer solutions in different pH ranges from 1 to 13.
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This document describes creating a calibration curve by making dilutions of a potassium permanganate solution and measuring their absorbance. A primary solution of 2mL KMnO4 in 100mL H2O was made. Dilutions of this were created and their absorbance measured with a spectrophotometer. The resulting calibration curve showed that as the concentration of the dilutions increased, so did their absorbance.
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This document describes a procedure to determine the concentration of acetic acid in vinegar through acid-base titration. Vinegar samples of known volume will be titrated with a sodium hydroxide solution of known molarity. The collected data on titrant volume will be used to calculate the moles of acetic acid present and from that, the molarity and percentage by mass of acetic acid in the vinegar samples. Students will perform the titration, record observations, calculate results, and report the average molarity and percentage of acetic acid determined.
Acidbasetitr
This document discusses acid-base titrations and summarizes the key steps in standardizing a sodium hydroxide (NaOH) solution and using it to determine the concentration of acetic acid in vinegar. It explains that NaOH is hygroscopic and absorbs moisture, so it must be standardized against a primary standard, potassium hydrogen phthalate (KHP), through titration. The standardized NaOH solution can then be used to titrate vinegar against it and calculate the moles and molarity of acetic acid present. It also discusses concepts like the pH at the equivalence point of a titration involving a weak acid and strong base.
Khpacidbaseneutralization1slideonechm240xxxxxxxxxxxxxxxxxxdontletgo2 14011010...
This document provides instructions for standardizing a sodium hydroxide solution by titrating it with a primary standard of potassium hydrogen phthalate. It describes cleaning and preparing the buret, titrating the potassium hydrogen phthalate sample, and calculating the molarity of the sodium hydroxide solution based on the titration results. It also discusses using potassium hydrogen phthalate as a primary standard due to its stability and ease of accurate weighing, and explains the titration process and calculating concentration from titration data.
Lab Report on copper cycle
I hope it might be helpful to you.
Email me on sidhu.s.karanvir@gmail.com to see more work.
Follow me at Linkedln
https://www.linkedin.com/in/karanvir-sidhu-b6995864/
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Report 1 prepare and standardize a 0.1 M NaOH solutions
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To estimate the concentration of KMnO4 and CuSO4 solutions, colorimetrically
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Precipitation reactions involve mixing two aqueous solutions together which results in the formation of an insoluble solid product; the ions from each solution interact and if they form an insoluble compound it will appear cloudy in the solution. Most precipitation reactions are extremely exothermic as they involve the formation of ionic bonds between oppositely charged ions. Tests can be done using silver nitrate or barium nitrate solutions to detect the presence of chloride, bromide, iodide or sulfate ions based on the color of precipitate formed.
As Chemistry Prep 2.2 Intermediate Bonding And Polarity
This document provides exercises for students to complete to help them understand the chemistry topic of intermediate bonding and bond polarity. It includes exercises to define key terms, find electronegativity values of elements, determine percentages of ionic and covalent character in bonds, draw molecules indicating partial charges, and describe an experiment to test if a compound is polar. Students are instructed to attempt the problems after the topic is covered in class and to submit completed answers at the start of the next lesson.
C6g Natural Fats And Oils
Natural fats and oils can be either solid or liquid depending on their saturation. They are esters made from glycerol reacting with fatty acids. Saturated fats have only single carbon-carbon bonds while unsaturated fats contain at least one double carbon-carbon bond. More unsaturated a fat is, the more bromine water it can decolorize. Vegetable oils are often hydrogenated to make them less runny for products like margarine, but this increases their saturated fat content which is less healthy. Vegetable oils can also be used to make biodiesel fuel.
C5f Equilibria
1) Reactions can reach equilibrium when the forward and reverse reactions occur at the same rate, resulting in no change in concentration of reactants and products over time.
2) To increase the yield of products in a reaction at equilibrium, conditions must be changed to shift the equilibrium towards the product side, such as increasing temperature, pressure, or reactant concentration.
3) The Haber process produces ammonia from nitrogen and hydrogen gases at high pressure and temperature in order to shift the reversible reaction towards more ammonia products. Removing ammonia also drives the reaction forward.
