Skip this Video
Download Presentation
بنام خدا عباس بهرامی عضو هیات علمی گروه بهداشت حرفه ای دانشکده بهداشت دانشگاه علوم پزشکی کاشان

Loading in 2 Seconds...

play fullscreen
1 / 30

بنام خدا عباس بهرامی عضو هیات علمی گروه بهداشت حرفه ای دانشکده بهداشت دانشگاه علوم پزشکی کاشان - PowerPoint PPT Presentation

  • Uploaded on

بنام خدا عباس بهرامی عضو هیات علمی گروه بهداشت حرفه ای دانشکده بهداشت دانشگاه علوم پزشکی کاشان [email protected] انتظار میرود در پایان جلسه دانشجو بتواند :. 1-روش تیتریمتری را توضیح دهد. 2- انواع تیتریمتری را بیان کند. Titration. Titration

I am the owner, or an agent authorized to act on behalf of the owner, of the copyrighted work described.
Download Presentation

PowerPoint Slideshow about ' بنام خدا عباس بهرامی عضو هیات علمی گروه بهداشت حرفه ای دانشکده بهداشت دانشگاه علوم پزشکی کاشان' - noleta

An Image/Link below is provided (as is) to download presentation

Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author.While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server.

- - - - - - - - - - - - - - - - - - - - - - - - - - E N D - - - - - - - - - - - - - - - - - - - - - - - - - -
Presentation Transcript

بنام خدا

عباس بهرامی

عضو هیات علمی گروه بهداشت حرفه ای

دانشکده بهداشت

دانشگاه علوم پزشکی کاشان

[email protected]


انتظار میرود در پایان جلسه دانشجو بتواند :

  • 1-روش تیتریمتری را توضیح دهد.
  • 2- انواع تیتریمتری را بیان کند.
  • Titration
    • A procedure in which one substance (titrant) is carefully added to another (analyte) until complete reaction has occurred.
      • The quantity of titrant required for complete reaction tells how much analyte is present.
  • Volumetric Analysis
    • A technique in which the volume of material needed to react with the analyte is measured
titration vocabulary
Titration Vocabulary
  • Titrant
    • The substance added to the analyte in a titration (reagent solution)
  • Analyte
    • The substance being analyzed
  • Equivalence point
    • The point in a titration at which the quantity of titrant is exactly sufficient for stoichiometric reaction with the analyte.
titration vocabulary1
Titration Vocabulary
  • End point
    • The point in a titration at which there is a sudden change in a physical property, such as indicator color, pH, conductivity, or absorbance. Used as a measure of the equivalence point.
  • Indicator
    • A compound having a physical property (usually color) that changes abruptly near the equivalence point of a chemical reaction.
titration vocabulary2
Titration Vocabulary
  • Titration error
    • The difference between the observed end point and the true equivalence point in a titration
  • Blank Titration
    • One in which a solution containing all reagents except analyte is titrated. The volume of titrant needed in the blank titration should be subtracted from the volume needed to titrate unknown.
titration vocabulary3
Titration Vocabulary
  • Primary Standard
    • A reagent that is pure enough and stable enough to be used directly after weighing. Then entire mass is considered to be pure reagent.
  • Standardization
    • The process whereby the concentration of a reagent is determined by reaction with a known quantity of a second reagent.
titration vocabulary4
Titration Vocabulary
  • Standard Solution
    • A solution whose composition is known by virtue of the way it was made from a reagent of known purity or by virtue of its reaction with a known quantity of a standard reagent.
  • Direct Titration
    • One in which the analyte is treated with titrant, and the volume of titrant required for complete reaction is measured.
titration vocabulary5
Titration Vocabulary
  • Back Titration
    • One in which an excess of standard reagent is added to react with analyte. Then the excess reagent is titrated with a second reagent or with a standard solution of analyte.
titration calculations
Titration Calculations
  • Titration Calculations rely heavily on the ability to perform stoichiometric calculations.
  • Examples
1. Neutralization

2. NaOH + HCl  H2O + NaCl

2NaOH + H2SO4  2H2O + Na2SO4

3. Twice as much HCl was required. Because it takes twice as much HCl (one H) as H2SO4 (two Hs) to neutralize the same amount of NaOH


