http://lawrencekok.blogspot.com

Prepared by Lawrence Kok

Tutorial on Titration Techniques, Acid/Base Titration and IA on Titrations.

Molarity- 0.1M Na2CO3

Preparation of standard (BASE)

Titration

Volumetric flask

10.6 gNa2CO3 10.6g in 1 L

Burette

Volumetric pipetteConical flask

Pipette filler

Molarity- 0.1M Na2CO3

Preparation of standard (BASE)

Titration

Volumetric flask

Unknown conc conical flask

Preparation of unknown conc of (ACID)

10.6 gNa2CO3 10.6g in 1 L

Burette

Burette

Conical flask

Volumetric pipette

Indicator

Retort stand

• Quantitative analysis - determine unknown conc of an analyte• Addition of known conc sol(standard) from burette to another sol (unknown conc) in a conical flask.• Titrant/titrator (added) + analyte/titrand (to be analyzed)

Conical flask

Pipette filler

Molarity- 0.1M Na2CO3

Preparation of standard (BASE)

Titration

Titration Set up

Titrant/Titrator

Analyte/Titrand

Titration

Notes/ sample titration calculationTitration

White tile

contain

contain

Volumetric flask

Unknown conc conical flask

Preparation of unknown conc of (ACID)

Standardization of (ACID) with standard (BASE)

10.6 gNa2CO3 10.6g in 1 L

Burette

Titration

Redox Titration Acid Base TitrationComplexometric titration

Titration

Redox Titration Acid Base TitrationComplexometric titration

Neutralization

IndicatorpH sensor Conductometric

Video on pH sensor Video on indicator Video on conductometric

measured usingmeasured using

Titration

Redox Titration Acid Base TitrationComplexometric titration

Neutralization

IndicatorpH sensor Conductometric

Changes colour (end point) at equivalent point

Indicator pKa pH rang

e

Colour Acid

Colour Base

Methyl orange 3.46 3.2- 4.4

RED Yellow

Bromophenol Blue

4.10 3.0- 4.6

Yellow Blue

Bromocresol Green

4.90 3.8- 5.4

Yellow Blue

Methyl Red 5.00 4.8- 6.0

Red Yellow

Bromothymol Blue

7.30 6.0- 7.6

Yellow Blue

Phenol Red 8.00 6.6- 8.2

Yellow Red

Phenolphthalein 9.50 8.2- 10.0

Colourless

Pink

Video on pH sensor Video on indicator Video on conductometric

measured usingmeasured using

Video on conductometric

3

1

6

2

4

5

Titration Steps/Techniques

Rinse burette – deionized water

Rinse burette – titrant

Bottom fill with titrant NOT air gap

Fix it on retort stand Record initial reading (Bottom of meniscus)

Record vol to nearest 0.01 ml

9

8 7

Add dropwise – end point is nearVery pale pink compare with control

Final vol to nearest 0.01 ml

Click here to view video

Titration

Redox Titration Acid Base Titration Complexometric titration

Neutralization

Condition for Acid/Alkali Titration-One reactant – must be standard (known conc) or capable being standardised- Equivalent point – equal amt neutralize each other- End point measurable/detectable by colour change (indicator), pH change /conductivity

Titration

Redox Titration Acid Base Titration Complexometric titration

Neutralization

Condition for Acid/Alkali Titration-One reactant – must be standard (known conc) or capable being standardised- Equivalent point – equal amt neutralize each other- End point measurable/detectable by colour change (indicator), pH change /conductivity

Acid/Base used as primary standard -Stable/solid

-Soluble in water-Does not decompose over time

Primary standard acids- Potassium hydrogen phthalate

Primary standard bases- Anhydrous sodium carbonate

10.6 gNa2CO3 10.6g in 1 L

Volumetric flask

Burette

Accurate Known conc

Volumetric flask

Burette

20.4 g KHP 20.4 g in 1L

Unknown Conc NaOH

Unknown Conc HCI

? ?

Accurate known conc

Titration

Redox Titration Acid Base Titration Complexometric titration

Neutralization

Condition for Acid/Alkali Titration-One reactant – must be standard (known conc) or capable being standardised- Equivalent point – equal amt neutralize each other- End point measurable/detectable by colour change (indicator), pH change /conductivity

Acid/Base used as primary standard -Stable/solid

-Soluble in water-Does not decompose over time

Primary standard acids- Potassium hydrogen phthalate

Primary standard bases- Anhydrous sodium carbonate

10.6 gNa2CO3

Standard 0.1M Na2CO3

10.6g in 1 L

Volumetric flask

Burette

Accurate Known conc

Unable to prepare accurate conc of NaOH/HCI due to •hygroscopic nature NaOH – absorb water vapour• HCI is in vapour state – difficult to measure amt

Volumetric flask

Burette

Standard 0.1M KHP

20.4 g KHP 20.4 g in 1L

Unknown Conc NaOH

Unknown Conc HCI

? ?