Energy
Heat is transferred through particles vibrating (conduction), air rising when hot (convection), and radiation being absorbed and reflected. Insulation in walls traps air which is an insulator, while different methods like passive solar heating and fossil fuels generate heat energy through various processes. When a solid melts it changes state at a constant temperature.
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As Chemistry Prep 2.2 Intermediate Bonding And Polarity
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This document discusses antacids and acid-base chemistry. It defines acids and bases using Arrhenius, Bronsted-Lowry, and Lewis theories. It explains how water dissociates to form hydronium and hydroxide ions. Antacids work by neutralizing excess stomach acid through acid-base reactions. Common antacids use calcium carbonate, magnesium hydroxide, aluminum hydroxide, and sodium bicarbonate. Titration can be used to determine the concentration of an unknown acid or base solution and the effectiveness of antacids is quantified through titration experiments.
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Acid-base titration is a technique used to determine the concentration of an acid or base by neutralizing a solution of unknown concentration with a solution of known concentration. The reaction is monitored using an indicator that changes color at the endpoint of the titration. The document outlines the basic procedure which involves transferring a sample of the solution of unknown concentration into a flask, adding an indicator, and then titrating with the solution of known concentration until the endpoint is reached as indicated by the color change of the indicator. The volume added is used to calculate the concentration of the original unknown solution.
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Scanned with CamScanner1 STANDARIZATION OF A B.docx
This document provides instructions for a two-part experiment involving titration. In part A, students will standardize a NaOH solution by titrating it against a primary standard of KHP. In part B, students will use their standardized NaOH solution to determine the concentration of acetic acid in a vinegar sample through titration. Key steps and concepts discussed include buret usage, endpoint determination, stoichiometric calculations to determine concentration from titration data, and the purpose and characteristics of primary standards.
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Vini Shukla completed a chemistry project to determine the amount of acetic acid in different types of vinegar using titration. The student titrated samples of household vinegar, wine vinegar, and fruit vinegar with a sodium hydroxide solution. By calculating the volume of sodium hydroxide needed to reach the endpoint with the indicator phenolphthalein, the student was able to determine the concentration of acetic acid in each vinegar. The results found wine vinegar had the highest concentration at 72 g/L, followed by fruit vinegar at 48 g/L, and household vinegar had the lowest at 40.5 g/L. The student expressed gratitude to the chemistry teacher for guidance on the project.
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.
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This document describes an experiment to determine the amount of acetic acid in different types of vinegar using titration. The student, G. Priyadharsan, under the guidance of Mrs. P. Muthuchelvi, titrated samples of laboratory vinegar, household vinegar, and wine vinegar with a sodium hydroxide solution of known concentration. By calculating the volume of sodium hydroxide needed to reach the endpoint with the indicator phenolphthalein, the concentration of acetic acid in each vinegar was determined. The results found the acetic acid content to be 22.8 g/L for laboratory vinegar, 40.5 g/L for household vinegar, and 72 g/L for wine vinegar.
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This document outlines an experiment to measure the amount of acetic acid in different types of vinegar using titration. Vinegar contains acetic acid, which can be titrated with a sodium hydroxide solution of known concentration. Phenolphthalein indicator is used to detect the endpoint when the solution turns pink. Three experiments are performed to titrate samples of household vinegar, wine vinegar, and fruit vinegar. The amount of sodium hydroxide used indicates the acetic acid content. Precautions are noted such as carefully transferring and measuring solutions to obtain accurate results.
Chapter 7 acid base
This document contains information about strong and weak acids, and procedures for acid-base titration experiments and standard solution preparation:
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2) An experiment is described to determine the endpoint of a titration between potassium hydroxide and hydrochloric acid solutions.
3) Instructions are provided for preparing a 0.1 M sodium hydroxide standard solution and calculating concentrations using molarity and dilution equations.
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This document describes an experiment to determine the amount of acetic acid in different types of vinegar using titration. The student titrated samples of household vinegar, wine vinegar, and fruit vinegar with a sodium hydroxide solution of known concentration. They found that wine vinegar had the highest concentration of acetic acid at 72 g/L, followed by fruit vinegar at 48 g/L, and then household vinegar at 40.5 g/L. The document provides the aim, introduction, materials, procedure, observations, calculations, results, and precautions for the experiment.
