using english to predict rendement in chemical reaction

In chemistry, the chemical yield, the yield of the reaction, or only the rendement refers to the amount of reaction product produced in the chemical reaction. [1] Absolute rendement can be written as weight in grams or in moles (molar yield). The relative yield used as a calculation of the effectiveness of the procedure is calculated by dividing the amount of product obtained in moles by the theoretical yield in moles:
Rendemen fractional = rendemen actual / theoretical rendemen
To obtain a percentage yield, multiply the fractional yield by 100%.

One or more reactants in chemical reactions are often used redundantly. The theoretical rendement is calculated based on the number of moles of the limiting reagent. For this calculation, it is usually assumed that there is only one reaction involved.

The ideal chemical yield value (theoretical rendement) is 100%, a value highly unlikely to be achieved in its practice. Calculate the percentage of rendement that is by using the following equations percent rendemen = weight yield / weight of yield divided by the sample weight multiplied by 100%.

We can learn with this practice :

ASETAT / CUKA ACID (CH3COOH)
WITH 0.1 N NaOH

Name : M. Aljaziri Badruzaman

Date of practice :

I. Purpose
The purpose and objective of this practicum is for the practitioner to know and understand how to determine the level of acetic acid with 0.1 N NaOH.

II. Tools and reagents
Tools :
# Erlenmeyer 250 ml
# Pipette volume 10 ml + 25 ml
# Buret 50 ml
# Cup cup 100 ml
# Funnels
Reactor :
** NaOH 0.1 N
** Acetic acid (Vinegar)
** PP Indicators
Reaction:
NaOH + CH3COOH >>> CH3COONa + H2O

III. Ways of working :
Clean and rinse buret with distilled water.
^^^
Bilasi and buret contents with 0.1 N NaOH solution until full and dihimpitka drawn (scale) zero.
  ^^^
Pipette 25 ml of acetic acid into 100 ml measuring flask, dilute to the line mark.
^^^
Beat the 12 x solution.
  ^^^
Pipette 10 ml aqueous solution into the erlenmeyer.
  ^^^
Spend 2 drops of PP indicator.
  ^^^
Titar with NaOH solution from burette to pink point of end.
  ^^^
Calculate the acetic acid level in% or g / l.

IV. Data and calculations
BE = BM = 60
Final volume: 39.60 ml
Initial Volume: 0.00 ml -
Titration volume: 39.60 ml
Final volume: 39.50 ml
Initial Volume: 0.00 ml -
Titration volume: 39.50 ml
# Average titration volume = (39.60 + 39.50): 2 = 39.55 ml
#Chart of CH3COOH = X ml x N. NaOH x P x BE = 39.55 ml x 0.1N x (100 x 1000) x 60: 250 = 39.55 x 0.1 x 400 x 60 = 94.920 mg / l = 94.920 g / l
#% CH3COOH = acetic acid concentration (g / l) x 100%
1000 x BJ (considered 1)
= 94.920 x 100%
1000
= 9,492%

V. Discussion:
In diluting the standard solution must be precisely coined zero (scale) in order to keep acetic acid content or unchanged. Then the solution should be shaken at least 12x for a homogeneous solution and the final result is appropriate. In this experiment, the indicator used is penolftalin (PP) with a pH trajectory between 8.2 to 10, because the guitar is a strongly alkaline NaOH. In practice, it should be done 2 times the experiment so that the results more accurate in determining levels. The difference between the 2 experiments is a maximum of 0.1 ml. In doing the titration should be careful because if less will only affect the final result. The result of end pointing should be pink because at that time the solution is neutral.

VI. Conclusion:
Thus, CH3COOH levels of 94.920 g / l or 9.492%