Standard

ize N

aOH

using K

HP

Standardize HCI

using Na2 CO

3

Accurate known conc

Mix till it dissolved 0.1M KHP – 0.1 mole of KHP in total vol of solution (1L)

Primary standard acid Accurate Conc 0.1M KHP

Preparing standard solution – 0.1 M

0.1 M – 0.1 mole KHP in 1 L

Mass of KHP → 0.1 mole KHP x M = 0.1 x 204.22gStep 1

Step 2

Pour from beaker to 1L volumetric flask Step 3

Add water (wash bottle) until 1L mark

Transfer to beaker, add water to dissolve it

Step 4

Step 5

20.4 g

Molarity = 0. 1 mole (0.1M) 1 L total vol (solute + solvent)

Primary standard

Mix till it dissolved 0.1M KHP – 0.1 mole of KHP in total vol of solution (1L)

Primary standard acid Accurate Conc 0.1M KHP

Preparing standard solution – 0.1 M

0.1 M – 0.1 mole KHP in 1 L

Mass of KHP → 0.1 mole KHP x M = 0.1 x 204.22gStep 1

Step 2

Pour from beaker to 1L volumetric flask Step 3

Add water (wash bottle) until 1L mark

Transfer to beaker, add water to dissolve it

Step 4

Step 5

20.4 g

Video standard solution preparation

Molarity = 0. 1 mole (0.1M) 1 L total vol (solute + solvent)

0.1M KHP

Primary standard

Mix till it dissolved 0.1M Na2CO3 – 0.1 mole of Na2CO3 in total vol of solution (1L)

Primary standard base Accurate Conc 0.1M Na2CO3

Preparing standard solution – 0.1 M

0.1M – 0.1 mole Na2CO3 in 1 L

Mass of Na2CO3 → 0.1 mole Na2CO3 x M = 0.1 x 106gStep 1

Step 2

Pour from beaker to 1L volumetric flaskStep 3

Add water (wash bottle) until 1L mark

Transfer to beaker, add water to dissolve it

Step 4

Step 5

10.6 g

Molarity = 0. 1 mole (0.1M) 1 L total vol (solute + solvent)

Primary standard

Mix till it dissolved 0.1M Na2CO3 – 0.1 mole of Na2CO3 in total vol of solution (1L)

Primary standard base Accurate Conc 0.1M Na2CO3

Preparing standard solution – 0.1 M

0.1M – 0.1 mole Na2CO3 in 1 L

Mass of Na2CO3 → 0.1 mole Na2CO3 x M = 0.1 x 106gStep 1

Step 2

Pour from beaker to 1L volumetric flaskStep 3

Add water (wash bottle) until 1L mark

Transfer to beaker, add water to dissolve it

Step 4

Step 5

10.6 g

Video standard solution preparation

Molarity = 0. 1 mole (0.1M) 1 L total vol (solute + solvent)

0.1M Na2CO3

Primary standard

Procedure

Step 1

Pipette 25.0ml NaOH in conical flask

Step 2

Fill burette with standard 0.1M KHP solution

Step 3

Step 4

Step 5

2 drops phenolthalein to NaOH – colourless to pink

Initial vol KHP recorded

Titrate until pink colour fades away

Final vol KHP recordedStep 6

Step 7 Perform rough titration, repeat till consistent result agree within 0.1cm3 (triplicate)

?

Standard 0.1M KHP

? Conc NaOH

Standardization of (BASE) with standard (ACID)

Procedure

Step 1

Pipette 25.0ml NaOH in conical flask

Step 2

Fill burette with standard 0.1M KHP solution

Step 3

Step 4

Step 5

2 drops phenolthalein to NaOH – colourless to pink

Initial vol KHP recorded

Titrate until pink colour fades away

Final vol KHP recordedStep 6

Step 7 Perform rough titration, repeat till consistent result agree within 0.1cm3 (triplicate)

Standardization of (ACID) with standard (BASE)

?