Chitranjan namdeo
This document describes an experiment to determine the amount of acetic acid in different types of vinegar using titration. The student titrated samples of household vinegar, wine vinegar, and fruit vinegar with a sodium hydroxide solution of known concentration. They found that wine vinegar had the highest concentration of acetic acid at 72 g/L, followed by fruit vinegar at 48 g/L, and then household vinegar at 40.5 g/L. The document provides the aim, introduction, materials, procedure, observations, calculations, results, and precautions for the experiment.
Preparing, Diluting of solutions of different Strengths & safety measures whi...
This document provides guidance on weighing and preparing solutions of different concentrations and their dilution, as well as handling techniques for solutions. It discusses solutions, measuring chemicals, different chemical concentrations, dilution of stock solutions, labeling, safety, and conclusions. Specifically, it defines types of solutions, provides procedures for preparing solutions by weighing solids or liquids and dilution, discusses units for reporting concentration like molarity and normality, and guidelines for proper labeling, storage, safety practices, and documentation when working with chemical solutions in the lab.
E q u i l i b r i u m D e t e r m i n a t i o n o f a n E
E q u i l i b r i u m :
D e t e r m i n a t i o n o f a n E q u i l i b r i u m C o n s t a n t
P u r p o s e
To determine the equilibrium constant of a reaction.
L e a r n i n g O b j e c t i v e s
Take a reaction to equilibrium by setting up and monitoring a reaction in a reflux apparatus.
Measure the amount of acid at equilibrium by carrying out an acid-base titration.
Apply the information from a balanced chemical equation and data obtained in the laboratory to de-
termine the concentrations of reactants and products at equilibrium.
Calculate the value of the equilibrium constant using data obtained in the laboratory.
L a b o r a t o r y S k i l l s
To set up and monitor a reflux apparatus.
To carry out an acid-base titration.
E q u i p m e n t
Two 50-mL
graduated cylinders
Two 125-mL
Erlenmeyer flasks
1-mL pipet
25-mL buret
Equipment necessary
to assemble the
reflux apparatus
shown in Figure 1.
C h e m i c a l s
Anhydrous ethanol
(ethyl alcohol)
Anhydrous acetic
acid
Concentrated sulfuric
acid
I n t r o d u c t i o n
From the beginning of this course, we have generally assumed that chemical reactions go to completion, that is,
the reaction proceeds in the forward direction until one of the reactants is completely used up. However, many
reactions do not go to completion and are able to move both in the forward and reverse directions simultaneously.
Such a reaction is called a reversible reaction. A double arrow in the chemical equation designates a reversible
reaction, as shown in Reaction 1:
aA + bB −−−⇀↽−−− cC + dD (Reaction 1)
1
D e t e r m i n a t i o n o f a n E q u i l i b r i u m C o n s t a n t
A reversible reaction has two reaction rates: a forward reaction rate, where the reactants A and B are consumed
andtheproductsCandDareproduced,andareversereactionrate,wheretheproductsCandDareconsumedand
thereactantsAandBareproduced. Allreversiblereactionseventuallyreachapointatwhichtheforwardreaction
rate equals the reverse reaction rate. This point is called equilibrium. At equilibrium, the concentration of
reactants and products do not change with time. It is important to remember that even though the concentration
of reactants and products do not change with time, the reaction has not stopped. Equilibrium is a dynamic state.
The state will persist as long as the reaction conditions remain constant.
A reaction at equilibrium follows the law of mass action which gives the relationship between concentrations
of the reactants and products at equilibrium. According to the law of mass action, the relationship between
concentrations of reactants and products at equilibrium for the above reaction is given in Equation 1:
𝐾eq =
[C]𝑐[D]𝑑
[A]𝑎[B]𝑏
(Equation 1)
Thisrelationshipiscalledtheequilibrium-constantexpression. Theconstant, 𝐾eq, isapositivenumberwhose
value depends on the reaction and temperature.