0.60 mol NaOH


1 mol H2SO4





0.175 mol H2SO4

2 mol NaOH

4. H2SO4(aq) + 2NaOH(aq)  2H2O + Na2SO4(aq)

# L H2SO4=

5. #H x MA x VA = #OH x MB x VB

0.010 LNaOH

= 0.01714 L = 17.1 mL

titration problems
Titration problems
  • What volume of 0.10 mol/L NaOH is needed to neutralize 25.0 mL of 0.15 mol/L H3PO4?
  • 25.0 mL of HCl(aq) was neutralized by 40.0 mL of 0.10 mol/L Ca(OH)2 solution. What was the concentration of HCl?
  • A truck carrying sulfuric acid is in an accident. A laboratory analyzes a sample of the spilled acid and finds that 20 mL of acid is neutral-ized by 60 mL of 4.0 mol/L NaOH solution. What is the concentration of the acid?
  • What volume of 1.50 mol/L H2S will neutral-ize a solution containing 32.0 g NaOH?
titration problems1
Titration problems

1. (3)(0.15 M)(0.0250 L) = (1)(0.10 M)(VB)

VB= (3)(0.15 M)(0.0250 L) / (1)(0.10 M) = 0.11 L

2. (1)(MA)(0.0250 L) = (2)(0.10 M)(0.040 L)

MA= (2)(0.10 M)(0.040 L) / (1)(0.0250 L) = 0.32 M

3. Sulfuric acid = H2SO4

(2)(MA)(0.020 L) = (1)(4.0 mol/L)(0.060 L)

MA = (1)(4.0 M)(0.060 L) / (2)(0.020 L) = 6.0 M

4. mol NaOH = 32.0 g x 1 mol/40.00 g = 0.800 (2)(1.50 mol/L)(VA) = (1)(0.800 mol)

VA= (1)(0.800 mol) / (2)(1.50 mol/L) = 0.267 L

titration summary
Titration summary
  • For titrations we use the formula:

#H x MA x VA = #OH x MB x VB

Or NA x VA = NB x VB

  • NA is the combination of MA and #H
  • N is also known as normality
  • You can think of it a neutralizing power
  • We will stick with the first equation, you do not have to know N or what it stands for
  • This is a simplification of stoichiometry. We could get the same answer by working with moles (n = MV) and by using the balanced chemical equation
titration showdown
Titration showdown
  • Titration competition (best with a burette): find the concentration of an H2SO4 solution – it could be anywhere from 0-18 mol/L
  • You will use the NaOH that you prepared two weeks ago and your vast knowledge of titration procedures and formulas.
  • The wining team, is the team closest to the correct value.
  • The only restriction is : don’t put base in the burette – only acid.
sources of error
Sources of error
  • NaOH was not exactly 0.10 mol/L
  • Calculation errors (e.g. converting mL to L)
  • Not rinsing and drying the beaker for the acid
  • Over titrating (ideally, 2 titrations should be done – one to get a rough estimate, and one to get the exact value).
  • Acid or base left on the side of the flask or on the tip of the burette (for greater precision, water is used to rinse the tip of the burette).
  • Errors reading volumes.
  • Using pipette (10 mL is measured from 0 mL to 10 mL, not from 10 mL to empty)
  • Using 10 mL of base vs. 25-50 mL

For more lessons, visit



NaOH, KOH, LiOH, MW : 40.00 (NaOH); CAS: 1310-73-2 RTECS: WB490000


and basic salts 56.11 (KOH) 1310-58-3 TT2100000 (KOH)

23.95 (LiOH) 1310-65-2 OJ6307070 (LiOH)


METHOD: 7401, Issue 2 EVALUATION: FULL Issue 1: 15 February 1984

Issue 2: 15 August 1994

OSHA : 2 mg/m3 (NaOH)

NIOSH: C 2 mg/m3/15 min (NaOH); Group I Pesticide

ACGIH: C 2 mg/m3 (NaOH)

PROPERTIES: basic, hygroscopic, caustic solids and

aerosols; VP not significant

SYNONYMS: alkali; caustic soda; lye; sodium hydroxide; potassium hydroxide




(1-μm PTFE membrane)

FLOW RATE: 1 to 4 L/min

VOL-MIN: 70 L @ 2 mg/m3

-MAX: 1000 L

SHIPMENT: routine


STABILITY: at least 7 days @ 25 °C [1,2]

BLANKS: 2 to 10 field blanks per set

PTFE Polytetrafluoroethylene; polyperfluoroethylene; tetrafluoroethene

homopolymer; Teflon.




