A titration method is conducted by the addition of a standard solution from a burette until reaction is completed. The volume of reagent needed for the completion of titration can be determine from the difference between the initial and final volume readings. When an analyte reacts with a reagent of known concentration, it is called as titration. Analyte is a chemical substance that is a chemical analysis subject 1. Titrant is the standard solution added from the burette.
g) I will then repeat the experiment, but using different concentrations of Sodium and water in the solution to see how the reaction rate changes. Apparatus ========= I will be using: 1 large beaker 1 small beaker (for Sodium Thiosulphate) 1 small beaker (for Hydrochloric Acid) 2 small measuring cylinders 1 stop clock Prediction ========== · I predict that the higher the concentration of Sodium Thiosulphate
It resembles sodium thiosulphate, Na2SO4, with one less oxygen atom and one more sulphur atom. The additional sulphur atoms can be driven out by an acid. Equation [IMAGE]Na2S2O3 + 2HCl S + 2NaCl + SO2 Sodium [IMAGE]Thiosulphate + Hydrochloric acid Sulphur + sodium chloride + sulphur dioxide Variables Independent Variable - factors to be changed: The concentration of sodium thiosulphate solution will be adjusted to be tested at different molars. This is changing the ratio of sodium thiosulphate to water. Dependant variable - factor to be measured: The time it takes for the cross to be fully out of vision will be measured to test the rate in which acid reacts with thiosulphate.
Rate of Reaction Between Thiosulphate and Various Concentrations of Hydrochloric Acid Aim: The aim of this experiment is to determine the rate of reaction between thiosulphate(Na2S2O3) and various concentrations of hydrochloric acid (HCl). The rate of reaction will be measured rather crudely by seeing how long it takes for the mixture of water and hydrochloric acid to cloud up the beaker and make a large 'X' under the beaker in which the solution will be placed unvisable. Method: In my experiment, I will be using the following apparatus: o 2 measuring cylinders o Water o Beaker o Hydrochloric acid o Thiosulphate solution o Laminated card with a oversized 'X' on it Diagram: [IMAGE] [IMAGE][IMAGE] [IMAGE] Firstly, I will fill the beaker with 50ml of water from the laboratory taps. The beaker will then placed on the marked paper. Next, the hydrochloric acid will be added to the Na2SO3 (thiosulphate).
Investigating the rate of reaction between sodium thiosulphate and hydrochloric acid I am going to measure the rate of the reaction when hydrochloric acid is added to sodium thiosulphate. I am going to investigate what effect the concentration of the sodium thiosulphate has on the reaction rate. When sodium thiosulphate and hydrochloric acid are mixed, a yellow precipitate of sulphur is produced. The solution becomes increasingly difficult to see through as more and more sulphur is formed. This is how I plan to measure the rate of the reaction.
The solubility product constant, Ksp is given in the following example: Ksp for AgCl is Ksp = [Ag][Cl] Ksp for PbI2 is Ksp = [Pb][I]2 This gives the relationship between the ions in the saturated solution and is the maximum concentration possible without creating precipitation. In this lab, solutions of lead nitrate and potassium iodide will be mixed at a number of dilutions. The reactions will then be observed to see at which point a precipitate no longer occurs. Ksp will then be stated as a range of values at room temperature, and the precipitate test tubes will be heated until the precipitate is dissolved so that Ksp may be observed and determined at different levels. In this experiment various solutions of lead nitrate and potassium iodide were mixed at a number of different dilutions.
How Concentration affects the rate of reaction I am investigating the rates of reaction and how the different variables can affect it. I know that the temperature, a catalyst, concentration, the surface area, light and pressure of a gas can affect the rate of reaction. In this particular experiment I am going to investigate on how the concentration of one of the reactants affects the rate of reaction. To show that the concentration does affect the rate of reaction I am going to carry out the reaction of sodium thiosulphate and hydrochloric acid. The reactant I am going to change in concentration for each experiment/reading is sodium thiosulphate.
Science lab report Aim: To find out the effect of concentration on rates of reaction using Sodium Thiosulphate. and Hydrochloric Acid. The purpose of the experiment is to see how different volumes of Hydrochloric Acid affect the rate of reaction. The reaction, which produces solid Sulfur, it will then be followed by measuring the time needed for the reaction to become opaque/cloudy. Hypothesis: I predict that the higher the volume of concentrated Hydrochloric Acid the less time it will take for the cross to disappear.
The rate of reaction is a measure of the change, which happens during a reaction in a single unit of time. The things that affect the rate of reaction are as follows: · Surface area of the reactants · Concentration of the reactants · The temperature at which the reaction is carried out · Use of a catalyst Reaction equation is mentioned above but rate equation could only be decided by doing experiments. So the following procedure can be used to carry out the experiment. Plan Equipment · 2 Measuring cylinders · Beaker · Stopwatch · Paper with black cross on it · Sodium Thiosulphate (different concentrations) · Hydrochloric acid (same concentration each time) · Water (different concentrations) · Pipette Prediction I predict that the greater the concentration of Sodium Thiosulphate
The Factors Controlling the Rate of the Sodium Thiosulphate and Acid Reaction Planning I am investigating the factors controlling the rate of thiosulphate / acid reaction. The reaction that will be taking place will follow the rate at which sulphur is formed in the reaction of sodium thiosulphate with dilute hydrochloric acid. In the experiment the sulphur will appear as an extremely fine precipitate. This will slowly be followed by a milky appearance in the reaction mixture in the conical flask. As the amount of the sulphur in the mixture increases, the precipitate will become milkier.