In today’s experiment, students will be determining the equilibrium constant for the reac
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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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This document summarizes a student's chemistry project on determining the acidity of different types of vinegar using titration. The student tested laboratory vinegar, household vinegar, and wine vinegar. Through the titration experiments, the student found that wine vinegar had the highest concentration of acetic acid at 72 g/L, followed by household vinegar at 40.5 g/L, and laboratory vinegar at 22.8 g/L. The student provided details on the titration procedure and observations, and concluded with advantages and disadvantages of using vinegar. Precautions for laboratory work were also outlined.
Ch 21sec1
This document discusses neutralization reactions, titrations, and related concepts:
- Neutralization reactions involve an acid and base reacting to form a salt and water. Titrations use a known concentration of acid or base to determine an unknown concentration by measuring the volume needed to reach the endpoint.
- Key terms discussed include equivalents, which represent the amount of acid or base that reacts with 1 mole of H+ or OH- ions, and normality, which relates equivalents to concentration in units of equivalents per liter.
- Sample problems demonstrate using the reaction stoichiometry relationship between normality, volume, and equivalents to calculate unknown values in neutralization reactions and titrations
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Food chains
A food chain shows how each living thing gets its food, with arrows indicating what eats what. Carnivores are meat-eating animals like cats, lions, and snakes. Producers like plants make their own food through photosynthesis. Consumers eat other organisms, and can be herbivores that eat plants or predators that hunt other animals. Prey are the animals or plants that are hunted by predators.
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C5d Titrations Higher
- 1. C5d Titrations (Foundation + Higher) This type of reaction is called a “___________________ reaction”. acid + alkali salt + water Diagram Equipment burette conical flask pipette pipette filler indicator Method 1. Carefully fill the burette with alkali and make a note of the starting volume (read from the bottom of the meniscus) 2. Using a pipette filler, fill a pipette up to the line with acid (the bottom of the meniscus should “sit” on the line) the pipette into the conical flask. 3. Slowly add the alkali to the acid swirling the conical flask all the time. Do this until the indicator suddenly changes colour (end point)
- 2. Results Titration volume before volume after titre (volume of alkali added) Average Titre cm3 cm3 cm3 cm3 1 0.0 24.9 2 24.9 49.7 3 0.2 25.1 1. Work out the titres (volume of alkali used to neutralise the acid each time). 2. Work out the average titre used and explain why we use an average 3. Why do we need three titre readings that are within ± 0.02cm3? HIGHER LEVEL 4. Using the average titre, calculate how many moles of alkali were added to the acid. Concentration of the alkali is 1.0 mol/dm3. 5. One mole of acid reacts with one mole of alkali so how many moles of acid must have been in the conical flask. 6. Now calculate the concentration of the original 25cm3 of acid 7. What mass of sodium hydroxide (NaOH) was dissolved in your average titre moles = concentration × volume in dm3 concentration = moles ÷ volume in dm3 volume in dm3 = moles ÷ concentration moles = mass ÷ molecular mass
- 3. Titration curves - if you measure the pH continually as you titrate you get a curve: HIGHER - You must be able to sketch a pH titration curve for the titration of an acid or an alkali 1. On your graph label the end-point of the reaction i.e when the solution neutralises. 2. Describe the shape of your graph in terms of the volume of the alkali added and the pH 3. As more alkali is added the pH of the solution____________________ 4. From your graph, what is the pH at: a) 10cm3 acid added b) 20cm3 acid added c) 40cm3 acid added
- 4. 5. What volume of alkali was added to make the solution neutral? Indicators Mixed Indicators e.g. universal indicator We use Universal indicator to estimate the pH of a solution. It is made from a mixture of different indicators so it produces a continuous colour change as the pH changes. 1. If we had used universal indicator, what colour would it turn for: a) pH 1 b) pH 5 c) pH 7 d) pH 9 e) pH 14 Single Indicators (used in titrations) In an acid-base titration you need a sudden colour change at the end-point i.e. when the solution neutralises. Indicator Colour in Acid Colour in Alkali Litmus Methyl Orange Phenolphthalein You need to learn these colours for the higher tier
- 5. 2. Explain why we need to use single indicators in titrations and not a mixed indicator like universal indicator.