Preparation & standadization of NaOH & HCL
ABABIO BUAHEN SAMUEL
CHEMISTRY ONE
REF. NO: 20216815
EXPERIMENT A.1.1.2
THE PREPARATION AND STANDARDIZATION OF NaOH AND HCL SOLUTION
AIMS & OBJECTIVES:
(1) To gain experience with titration procedure
(2) To learn to standardize acid & base solution
(3) To carry out the preparation of solution of a desired concentration
(4) To carry out the preparation of solutions of desired concentration from more concentrated solution
INTRODUCTION:
Titration is a convenient quantitative method for accurately determining unknown concentrations of solutions. A necessary requirement for its use is that a standard solution (a solution of known concentration) reacts chemically with the solution whose concentration is being determined. The standard solution is added to a solution of unknown concentration until all of the unknown solution has reacted. From the known quantity and molarity (or normality) of the standard solution and the measured volume of unknown solution used, the unknown concentration can be calculated. For example, standard base solution (NaOH) is added from a burette to an accurately known volume of the acid solution (HCl).
CHEMICALS/EQUIPMENT:
Burette, retort stand & clamp, pipette, measuring cylinder, 500ml volumetric flask, 3 conical flasks, methyl orange,2g of NaOH salt,12M HCl,0.3g of oxalic acid dehydrate, distilled water, wash bottle ,analytical balance.
PROCEDURE (A): TITRATION OF 0.1 NaOH AGAINST 1.0G OXALIC ACID
(1) 250ml of about a 0.1M NaOH solution is prepared from the solid NaOH. (2) Accurately weigh 3 samples of about 0.1g of reagent grade oxalic acid dehydrate into 3 conical flasks.
(3) Add about 50ml of distilled water to dissolve the acid & add few drops of phenolphthalein
(4) Rinse the burette out couple of times with distilled water & the solution to be standardized. Fill the burette with NaOH ensuring that all air bubbles are displaced from the burette tip.
CHEMISTRY ONE
REF. NO: 20216815
EXPERIMENT A.1.1.2
THE PREPARATION AND STANDARDIZATION OF NaOH AND HCL SOLUTION
AIMS & OBJECTIVES:
(1) To gain experience with titration procedure
(2) To learn to standardize acid & base solution
(3) To carry out the preparation of solution of a desired concentration
(4) To carry out the preparation of solutions of desired concentration from more concentrated solution
INTRODUCTION:
Titration is a convenient quantitative method for accurately determining unknown concentrations of solutions. A necessary requirement for its use is that a standard solution (a solution of known concentration) reacts chemically with the solution whose concentration is being determined. The standard solution is added to a solution of unknown concentration until all of the unknown solution has reacted. From the known quantity and molarity (or normality) of the standard solution and the measured volume of unknown solution used, the unknown concentration can be calculated. For example, standard base solution (NaOH) is added from a burette to an accurately known volume of the acid solution (HCl).
CHEMICALS/EQUIPMENT:
Burette, retort stand & clamp, pipette, measuring cylinder, 500ml volumetric flask, 3 conical flasks, methyl orange,2g of NaOH salt,12M HCl,0.3g of oxalic acid dehydrate, distilled water, wash bottle ,analytical balance.
PROCEDURE (A): TITRATION OF 0.1 NaOH AGAINST 1.0G OXALIC ACID
(1) 250ml of about a 0.1M NaOH solution is prepared from the solid NaOH. (2) Accurately weigh 3 samples of about 0.1g of reagent grade oxalic acid dehydrate into 3 conical flasks.
(3) Add about 50ml of distilled water to dissolve the acid & add few drops of phenolphthalein
(4) Rinse the burette out couple of times with distilled water & the solution to be standardized. Fill the burette with NaOH ensuring that all air bubbles are displaced from the burette tip.