Title:
Acid base titration –Define the end point by using various indicators
Aim:
To define the end point of an acid-base titration effect by using various indicators.
Introduction:
The titration is a scientific method applied to define the specific amount of a substance by the substance with a known amount of another substance. The completed reaction of a titration is normally shown by the colour change or an electrical measurement.
The elements needed to be applied in a titration as a standard amount of the material present is precisely identified. The standard can be present both in the form of a pure substance or standard solution which solution whose composition is precisely identified. The standard can be equipped in two ways, primary standard or standardize by titration against some previously standardized solution. A primary standard
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Within the acid-base titration process, the molarity of antacid A, B and C can be found. The molarity of antacid A is 0.107 M, antacid B is 0.054 M and antacid C is 0.083 M
The reaction in the acid-base titrations is neutralization. During the neutralization, an acid and base react to produce salt and water. For example is when hydrogen ion (H+) reacts with hydroxyl ion (OH-) produce water (H2O). Since the reactants are colourless, a suitable indicator should be used to indicate the colour change at the end point.
The equivalence point can be determined through titration by adding minimum amounts of a substance (indicator). The colour will change when the equivalence point reached the solution. When a strong base is titrated with a strong acid or vice versa the pH of the solution will be about 7.0 at the equivalence point. The indicator used in this experiment is phenolphthalein. Phenolphthalein turned pink in alkaline solutions and colourless in acidic
These color changes indicate a chemical change, which show that a reaction had occurred. In the first step when o-vanillin and p-toludine, imine was formed. The color change from green to orange suggests that imine appears as orange colored. In the second step, the addition of sodium borohydride reduced the imine into another derivative, which was yellowish lime color. The solution turned clear when acids and anhydrides was added, which indicated the precipitate were dissolved.
Later on the color changed to green, which indicated the pH was 8.0. Then when we tested the pH with the pH strips they both showed the pH as being 5.0. After that, we added HCl or stomach acid and both drugs dissolved and were soluble. We tested the pH and it dropped to 1.0. They both turned a brownish-yellow when the iron nitrate was added and no other pain reliever or antacid looked like those two.
Standard Sodium hydroxide solution is the alkaline solution that will be used to titrate with soda water as it is a common solution that can be easily found in an ordinary school laboratory. It is a strong base. Carbonic acid is a weak acid which will react with a strong base to form a basic (pH > 7) solution. When Phenolphthalein is added to Soda water, the resultant solution is colourless. After titration with a strong base (sodium hydroxide), the solution will turn to pink as the solution becomes
The Problem: How does temperature affect the dissolving time of an antacid tablet? Antacid tablets are medicines that help neutralize the acid in your stomach. Antacid tablets are made of numerous numbers of components, such as sodium bicarbonate (baking powder), magnesium hydroxide, critic acid, and many others. When Antacid tablets are placed in water, they undergo a chemical reaction, where the sodium bicarbonate breaks apart to make sodium and bicarbonate ions. When the bicarbonate ions collide with hydrogen ions, it produces carbonic acid.
The percent recovery of the copper was calculated using the equation, percent recovery = (the mass of the copper recovered after all the chemical reactions/the initial mass of the copper) x 100. The amount of copper that was recovered was 0.32 grams and the initial mass of the copper was 0.46 grams. Using the equation, (0.32 grams/0.46 grams) x 100 equaled 69.56%. The amount of copper recovered was slightly over two-thirds of the initial amount.
In this experiment rate of reaction with different reactants concentration: KI (0.010 M), KBrO3 (0.040 M), and HCl (0.10 M) will be observed. So, this is reaction between iodide and bromate ion under acidic conditions: 6 I- (aq) +BrO3-(aq)+ H+(aq)→ 3I2(aq) + Br-(aq)+ 3H2O The end of the reaction, will be determined by observing color change of solution. Thus, solution should shange color to blue.
CLAIRE MUNTING 29/01/2018 Criterion C EFFECTS OF SURFACE AREA OF CALCIUM CARBONATE UPON RATE OF REACTION Calcium Carbonate Chips 1 Introduction: Within the current investigation, the effects of the surface area of Calcium Carbonate (CaCO3) in combination with Hydrochloric acid (HCl) upon its rate of reaction. CaCO3, commonly referred to as limestone, is an organic substance and is, in a sense, the crystallised “carbonic salt” of the element, calcium2. In addition to being a salt, the pH level of Calcium Carbonate is 9.91, and it is therefore, a basic substance, due to the fact that it is comprised of a pH level higher than 7, which is neutral3. HCl, however, is the bodily acid found in the stomach of human beings.
Verna Wang Hannah Palmer CHEM 101-069 Lab 11-19-16 Stoichiometry and Limiting Reagents Lab Report Purpose: We are using the reaction of sodium hydroxide and calcium chloride to illustrate stoichiometry by demonstrating proportions needed to cause a reaction to take place. Background: Just like a recipe would call for a specific amount of one ingredient to a specific amount of another, stoichiometry is the same exact method for calculating moles in a chemical reaction. Sometimes, we may not have enough of or too much of one ingredient , which would be defined as limiting and excess reagent, respectively.
In test tube E, a colourless colour formed. It is because redox reaction occurred during the test. Idoine reduced into idoine ion , which changre from brown to colourless. In test tube F, the iodine solution change from brown to purple . It is because the salt has a function of cofactor which will shorten the time for amylase to take to break down the
The equation of the reaction between sodium hydroxide and ethanoic acid is as follows: CH3COOH + NaOH → CH3COONa + H2O We can measure the end point of titration process and we can also measure the amount of reactants. The concentration of ethanoic acid in the vinegar can be determined through stoichiometric calculations, Using the values obtained from the titration, and also the chemical equation as a reference. Phenolphthalein indicator is used in this acid-base titration Equipment and materials:
Its pH is greater than 7 and turns red litmus paper into blue. Acid- base neutralization is done by adding an acid to a base or a base to an acid until the substance has equal hydrogen and hydroxide ions. This is used to determine unknown concentration of a
To identify the unknown acid. 4. To determine acid dissociation constant, Ka and pKa for the unknown acid. Introduction: Titration process is used in an acid-base experiment in order to determine the concentrations of solutions of acids and bases.
The solution with the pigments was spotted 15 times on both region A and region B and then allowed to dry. When the plate was dry it was placed into the tank for at least 20
Introduction The goal of the experiment is to examine how the rate of reaction between Hydrochloric acid and Sodium thiosulphate is affected by altering the concentrations. The concentration of Sodium thiosulfate will be altered by adding deionised water and decreasing the amount of Sodium thiosulphate. Once the Sodium thiosulphate has been tested several times. The effect of concentration on the rate of reaction can be examined in this experiment.
That caused a new initial reading of NaOH on the burette (see Table1 & 2). The drops were caused because the burette was not tightened enough at the bottom to avoid it from being hard to release the basic solution for titrating the acid. The volume of the acid used for each titration was 25ml. The volume of the solution was then calculated by subtracting the initial volume from the final volume. We then calculated the average volume at each temperature.