ANALYTE: OH- (alkalinity)

EXTRACTION: 5.00 mL 0.01 N HCl, 15 min under

nitrogen with stirring

TITRATION: 0.01 N NaOH under nitrogen, endpoint

by pH electrode

CALIBRATION: 0.01 N NaOH standardized with

0.01 N HCl

RANGE: 0.14 to 1.9 mg (as NaOH) per sample [1]

ESTIMATED LOD: 0.03 mg per sample (as NaOH) [1]

(7 x 10-4 moles of alkalinity)

PRECISION (S r): 0.033 @ 0.38 to 1.5 mg NaOH

per sample [1]



RANGE STUDIED: 0.76 to 3.9 mg/m3 [1]

(360-L samples)

BIAS: 5.6%

OVERALL PRECISION (Sˆ rT): 0.062 [1]

ACCURACY: ± 16.2%

APPLICABILITY: The working range is 0.4 to 5.4 mg/m 3 for a 360-L air sample. The method measures total alkalinity of alkali

hydroxides, carbonates, borates, silicates, phosphates, and other basic salts, expressed as equivalents of NaOH.


INTERFERENCES: Carbon dioxide in the air may react with alkali on the filter to produce carbonates but does not interfere when

titrated. The carbonates will produce the equivalent amount of strong alkali that was consumed on the filter [1]. Acid a erosols

may neutralize the sample, if present, producing a negative interference.

OTHER METHODS: This revises Methods S381 [2] and P&CAM 241 [3].

NIOSH Manual of Analytical Methods (NMAM), Fourth Edition, 8/15/94



1. Sodium carbonate, primary standard grade.

2. Hydrochloric acid stock solution, 0.1 N.

Standardize with sodium carbonate primary


3. Dilute hydrochloric acid, 0.01 N. Dilute 10.0

mL 0.1 N stock HCl to 100 mL in a volumetric

flask with distilled water.

4. Water, distilled, CO 2-free. Boil and cool under

N2 or bubble nitrogen through distilled water

for 30 min. Store with an Ascarite trap.

5. Nitrogen, compressed.

6. Sodium hydroxide, 50% w/v.* Dissolve 50 g

NaOH in CO 2-free distilled water and dilute to

100 mL.

7. Stock sodium hydroxide, 0.1 N. Dilute 8 mL

50% NaOH to 1.0 L with CO 2-free distilled

water. Store under Ascarite or other CO 2-

absorbing trap.

8. Working sodium hydroxide solution, 0.01 N.

Dilute 10 mL stock (0.1 N NaOH) to 100 mL

with CO2-free distilled water.

9. Standard buffer solutions, pH 4 and 7.

* See Special Precautions



1. Sampler: 37-mm diameter PTFE membrane

filter (Millipore, Fluoropore or equivalent), 1.0-

μm pore size, supported by a cellulose backup

pad in a cassette filter holder.

2. Personal sampling pump, 1 to 4 L/min, with

flexible connecting tubing.

3. pH meter with pH electrode and recorder.

4. Titration vessel, 150 to 200 mL beaker, flask

or jar with cover containing openings for the

pH electrode and N 2 inlet and outlet.

5. Stirrer, magnetic, and stir bar.

6. Glass rod, ca. 5-mm diameter and 10 cm long

to hold filter under liquid surface in titration


7. Pipets, 5- and 10-mL.

8. Volumetric flasks, 100-mL and 1-L.

9. Burets, 50-mL, readable to 0.1 mL.

10. Tweezers.



SPECIAL PRECAUTIONS: NaOH solutions are corrosive to tissue [4]. Handle with care.

1. Calibrate each personal sampling pump with a representative sampler in line.

2. Sample at an accurately known flow rate between 1 and 4 L/min for a sample size of 70 to 1000

L. Do not exceed a filter loading of ca. 2 mg total dust.



3. Transfer the sample filter to a titration vessel with tweezers. Place the filter face down in the

titration vessel.

4. Place the end of a glass rod in the center of the filter to maintain the filter below the liquid

surface during the analysis.

5. Cover the titration vessel, add 5.00 mL 0.01 N HCl, start the magnetic stirrer and N 2 purge (ca.

0.1 L/min).

6. Allow to stand 15 min (with stirring).



7. Calibrate the pH meter with pH 4 and pH 7 buffer solutions.

8. Standardize aliquots of the 0.1 N HCl stock solution with sodium carbonate in triplicate [3].

a. Dry 3 to 5 g primary standard grade Na 2CO3 at 250 °C for 4 h. Cool in a desiccator.

b. Weigh ca. 2.5 g Na 2CO3 to the nearest mg. Dissolve and dilute to exactly 1 L with CO 2-free

distilled water. The concentration is ca. 0.05 N Na2CO3.

c. Place 5.00 mL 0.05 N Na2CO3 solution into a titration vessel and titrate potentiometrically to

a pH of 5.



d. Remove electrodes, rinse them into the titration vessel, and bubble N 2 gas through contents

of the titration vessel for 3 to 5 min to remove dissolved CO 2.

e. Proceed with the titration to the inflection point.

f. Calculate the normality of the stock HCl solution