Its a subject all about Analytical Chemistry which datas about the experiment.

1. GROUP 2 - MLS 1C
Learning Activity No. 11
Midterm POST - LABORATORY Presentation
BONIFACIO, FEROLINO, CONSTANTINO, CAL,
DELACRUZ, GOMEZ

2. (01) SPECIFIC LEARNING OBJECTIVES
(02) INTRODUCTION
(03) RATIONALE / GOVERNING PRINCIPLES
(04) INFORMATION TABLE AND ACTUAL GARNERED DATA
(05) ANALYSIS AND CONCLUSION

3. To prepare and standardize 1N Sodium Hydroxide

4. This experiment primarily involves the
standardization process of a specific solution,
namely NaOH. This entails the dissolving NaOH from
its solid pellet form into a solution in distilled water.
To titrate with NaOH solution until it reaches a light
pink color, which indicates the endpoint,
phenolphthalein will be used as an indicator.
Ultimately, the normality of the NaOH solution is
determined through this process.

5. The second standard is the eleventh governing principle for this learning
exercise. The chemical being standardized using the primary standard is what we
mean when we refer to it as the second standard. The primary standard in this
instance is hydrochloric acid, while the secondary standard is sodium hydroxide.
Once a solution's precise concentration is attained, hydrochloric acid can be utilized
as a titrant in the following tests. Thus, making it as a secondary standard.
Since sodium hydroxide will be our secondary standard and hydrochloric acid
our primary standard, the preparation of hydrochloric acid must come first in this
experiment before proceeding to the following step. Our equation will therefore be
as follows: the reagent will be sodium hydroxide plus hydrochloric acid, and the
product will be sodium chloride plus water. The normality of sodium hydroxide is
equal to the normality of hydrochloric acid multiplied by the hydrochloric acid
volume, according to the formula provided to solve this problem. Once the solution is
obtained, divide it by the sodium hydroxide volume. And that's how the secondary
standard answer is solved.

6. TRIAL 1 TRIAL 2
A. Final Reading (HCl) 5.3 mL 5.0 mL
B. Initial Reading (HCl) 0.0 mL 0.0 mL
C. Volume of (HCl) 20 mL 20 mL

7. D. Final Reading (NaOH) 20.2 mL 20.1 mL
E. Initial Reading (NaOH) 0.0 mL 0.0 mL
F. Volume NaOH used 20.2 mL 20.1 mL
G. Normality of NaOH 0.1157 N 0.1177 N
H. Average Normality of NaOH 0.2334 N or 0.2 N

8. TRIAL 1:
N NaOH = N HCl x V HCl/ V NaOH
N NaOH = 0.441 x 5.3 / 20.2
= 0.1157 N or 0.1 N
TRIAL 2:
N NaOH = N HCl x V HCl/ V NaOH
N NaOH = 0.473 x 5.0 / 20.1
= 0.1177 N or 0.1 N
AVERAGE NORMALITY: 0.2334 N or 0.2 N

9. There are two trials in all. We drain 20 milliliters of stand HCl solution from the Geisslerburet. Two
drops of phenolphthalein were introduced after 40 milliliters of distilled water. Using a Mohr
buret, we titrate NaOH until the endpoint is light pink. Then, in both experiments, they produced a
light pink color. Thus, both trials have the same volume of NaOH consumed which is 20 milliliters.

11. • The NaOH solution is prepared by dissolving a known mass of NaOH pellets or flakes in a precise volume of distilled water.
This process ensures the concentration of the solution is accurately determined.
• A primary standard, such as potassium hydrogen phthalate (KHP), is employed as a standard acid to standardize the
mixture. A burette is used to titrate the solution against the standard acid solution until the endpoint is reached, which is
usually signaled by a shift in color from pink to colorless.
• The volume and concentration of the NaH solution used in the titration are the used to calculate the
exact concentration of the NaOH solution.

12. The preparation and standardization of NaOH solution are crucial processes in analytical
chemistry, ensuring precision in numerous experiments and analyses. We can ensure
consistent and dependable outcomes in their study by carefully monitoring and calibrating the
concentration of NaOH.
The preparation involves precisely weighing NaOH pellets and dissolving them in distilled
water to get the desired concentration. Titration with a primary standard acid solution, often
HCl, was used to achieve standardization, with an endpoint determined by an appropriate
indicator. This procedure is based on the stoichiometric principle, which states that the
reaction between NaOH and acid occurs in a 1:1 ratio, allowing for exact determination of the
NaOH concentration.
Following thorough titration and computations, the concentration of the NaOH solution
was found to be within acceptable ranges of accuracy and precision. The results were
consistent across several trials, showing that the standardized solution is reliable for use.
The effective preparation and standardization of NaOH solution ensures the accuracy
and reliability of analytical data received from various chemical investigations. This
standardized solution is an invaluable resource for us, giving a consistent baseline for
conducting experiments and calibrating devices, thereby furthering scientific knowledge and
discovery.

13. JAZELLE FAITH DELA CRUZ
(RATIONALE/GOVERNING PRINCIPLES)
CARYL GUILLEN GOMEZ
(SPECIFIC LEARNING OBJECTIVES)
GABRIELLE NEVIC FEROLINO
(INTRODUCTION)
FRANCIS MIGEL BONIFACIO
(INFORMATION TABLE/ACTUAL GATHERED DATA)
(DOCUMENTATION)
IRHA CONSTANTINO
(ANALYSIS)
MICHAEL SIDNEY CAL
(CONCLUSION)