Titration Practical

Use Titration Practice Plan Evaluation Equipment: · Beaker · 250 cm 3 Female Flask · Rot · Buret · Pipette · White Tile · Erlenmeyer Flask · Scaler · Scaler · Weighing Bottle · Glass Rod Method for Producing Standard Solution: About accurate weighing bottle Weigh 5 g of anhydrous sodium carbonate and record bottle weight and solid weight. The anhydrous sodium carbonate was then transferred to a clean 100 cm 3 beaker.

The purpose of this experiment is to deepen the understanding of the practical application of back titration. Counter titration is designed to solve the problems encountered with positive titration. There are many reasons why the back titration method can be used: there are many reasons: if the sample volatilizes or does not dissolve in water, if the specimen contains impurities that interfere with positive titration, it is difficult to identify the end point with positive titration. When reacting slowly with titrant. In this experiment, the weighted portion of the toothpaste was analyzed to determine the mass percentage of CaCO 3 present in the toothpaste sample. This experiment uses reverse titration technique instead of forward titration. This is because the toothpaste which is the substance to be analyzed is insoluble in water but soluble in acid.

The purpose of this experiment was to determine the proportion of calcium carbonate in toothpaste using back titration. Instead of using a standard titration method where the acid is directly titrated using a base solution of base, back titration is used as the sample CaCO 3 to be analyzed is insoluble in water. Hydrochloric acid and sodium hydroxide are reagents used in this experiment. A precisely measured amount of HCl is added to the weighted portion of CaCO 3 of the toothpaste. When the reaction between HCl and CaCO 3 was complete, the excess HCl was back-titrated with NaOH until the reaction reached the end point and the indicator changed from pink to orange. Therefore, the amount of HCl reacted with CaCO 3 can be calculated by using an initial excess of HCl to subtract the amount of HCl remaining after the reaction.

The backward titration is backward titration, instead of titrating the original sample, add a known excess of standard reagent to the solution and titrate excess standard reagent. If the end point of back titration is easier to distinguish than the end point of ordinary titration, reverse titration is useful as well as precipitation reaction. Reverse titration is also useful if the reaction between the analyte and the titrant is very slow, or if the analyte is in an insoluble solid. The composition of the solution produced by the titration method ranges from pure acid to soda ash. Identifying the pH associated with any stage of the titration process is relatively simple with monoprotonic acids and bases. The presence of more than one acid or base group complicates these calculations. Graph methods (such as equivalence graphs) have been in use for a long time to explain the coupling equilibrium interaction.