Acid-base neutralization titration is a method to determine the alkali (or acid) of unknown substances with the acid (or alkali) of known substances. So how to write the experimental report of acid-base titration in college chemistry? The following is the sample report of acid-base titration experiment in college chemistry that I compiled for you _ Acid-base neutralization titration test report. Welcome to learn from it, I hope it will help you.

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Part I: Acid-base neutralization titration test report

_ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ Class (in English)

First, the experimental purpose

In this experiment, hydrochloric acid is used as the standard solution to determine the unknown solution (to be measured)

In this experiment, the concentration of sodium hydroxide is the solution to be tested.

Second, the experimental principle

In the acid-base neutralization reaction, the new acid (or alkali) solution is completely neutralized by the new alkali (or acid) solution, and the concentration of the alkali (or acid) solution can be calculated according to the ratio of the amount of acid and alkali in the chemical equation. Calculation formula: c(NaOH)?

c(HCl)？ V(HCl)c(NaOH)？ sodium hydroxide

Or c(HCl)? .

Sodium hydroxide and hydrochloric acid

Third, experimental supplies.

Acid burette, alkaline burette, conical flask, iron frame, burette clamp, 0. 1000mol/L hydrochloric acid (standard solution), NaOH solution with unknown concentration (solution to be tested), phenolphthalein (color change range 8.2~ 10).

1, the essence of acid-base reaction is.

2. Phenolphthalein is used as indicator in acid-base neutralization titration, but the color change point of titration end point is not pH=7. Does this affect the judgment of neutralization titration end point?

3. What is the difference between burette and measuring cylinder reading?

Third, data recording and processing.

Fourth, the discussion of the problem.

What is the key of acid-base neutralization titration?

Part II: Experimental report on acid-base neutralization titration.

1. experimental purpose: 1. Cultivate students' experimental idea of "testing the unknown with the known by experimental means".

2. Learn how to use relevant instruments and master the principle and operation steps of acid-base titration.

3. Realize the combination of learning and doing.

2. Experimental instruments and drugs:

Instruments: titration stand, 25mL acid (alkali) burette, 10mL pipette and two 250mL conical bottles.

Drugs: 0. 1mol/L NaOH solution, 0. 1mol/L hydrochloric acid, 0.05mol/L oxalic acid (oxalic acid dihydrate), phenolphthalein reagent and methyl orange reagent.

3. Experimental principle: Neutralization titration is an acid-base reaction to generate salt and water.

Section, using the known to measure the unknown. That is, the acid (alkali) solution with known concentration and the alkali (acid) solution with unknown concentration are completely neutralized, and the volumes of the two are determined, and then the concentration of the unknown solution is calculated according to the stoichiometry of the two in the chemical equation. Acid-base titration usually uses hydrochloric acid solution and sodium hydroxide solution as standard solutions. However, because concentrated hydrochloric acid is volatile, sodium hydroxide can easily absorb water and carbon dioxide in the air, so it cannot be directly prepared into a solution with precise concentration. Generally, the solution with approximate concentration is prepared first, and then calibrated with reference material. In this experiment, oxalic acid (oxalic acid dihydrate) was used as the reference substance.

Calibration of (1) sodium hydroxide solution: H2C2O4+2NaOH=Na2C2O4+2H2O.

When the reaction reaches the end point, the solution is weakly alkaline, and phenolphthalein is used as an indicator. (Parallel titration twice)

⑵ hydrochloric acid solution calibration: HCl+NaOH=NaCl+H2O.

When the reaction reached the end point, the solution was weakly acidic, and methyl orange was used as an indicator. (Parallel titration twice)

Four. Experimental contents and steps:

1. Instrument leak detection: acid (alkali) burette leak detection.

2. Instrument cleaning: clean the burette and conical flask as required, and wet the burette.

3. Add 10.00mL oxalic acid (oxalic acid dihydrate) to the two conical bottles with a pipette, and then drop two drops of phenolphthalein respectively. Add the medicine to the basic burette until it is higher than the zero dividing line, expel all bubbles, adjust the liquid level to the zero dividing line, and record the reading.

4. Titrate the oxalic acid (oxalic acid dihydrate) solution with sodium hydroxide solution, shake the conical flask circumferentially in the same direction, and keep the solution from colorless to pink for 30 seconds, then it can be considered as reaching the end point and record the reading.

5. Add 10.00 mL sodium hydroxide solution into two cleaned conical bottles with a pipette, and then drop two drops of methyl orange respectively. Add hydrochloric acid solution to the acid burette to 2-3 cm above the zero dividing line, discharge all bubbles, adjust the liquid level to the zero dividing line, and record the reading.

6. Titrate the sodium hydroxide solution with hydrochloric acid solution. When the solution in the conical flask changes from yellow to orange and remains unchanged for 30 seconds, it can be considered that the titration end point has been reached, and the reading is recorded.

