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IB Chemistry HL IA ideas list is available online with expert guidance and examples. The list contains 20 to 50+ IA ideas, including research questions and topic descriptions and IB Chemistry HL Internal assessment examples. Choosing the perfect IB Chemistry IA topic can be made easier by approaching it methodically and evaluating existing research before conducting further research on a topicChemistry HL IA ideas
To determine the amount of vitamin C content in the water after boiling the vegetables, a titration reaction will be performed. The end point of the titration is detected when the color of the solution turns blue black after all the ascorbic acid is used up (the volume of iodine solution used will be recorded)
Cooking time of superfoods, superfoods
Temperature of cooking water, Volume of water boiled, Starch indicator and amount, mass of vegetables, etc.
Volume of iodine solution used
Using the Winkler method to measure the dissolved oxygen concentrations in tap water at varying temperatures of the water samples.
Temperature of the water samples
‘Pressure and salinity of the water, Time each sample is left
DO concentration of the water sample
To determine the concentration of aspirin passed out of the vising tubing, a titration reaction is performed. The endpoint is indicated by a permanent trace of a pink color due to the formation of a basic solution.
Time
Number of aspirin tablets, Volume of water, Amount of indicator
Volume of Sodium Hydroxide
Any friable food is put in the oil and is let to fry for about 25-30 seconds. After each cycle, some of the oil is stored aside to perform the titration. This is repeated until the same oil has undergone the frying process 5 times. The experiment is to see how the peroxide value changes for the oil when it is fried once and five times. To determine the amount of peroxide value, a titration reaction will be performed and the volume of sodium thiosulfate used in titration is recorded. The end point of the titration is detected when the color of the solution turns blue black. Using the volume of solution used in the titration procedure, the peroxide value is calculated.
Type of oil, antioxidant
Temperature of the oil, Mass of antioxidant, oil and the frying food, The concentration of Sodium Thiosulfate
The volume of sodium thiosulfate used in titration, Peroxide value
Samples of powdered vitamin C tablets were exposed to the atmosphere for different periods of time, and then dissolved in distilled water. 1 ml of the solution was then titrated with DCPIP (Di-chlorophenol indophenol) stock solution until the solution retained the dark blue-black color. Using the raw data obtained, the shelf life of the vitamin C tablets and the rate of degradation of Vitamin C were calculated.
The time each group of tablets are exposed to the atmosphere
Brand of the tablets, mass of Vitamin C dissolved in distilled water
Mass of Vitamin C present in the tablets
The temperature of the buffer solution will be changed by 20, 30 up to 60 degrees and the pH of the solution will be measured until the buffer reaches a pH of 12. Then, with that, the buffer capacity is calculated along with the temperature dependance of the buffer solution. Firstly, sodium acetate is prepared. Then, sodium hydroxide solution is made. Then, the acetate buffer is prepared. The burettes are then set up according to the experimental setup. Then the buffer solution is heated. Afterward, the acetate buffer solution is set up below the burette system and titration starts. The same is repeated for different temperatures.
Temperature of the acetate buffer
Initial concentration of acetate buffer and sodium hydroxide, volume of the solutions
pH of the acetate buffer
Set up the appropriate experiment setup. Measure water and put it into the metal can. Pour an alcohol into a spirit burner and then adjust the wick accordingly. Weigh the spirit burner with the cap. Stir the water in the metal can and record the temperature. Remove the cap of the spirit burner and light the wick. Immediately, put it under the metal can of water and continuously stir the water. When there has been a 10 degree rise in the temperature, blow out the flame and replace the cap. Reweigh the spirit burner. Repeat with other alcohols.
Alcohol used
Volume of water used, Distance from can to wick, Temperature rise, etc.
Mass of alcohol lost
To determine the concentration of free chlorine in the water samples, an iodometric redox titration technique is used. Three water samples with different chlorine concentration are obtained. Afterwards, Potassium iodide and starch indicator to determine if they are able to indicate these small concentrations of chlorine in the samples and change the color of the solution. Titration was performed using the water samples and the sodium thiosulfate. The amount of sodium thiosulfate used will determine the amount of free chlorine present.
Concentration of cyanuric acid
pH, temperature, initial chlorine concentration, concentration of urea, etc.
