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DEPARTMENT OF CHEMISTRY FACULTY OF SCIENCE & MATHEMATICS UNIVERSITI PENDIDIKAN SULTAN IDRIS
CHEMISTRY 1 LABORATORY REPORT Student’s Name
Matric Number Lecturer’s Name
Date/Day/Time Laboratory
Muhammad Nurakmal bin Abdul Rahman D20141066985 Dr. Yusnita Binti Juahir 8/10/2014 Experiment 3 : Acid And Base Titration
Title: Acid And Base Titration
Objective: To determine the concentration of sodium hydroxide solution through titration technique using hydrochloric acid and sulfuric acid.
Introduction: Acids and bases play a central role in chemistry. The process of obtaining quantitative information of a sample using a fast chemical reaction by reacting with a certain volume of reactant whose concentration is known is called titration. When an acid-base reaction is used, the process is called acid-base titration. The neutralization of acid and base will produce salt and water Acid + Base →
O + NaCl
Neutralization occurs when acid and base where react in stoichiometry.
Apparatus
Volumetric flask
(250 Ml)
Filter funnel
Beaker
(1×250 mL)
Burette
(1×50 mL)
Pipette
(1×25 mL)
Material
100 mL 1.000× M HCl solution
100 mL 1.000× M solution
10 mL C solution NaOH (with pipette)
Phenolphthalein solution *concentration of C solution → 0.3 M*
Method : 1) 10mL of C solution were put in volumetric flask and was diluted with distilled water until to the mark and was mixed thoroughly. The solution was then transferred to a clean beaker. The solution was labeled as C. A flask was rinsed twice with water. 2) The
burette
was
rinsed
and
cleaned
with
5mL
HCl
solution
(1.000× . 25 mL of HCl solution (1.000× M) were placed to burette by using funnel. 3) The pipette was cleaned and rinsed twice using C solution. 25mL of C solution was pipetted in three Erlenmeyer flask. 2 drops of phenolphthalein indicator was added. 4) The initial volume reading was recorded to the nearest two decimal points. C solution was titrated with HCl from burette to a colourless solution end point. The final volume reading was recorded and the used volume of acid was calculated. *note : phenolphthalein colour will be changed from margenta (base) to colourless (acid)
5) The titration was repeated until the different volume of acid is in the range of 0.003 for three experiments. 6) The concentration of NaOH solution (that was in the flask) and the concentration of C was calculated. 7) Steps 3 to 7 were repeated by replace HCl with .
Result :
Reagent
First reading (mL)
Third reading (mL) 7.30
Average
7.40
Second reading (mL) 7.50
Solution C + Hydrochloric Acid Solution C + Sulphuric Acid
There were some mistakes while doing the experiment. The amount of acid used were slightly more than it should be, to prevent that happen is to check if there are any air bubbles at the nozzle of the burette. Other than that, the volumetric flask must be in cleaned and dry condition, if the volumetric flask were used back to back, this can effects the new concentration of solution. An indicator is used to indicate which point its stopped, the indicator used is phenolphthalein, at the end point, the solution in the volumetric flask will turn to pale pink.to ensure correct way of titrant we could titrate it slowly and swirl the solution a bit longer. The chemical equation is: Reaction between HCl and NaOH: HCl + NaOH →NaCl +
O
Reaction between S and NaOH:
S + 2NaOH → + 2 O The problem had took effect on our experiment, that cause our result is slightly off and not precise from the exact value.
Conclusion : The concentration and mole of both acid and base can be determined by using the formula of =
= . The accepted values of concentration
NaOH using HCl is 0.074M, but the value of concentration NaOH using is 0.077 M.
References : 1) Martin S. Silberberg (Global Edition) 2) Matriculation Chemistry Book Semester 1