7. Clean up the experimental instruments and clean the experimental platform.

Verb (abbreviation of verb) data analysis;

1. calibration of sodium hydroxide solution concentration: experimental report of acid-base titration.

2. Calibration of hydrochloric acid solution concentration: acid-base titration experimental report

Experimental results: ① The measured concentration of sodium hydroxide solution is 0.100 mol/L/L.

② The measured concentration of hydrochloric acid is 0.1035 mol/L/L.

7. Error analysis: The purpose of judging the solution concentration error is the concentration of the solution to be tested and the consumption of the standard solution.

Is proportional to the volume.

Possible factors causing errors and results analysis: ① visual field (reading) ② flushing (instrument flushing) ③ leakage (liquid overflow).

(4) Bubble (bubble at the tip of burette) (5) Color (indicator discoloration control and selection)

8. Precautions: ① The burette must be wetted and rinsed with the corresponding solution to be tested for 2-3 times.

② The conical flask cannot be wetted by the liquid to be tested.

(3) The bubbles at the tip of burette must be exhausted.

(4) Make sure that the end point has been reached and there are no droplets at the tip of the burette.

⑤ During titration, droplets will not form a line. When the color of the liquid in the conical flask changes slowly, add it drop by drop, shake the solution evenly after adding one drop, and observe the color change. When approaching the finish line, control the droplets to hang and not fall, lean down with a conical bottle, then blow with a washing bottle and shake well.

6. When reading, the line of sight must be at the lowest point of the concave surface of the liquid level.

Part III: Experimental report on acid-base neutralization titration.

Experimental name: acid-base neutralization titration

Time Experiment (Grouping) Table Number Partner Lecturer

One: experimental purpose:

The solution with known concentration (standard solution) is used, and the concentration of unknown solution (solution to be tested) is determined by using hydrochloric acid as the standard solution and sodium hydroxide as the solution to be tested in this experiment.

Two: experimental instruments:

Acid burette, alkaline burette, conical flask, iron frame (including burette clamp).

Experimental drug: 0. 1000mol/L hydrochloric acid (standard solution), NaOH solution with unknown concentration (solution to be tested), acid-base indicator: phenolphthalein (color change range 8~ 10) or methyl orange (3. 1~4.4).

Three: experimental principle:

C (standard) ×V (standard) = c (to be )× V (to be) The stoichiometric ratio of the reaction is 1: 1. This experiment is concrete: c(H+)×V (acid) = c(OH-)×V (alkali).

Four: Experimental process:

(A) the preparation stage before titration

1, leak detection: check whether the burette leaks water (specific method: acid burette, add water to burette, and close the piston. Let it stand for 5 minutes to see if there is any water leakage. If there is leakage, vaseline must be applied to the piston. Be careful not to smear too much, so as not to block the piston mouth. The leak detection method of alkaline burette is to add water to the burette and close the piston. Let it stand for 5 minutes to see if there is any water leakage. If there is leakage, the rubber tube must be replaced. )

2. Rinse: rinse the burette with distilled water first, and then wet it with the liquid to be filled for 2-3 times. Conical bottles can be cleaned with distilled water and are not allowed to be wet or dry.

3. Measurement: Measure a certain volume (e.g. 20.00ml) of NaOH solution with unknown concentration with an alkaline burette (note, adjust the initial scale.

Below 0 or 0 scale) into the conical flask.

Measure the hydrochloric acid standard solution with an acid burette, remove all bubbles, adjust the liquid level so that the liquid level is just at or below the 0 scale, and record the reading.

V 1, read the second place after the decimal point.

(2) titration stage

1. Put the conical flask under the acid burette and add 1-2 drops of phenolphthalein (if the color is not obvious, put the conical flask on a white porcelain plate or white paper). Drop the solution in the burette into the conical flask drop by drop. During titration, the right hand keeps shaking the conical flask, and the left hand controls the titration.

Observe the color change of the solution in the conical flask with eyes by holding the piston until the solution becomes colorless after dropping a drop of hydrochloric acid, and the original color will not be restored within half a minute. At this point, sodium hydroxide is completely neutralized by hydrochloric acid, reaching the titration end point. Record the level gauge V2 after titration.

2. Pour the solution in the conical flask into the waste liquid tank, clean the conical flask with distilled water, and repeat the above operation for 2~3 times.

(3) experimental records

(4). Experimental data record:

Treatment of experimental results of verbs (abbreviation of verb);

C (waiting) =c (standard) ×V (standard) /V (waiting) Pay attention to the average number of times.

Sixth, experimental evaluation and improvement:

[Based on: c(H+)×V (acid) = c(OH-)×V (alkali) analysis]

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