Concentration of free chlorine
The reactants were placed in individual test tubes. The test tubes filled with reactant solution were placed into the test tube rack and the thermometer was put in one of the test tubes. The test tube rack was placed into the Clifton Water Bath. The test tubes were left in the water bath for 10 minutes, and the reactant solutions were made sure to have achieved the desired temperature by using the thermometer. A cross was drawn on the paper using the pen, and then placed on a surface ready for a measuring cylinder to be put above it. Five measuring cylinders were placed next to the water bath. The Iron(IlI) nitrate reactant solution was poured into the measuring cylinder placed above the cross. The sodium thiosulfate reactant solution was soon after poured into the same measuring cylinder, and then the measuring cylinder was immediately afterwards observed from above. The timer started and stopped as soon as the cross was visible to the naked eye from the top of the measuring cylinder and the time was recorded on the data table.
Temperature
Concentration and Volume of Reactant and Catalyst solutions, Reaction vessel, etc
Time taken for the reaction to reach the end point
Utilising chromatography, identify and analyse the various pigments within various shades of lipstick and then heating these samples and measuring the degradation of certain pigments
Lipstick shades
Degradation of certain pigments
Procuring various transition metal catalysts and measuring their effect on the rate of any reaction by measuring the concentration of a substance with accordance to time
Transition metal catalysts
Rate of reaction
In this experiment, we aim to determine the relationship between the concentration of a sucrose solution and its optical rotation. We will measure the optical rotation of sucrose solutions of varying concentrations using a polarimeter. We will prepare solutions of sucrose of concentrations ranging from 1% to 10%. Each solution will be measured in triplicate to ensure precision in the readings. The optical rotation will be recorded as degrees of rotation, and a graph of the optical rotation versus concentration will be plotted.
Concentration of the sucrose solution
The temperature of the solution, the length of the polarimeter tube, and the wavelength of the light used
Optical rotation of the sucrose solution
Enzymes are biological catalysts that speed up chemical reactions. The activity of enzymes is affected by the pH of the solution they are in. In this experiment, you could investigate how the activity of an enzyme (e.g. catalase) changes as you vary the pH of the solution. You could measure the rate of an enzyme-catalyzed reaction (e.g. decomposition of hydrogen peroxide) at different pH values.
pH of the solution
Concentration of the enzyme, Concentration of the substrate, and the temperature
Rate of the reaction (measured as the amount of gas produced over time)
To do this experiment, we will collect several water samples from different sources and measure their dissolved oxygen concentration using both the Winkler method and the dissolved oxygen meter. We will then compare the results and calculate the percentage error for each method. We will also investigate the effect of temperature and pH on the accuracy of the Winkler method by repeating the measurements at different temperature and pH levels.
Water sample source, temperature, and pH
The method of measurement (Winkler method and dissolved oxygen meter)
Dissolved oxygen concentration
To conduct this experiment, we would first prepare a solution of sodium thiosulfate and potassium iodide in a conical flask. We would then add a known amount of iodine solution to the flask and allow the reaction to reach equilibrium. This can be detected by adding starch solution, which forms a blue-black color in the presence of iodine. We would then titrate the remaining iodine with sodium thiosulfate solution to determine the concentration of iodine that was consumed in the reaction. We would then repeat the experiment at different temperatures, using a water bath or a thermostatically controlled heating mantle to maintain the temperature. We would measure the equilibrium constant at each temperature by calculating the concentration of iodine that was consumed in the reaction and using an equation.
Temperature
Initial concentrations of the reactants, the volume of the reaction mixture, and the titration procedure used to determine the concentration of iodine
Equilibrium Constant
The aim of this experiment is to determine how storage temperature affects the sulfite concentration in wine. Different samples of wine will be stored at various temperatures (e.g. 5°C, 15°C, and 25°C) for a set period of time. The sulfite concentration in each sample will then be measured using a spectrophotometer. The results will be analyzed to identify any correlations between storage temperature and sulfite concentration.
Storage temperature (5°C, 15°C, and 25°C)
Type of wine, initial sulfite concentration, duration of storage, volume of wine sampled, method of sulfite measurement
Sulfite concentration in wine
A sample of a ferromagnetic material such as iron or nickel will be subjected to different temperatures ranging from -10°C to 100°C. A magnetometer will be used to measure the strength of the material’s magnetic field. The experiment will be repeated three times for each temperature, and the average magnetic field strength will be calculated.
Temperature
Type of ferromagnetic material, size and shape of the sample, the distance of the magnetometer from the sample, and the strength of the magnetometer
Magnetic field strength
In this experiment, you would determine the concentration of an unknown acid by back titration with a standard solution of a base. You would first react to a known amount of the acid with an excess of a known concentration of a base. The remaining base in the solution would then be titrated with a standard solution of an acid to determine the amount of base that was not consumed in the first reaction. From this, you could calculate the amount of acid that was consumed in the first reaction and therefore the concentration of the unknown acid.
the volume and concentration of the base used in the first reaction.
the volume and concentration of the unknown acid, the volume of the base added, the temperature of the solutions, the accuracy of the burette, and the pH indicator used.
the volume and concentration of the standard acid solution needed to neutralize the excess base.
You could synthesize several metal complexes using a common transition metal (e.g. cobalt) and various organic ligands (e.g. ammonia, ethylenediamine, diethylenetriamine). You could then analyze the complexes using various techniques such as UV-Vis spectroscopy, infrared spectroscopy, and melting point determination to determine their structure and stability. You could also compare the reactivity of the complexes with different ligands by performing a substitution reaction to displace one ligand with another.
the different ligands used to synthesize the metal complexes.
the same transition metal used to synthesize all the complexes, the concentration of the metal ion in the reaction mixture, the solvent used to dissolve the metal ion and ligand, and the temperature at which the reaction is carried out.
the structural and stability differences between the metal complexes synthesized with different ligands
In this experiment, the effect of the concentration of a solute on the rate of crystal formation during crystallization will be investigated. Sodium chloride will be used as the solute, and distilled water will be used as the solvent. The experiment will involve dissolving varying amounts of sodium chloride in the distilled water to create solutions of different concentrations. The solutions will then be placed in a controlled environment to allow for crystallization to occur. The rate of crystal formation will be measured by observing and recording the time taken for crystals to form in each solution.
The concentration of the solute (sodium chloride)
Temperature, volume of solvent, type of solute, method of mixing the solution
The rate of crystal formation
In this experiment, the accuracy and precision of a spectrometer will be investigated with respect to the wavelength of light used. A spectrometer will be set up and calibrated with a known light source, and measurements will be taken at various wavelengths using a series of calibration lamps. The spectrometer readings will be compared to known values to determine accuracy, and multiple measurements will be taken at each wavelength to determine precision.
The wavelength of light used in the experiment
The same spectrometer will be used throughout the experiment, with the same calibration lamps and settings, the temperature and humidity of the room and the same operator to avoid human error
The accuracy and precision of the spectrometer readings
The aim of this experiment is to investigate the effect of temperature on the activation energy of the reaction between hydrochloric acid and sodium thiosulfate. To do this, a series of experiments will be conducted, in which the temperature of the reaction mixture will be varied, and the rate of the reaction will be measured. The reaction will be monitored by measuring the time taken for a cross drawn on a piece of paper to disappear. The temperature of the reaction mixture will be varied by placing the reaction vessel in a water bath set to a specific temperature.
The temperature of the reaction mixture, The concentration of the reactants
The volume of the reaction mixture, and the method of mixing
The rate of the reaction
The experiment aims to investigate the effect of changing the concentration of the electrolyte on the potential difference and current generated in a voltaic cell. The experiment will involve setting up a simple voltaic cell using zinc and copper electrodes and different concentrations of a common electrolyte, such as copper sulfate solution. The potential difference generated across the electrodes will be measured using a voltmeter, and the current flowing through the cell will be measured using an ammeter. The experiment will be repeated at least three times for each concentration of the electrolyte to ensure accuracy and reliability of results.
The concentration of the electrolyte, Temperature of the electrolyte
The type of electrolyte, Surface area of the electrodes, Distance between the electrodes, and type of electrodes used
The potential difference and current
In this experiment, the effect of concentration on the rate of reaction and the mechanism of reaction between sodium thiosulphate and hydrochloric acid will be investigated. The reaction involves the formation of a yellow precipitate of sulfur when the two solutions are mixed. By measuring the time taken for the precipitate to form, the rate of reaction can be calculated. The concentration of sodium thiosulphate and hydrochloric acid will be varied independently to determine the effect of concentration on the rate of reaction. The experiment will be repeated three times for each concentration to ensure accuracy. The temperature of the solutions and the volume of the solutions will be kept constant to ensure that these variables do not affect the rate of reaction.
Concentration and temperature of sodium thiosulphate and hydrochloric acid
The volume of the solutions
The rate of reaction
In this experiment, we will investigate the relationship between entropy and spontaneity by measuring the Gibbs free energy change (ΔG) of a chemical reaction at different temperatures. We will use a coffee cup calorimeter to measure the heat absorbed or released during the reaction and calculate ΔG using the equation ΔG = ΔH – TΔS, where ΔH is the enthalpy change of the reaction, T is the temperature in Kelvin, and ΔS is the change in entropy. We will vary the entropy of the system by adding different amounts of a solid solute to a fixed amount of solvent and measure the temperature at which the reaction becomes spontaneous (ΔG < 0). We will repeat the experiment with different solutes to determine the effect of molecular size and structure on entropy and spontaneity.
Amount and type of solute added to the solvent, temperature of the reaction, the volume and concentration of the solvent.
The mass and purity of the solutes, the pressure and atmospheric conditions in the laboratory, the equipment used to measure temperature and heat.
Change in Gibbs free energy, temperature at which the reaction becomes spontaneous.
This experiment aims to investigate the effect of the concentration of an acid on the pH curve during titration with a strong base. The experiment will involve the titration of different concentrations of hydrochloric acid with sodium hydroxide. A pH meter will be used to measure the pH of the solution at different points during the titration process, and the data will be used to plot the pH curve.
Concentration of hydrochloric acid, temperature of the solution, concentration of the base
Volume of acid and base used.
pH of the solution at different points during the titration process
The experiment aims to investigate the effect of different types of alcohol on the rate of esterification of carboxylic acid and alcohol using sulfuric acid as a catalyst. A series of reactions will be carried out by mixing different types of alcohols such as methanol, ethanol, propanol, and butanol with acetic acid, and then adding sulfuric acid as a catalyst. The reaction mixture will be heated under reflux for a fixed amount of time, and the products will be extracted with a separating funnel and analyzed using gas chromatography. The rate of the reaction will be calculated by measuring the amount of ester formed over time.
The type of alcohol used in the reaction (methanol, ethanol, propanol, butanol), the temperature of the reaction mixture.
The concentration of the reactants, the amount of sulfuric acid used as a catalyst, the duration of the reaction, and the analytical method used for measuring the amount of ester formed.
The rate of esterification, measured by the amount of ester formed over time.
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This list of IB Chemistry SL IA ideas is a helpful resource for students to showcase their understanding of chemistry concepts and theories. The IA is a research project that accounts for a significant portion of the grade, and students can choose from a wide range of topics and IB chemistry internal assessment examples , such as organic chemistry, chemical kinetics, and applications in the real world. Students can also find expert guidance and examples to improve their own work.
To determine the amount of vitamin C content in the water after heating the orange juice (different temperatures), a titration reaction will be performed. The end point of the titration is detected when the color of the solution turns blue black after all the ascorbic acid is used up (the volume of iodine solution used will be recorded).
Temperature of orange juice
Brand of Orange Juice, Volume of orange juice for titration, Amount of Starch indicator solution
Amount of potassium iodate in titration with orange juice (vitamin C)
Measure the initial mass of the rusted nail and put it into a test tube. Following that, pour in the rust removers and let the rusted nail soak in it for 5 days. Once it is done, use steel wool to remove the rust and wipe with a cloth. Measure the mass of the nail now and then compare how the mass differs while using different kinds of rust removers.
Rust remover
Rusted iron nail size and mass, Amount of rust approximately
Mass of iron nail without rust
A set amount of tap water sample is collected in a conical flask and the EBT indicator and the buffer solution is added to it. Complex metric titration is performed by titrating the solutions against EDTA. The volume of EDTA used for the solution to turn blue indicates the end point.
Temperature of tap water
Volume of Water, Concentration of EDTA, Source of tap water, Volume of indicator and buffer
Hardness of tap water
2 methods can be used to determine the iron content. 1st is the redox titration: Potassium permanganate is titrated against the iron solution (iron tablet into deionized water with sulfuric acid added to make it acidic in nature) and the end point is determined when the color changes from colorless to light pink. The 2nd method is the precipitation method: Dissolve iron tables into sulfuric acid and add concentrated nitric acid to it. Add sodium hydroxide solution to neutralize the excess acid and precipitate the iron in the solution. Put a filter paper on top of the vacuum flask and filter the precipitate. Weight the filter paper in intervals until the weight is constant.
Determining and comparing the energy released in the combustion of different alcohols, and concluding with a research on which one of them is more efficient as a fuel substituent to fossil fuels. A copper calorimeter, 3 different kinds of alcohol and a spirit burner is used to conduct the experiment.
Number of carbon atoms in the molecule
Volume of water, initial mass of alcohol
Enthalpy change of combustion of the alcohol
By redox titration, one can determine the amount of sodium thiosulphate required to reduce iodine to Iodide ions. To begin with, a sodium thiosulfate solution is prepared. After, a 0.5% starch indicator solution is also made. Then, distilled water is added to the iodised salt for it to get dissolved. Then, hydrochloric acid and potassium iodide solution is added to the dissolved salt. The solution will turn a yellow/brown color as iodine is produced. The solution is later titrated with the sodium thiosulfate solution until the yellow/brown color of iodine becomes very pale. Titration is repeated until concordant results come.
Iodised salt
Hydrochloric acid, Potassium iodide,
Sodium thiosulfate solution
Providing different concentrations of an electrolyte(copper sulphate) in the electroplating process for an iron sheet and measuring the amount of copper electroplated within a time duration.
Various concentrations of copper sulphate solution
Mass of copper electroplated
Heating different types of milk(such as oat, almond, cow etc.) at different temperatures for a certain duration of time and measuring the calcium concentration of the sample before and after utilising complexometric titration
Varieties of Milk
Calcium concentration
The experiment aims to investigate the clock reaction, which is a reaction that changes color after a certain time interval. The experiment will use the reaction between potassium iodide (KI) and sodium thiosulfate (Na2S2O3) in the presence of starch as an indicator. The experiment will vary the concentration of the reactants to determine how it affects the time it takes for the reaction to occur. By measuring the time it takes for the reaction to occur at different concentrations of reactants, we can determine the rate of reaction and calculate the activation energy.
Concentration of KI and Na2S2O3
Amount of starch used, the temperature of the reaction, and the volume of the reactants
Time it takes to change color (Reaction time)
In this experiment, students will set up galvanic cells using zinc and copper electrodes immersed in various electrolyte solutions of different concentrations. The rate of the galvanic cell reaction will be measured by monitoring the potential difference (voltage) between the electrodes over time. The electrolyte solutions tested will include solutions of different concentrations of copper sulfate, zinc sulfate, and potassium chloride. The aim of the experiment is to determine how the concentration of the electrolyte affects the rate of the galvanic cell reaction, which can be used to predict the feasibility and efficiency of electrochemical processes.
Concentration of electrolyte solution
Type of electrode, surface area of electrode, temperature, and time of reaction.
Rate of galvanic cell reaction (measured as voltage change over time)
In this experiment, the effect of varying the amount of acid catalyst on the yield of the esterification reaction will be investigated. A mixture of carboxylic acid and alcohol will be heated in the presence of sulfuric acid catalyst, and the yield of the ester product will be determined by the amount of soap produced. The experiment will be carried out by preparing several reaction mixtures with different amounts of sulfuric acid catalyst and the same amount of reactants. The reaction progress will be monitored by measuring the pH and the temperature of the reaction mixture. After the reaction is complete, the yield of soap will be determined by titration with a standardized sodium hydroxide solution.
Amount of sulfuric acid catalyst (0.1 M, 0.2 M, 0.3 M, 0.4 M)
Amount of reactants (carboxylic acid and alcohol), reaction time and temperature, concentration and volume of sodium hydroxide solution used for titration.
Yield of soap (measured by titration with sodium hydroxide)
The aim of this experiment is to determine the stoichiometry of a chemical reaction between vinegar and baking soda. This experiment involves measuring the volume of CO2 gas produced during the reaction between vinegar and baking soda. The reaction equation for this experiment is CH3COOH + NaHCO3 → CH3COONa + CO2 + H2O. The experiment will be conducted by mixing different amounts of vinegar and baking soda in a flask and measuring the volume of CO2 gas produced. The volume of CO2 gas produced will be recorded at regular intervals of time using a gas syringe. The stoichiometry of the reaction will be determined by calculating the ratio of the moles of reactants and products involved in the reaction.
The amount of vinegar and baking soda used in the reaction.
The temperature, pressure, and time of the experiment.
The volume of CO2 gas produced during the reaction.
The experiment involves preparing solutions of a fluorescent dye in various solvents, such as water, ethanol, and acetone. The solutions are then exposed to a UV light source, and the intensity of the fluorescence emitted by the dye is measured using a spectrophotometer. The experiment is repeated with different concentrations of the dye in each solvent to investigate the effect of concentration on fluorescence.
The type of solvent used.
The concentration of the dye in each solution, the volume of solvent used, the wavelength of the UV light source, and the distance between the sample and the spectrophotometer.
The intensity of fluorescence emitted by the dye.
In this experiment, the energy content of two different fuels, such as ethanol and gasoline, will be compared. The fuels will be burned in a calorimeter, and the heat released during the combustion reaction will be used to heat a known amount of water. The change in temperature of the water will be used to calculate the energy content of each fuel. The experiment will be repeated three times for each fuel to ensure accuracy and reliability.
The type of fuel being burned (ethanol or gasoline)
The amount of fuel used, the amount of water used, the temperature of the water before the combustion reaction, the mass of the calorimeter, the time over which the reaction occurs, the pressure and volume of the reaction environment.
The energy released during the combustion reaction (measured in joules or calories)
To do this experiment, we could first use a pH meter to measure the initial pH of a simulated stomach acid solution (e.g. 0.1 M HCl), and record this as the dependent variable. Next, we could add a known amount of each tablet to separate portions of the acid solution, and record the time it takes for the pH to reach a neutral value of 7.0. This would be repeated for several different types of tablets and for a control (i.e. a portion of acid without any tablet added). Finally, we could calculate the average time taken to neutralize the acid for each type of tablet, and compare these values to determine which tablet is most effective in terms of speed and efficiency of acid neutralization.
type of indigestion tablet
time taken to neutralize acid solution
starting pH of acid solution, amount of acid solution, amount of tablet added, temperature of solution, stirring rate, etc.
In this experiment, the rate of effervescence in Alka-Seltzer tablets will be measured by observing the time it takes for the tablet to completely dissolve and produce bubbles. To carry out the experiment, each concentration of citric acid solution will be prepared and labeled. Then, an Alka-Seltzer tablet will be added to each solution, and the time it takes for the tablet to completely dissolve and produce bubbles will be recorded. The data collected will be used to create a graph of the time it takes for the tablet to dissolve versus the concentration of citric acid solution. The graph will be used to analyze the relationship between the two variables and draw conclusions about the effect of citric acid concentration on the rate of effervescence in Alka-Seltzer tablets.
Concentration of citric acid solution, Amount of water
The temperature (room temperature), and the brand of Alka-Seltzer tablets used
Time it takes for the tablet to dissolve completely
In this experiment, the enthalpy change of combustion of magnesium will be determined by measuring the heat released from the reaction between magnesium and hydrochloric acid. The heat released will be measured using a simple calorimeter. The experimental value will then be compared to the theoretically calculated value using Hess’s Law, which states that the enthalpy change of a reaction is independent of the pathway taken, provided that the initial and final conditions are the same. The enthalpy change of combustion of magnesium can be calculated by combining the enthalpy changes of the reactions that make up the overall reaction.
The mass of magnesium used in the reaction, the concentration and volume of hydrochloric acid used in the reaction
The mass and type of calorimeter used, the initial and final temperature of the reaction mixture, and the atmospheric conditions during the experiment
The heat released from the reaction
In this experiment, the iodine-clock reaction will be used to investigate the effect of changing the concentration of a reducing agent on the rate of the reaction. The reaction involves the oxidation of iodide ions by hydrogen peroxide, which is catalyzed by iodide ions. The time taken for the blue-black color to appear will be measured using a stopwatch. The reducing agent will be varied in concentration by diluting it with water. A range of concentrations will be used to determine the effect of concentration on the rate of the reaction. The experiment will be conducted at room temperature to control the temperature as a variable.
Concentration of reducing agent (varied by dilution with water), Temperature, volume of reactants
Concentration of iodine, concentration of hydrogen peroxide, use of the same stopwatch for all trials
Time taken for the blue-black color to appear (indicating completion of the reaction)
The experiment involves constructing a simple electrochemical cell using two different metals (e.g., copper and zinc) as electrodes and a salt bridge filled with different concentrations of electrolyte (e.g., NaCl). The voltage output of the cell will be measured using a voltmeter for each concentration of electrolyte. The experiment will be repeated with different concentrations of electrolyte to observe the effect of concentration on the voltage output of the cell.
Concentration of electrolyte
The type of metals used as electrodes, the size of the electrodes, the distance between the electrodes, the temperature, the surface area of the electrodes, the type of electrolyte used, and the concentration of the metals used.
Voltage output of the electrochemical cell
The purpose of this experiment is to investigate how the polarity of different solvents affects the separation of ink components in paper chromatography. The experiment will involve placing a small spot of ink at the bottom of chromatography paper and then dipping the paper in different solvents of varying polarities. As the solvent travels up the paper, it will carry the ink components with it, and the separation of the components will be observed. The distance traveled by each component and the Rf value will be calculated for each solvent.
The polarity of the solvents used (e.g. water, ethanol, acetone, etc.), the size of the ink spot
The type of ink used, the type and size of the chromatography paper used, the temperature and humidity of the experimental environment, the length of time the paper is left in the solvent
The distance traveled by each component of the ink and the Rf value
The aim of this experiment is to compare the energy content of different fuels by determining the enthalpy change of combustion. The fuels used in this experiment will be ethanol, propanol, and butanol. A calorimeter will be used to measure the heat released during the combustion of each fuel. The mass of each fuel burned will be controlled, and the temperature change of water will be recorded before and after each combustion. The enthalpy change of combustion will then be calculated using the formula ΔH = q/m where ΔH is the enthalpy change, q is the heat released, and m is the mass of fuel burned.
The independent variable in this experiment is the type of fuel used (ethanol, propanol, and butanol).
The mass of fuel burned will be controlled, and the same calorimeter will be used for each combustion. The starting temperature of the water will also be controlled, as will the room temperature during the experiment.
The dependent variable is the enthalpy change of combustion, which will be calculated based on the heat released during combustion.
The experiment will involve creating sodium polyacrylate solutions of varying concentrations, and then measuring their ability to absorb water. This will be done by placing a small amount of each solution in a separate container, and then adding a fixed amount of water to each container. The containers will be left undisturbed for a set amount of time to allow the sodium polyacrylate to absorb as much water as possible. After the set time, the remaining water in each container will be measured, and the amount absorbed will be calculated. The results will be analyzed to determine the relationship between the concentration of the sodium polyacrylate solution and its ability to absorb water.
Concentration of sodium polyacrylate solution
Type of sodium polyacrylate used, amount of water added, temperature, and time allowed for absorption
Amount of water absorbed by the sodium polyacrylate
The purpose of this experiment is to determine the solubility of KNO3 in water at different temperatures and compare the results with the literature values. The experiment will involve dissolving a set amount of KNO3 in a fixed amount of water at different temperatures, ranging from 10°C to 70°C. The solutions will then be cooled and allowed to crystallize, and the mass of KNO3 crystals formed will be measured. These measurements will be used to construct a solubility curve for KNO3 at different temperatures. The solubility curve will then be compared to the literature values to assess its accuracy.
Temperature (10°C, 20°C, 30°C, 40°C, 50°C, 60°C, 70°C)
Control Variables: Mass of KNO3, Volume of water, stirring rate, cooling rate, and measurement instruments
The amount of fuel used, the amount of water used, the temperature of the water before the combustion reaction, the mass of the calorimeter, the time over which the reaction occurs, the pressure and volume of the reaction environment.
Solubility of KNO3 in water (grams of KNO3 per 100g of water)
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