Standard 0.1M KHP

? Conc NaOH

Procedure

Standardization of (BASE) with standard (ACID)

Step 1 Step 2 Step 3 Step 4

Step 5 Step 6

Step 7

Fill burette with standard 0.1M Na2CO3 solution

Initial vol Na2CO3 recorded

Pipette 25.0ml HCI in conical flask

2 drops methyl orange to HCI – red

Titrate until red changes to pink

Final vol Na2CO3recorded

Perform a rough titration, repeat till consistent result agree within 0.1cm3 (triplicate)

Standard 0.1M Na2CO3

? Conc HCI

?

red pink

Standardization of (BASE) with standard (ACID)

Vol KHPVol KHP

Fin vol = (29.50 ± 0.05)Ini vol = (3.10 ± 0.05)

KHP vol = (26.40 ± 0.10)

Data Collection

Standardization of (BASE) with standard (ACID)

Vol KHP

Average vol KHP= 26.4 + 26.4 = 26.4cm3

2

Vol KHPFin vol = (29.50 ± 0.05)Ini vol = (3.10 ± 0.05)

KHP vol = (26.40 ± 0.10)

Uncertainty in vol KHPAdd absolute uncertainty for final + initial= (0.05 + 0.05) = ± 0.10

Average Vol KHP ± uncertainty= 26.4 + 26.4 = (26.4± 0.10)cm3

2

Data Collection Data Processing

Standardization of (BASE) with standard (ACID)

Vol KHP

Average vol KHP= 26.4 + 26.4 = 26.4cm3

2

Vol KHPFin vol = (29.50 ± 0.05)Ini vol = (3.10 ± 0.05)

KHP vol = (26.40 ± 0.10)

Uncertainty in vol KHPAdd absolute uncertainty for final + initial= (0.05 + 0.05) = ± 0.10

Average Vol KHP ± uncertainty= 26.4 + 26.4 = (26.4± 0.10)cm3

2

Data Collection Data Processing

Error Analysis

% Uncertainty - burette

Absolute uncertainty vol x 100% Average vol added= 0.10 x 100% 26.4 = 0.38%

% Uncertainty - pipette

± 0.03Absolute uncertainty vol x 100% Average vol added= 0.03 x 100% 25.00 = 0.12%

KHP

NaOH

Standardization of (BASE) with standard (ACID)

Vol KHP

Average vol KHP= 26.4 + 26.4 = 26.4cm3

2

Vol KHPFin vol = (29.50 ± 0.05)Ini vol = (3.10 ± 0.05)

KHP vol = (26.40 ± 0.10)

Uncertainty in vol KHPAdd absolute uncertainty for final + initial= (0.05 + 0.05) = ± 0.10

Average Vol KHP ± uncertainty= 26.4 + 26.4 = (26.4± 0.10)cm3

2

Data Collection Data Processing

Error Analysis

% Uncertainty - burette

Absolute uncertainty vol x 100% Average vol added= 0.10 x 100% 26.4 = 0.38%

% Uncertainty - pipette

± 0.03

Total % Uncertainty = % uncertainty burette + % uncertainty pipette = 0.38% + 0.12%

= 0.5%

Conc NaOH = 0.106 ± 0.5%( % uncertainty)

Absolute uncertainty vol x 100% Average vol added= 0.03 x 100% 25.00 = 0.12%

0.5 x 0.106 = 0.0005 = 0.001100 (% Abs uncertainty)

Conc NaOH=0.106 ± 0.001M(Absolute uncertainty)

Conc ± uncertainty % Error

Lit value - NaOH = 0.100MExpt value– NaOH = 0.106MDifference = 0.006% Error – Difference x 100% Literature value 0.006 x 100% = 6%0.100

KHP

NaOH

Standardization of (ACID) with standard (BASE)

Vol Na2CO3 Vol Na2CO3

Fin vol = (29.50 ± 0.05)Ini vol = (3.10 ± 0.05)

Na2CO3 vol = (26.40 ± 0.10)

Data Collection

Standardization of (ACID) with standard (BASE)

Vol Na2CO3

Average vol Na2CO3 = 26.4 + 26.4 = 26.4cm3

2

Vol Na2CO3

Fin vol = (29.50 ± 0.05)Ini vol = (3.10 ± 0.05)

Na2CO3 vol = (26.40 ± 0.10)

Uncertainty in vol Na2CO3 Add absolute uncertainty for final + initial= (0.05 + 0.05) = ± 0.10

Average Vol Na2CO3 ± uncertainty= 26.4 + 26.4 = (26.4± 0.10)cm3

2

Data Collection Data Processing

Standardization of (ACID) with standard (BASE)

Vol Na2CO3

Average vol Na2CO3 = 26.4 + 26.4 = 26.4cm3

2

Vol Na2CO3

Fin vol = (29.50 ± 0.05)Ini vol = (3.10 ± 0.05)

Na2CO3 vol = (26.40 ± 0.10)

Uncertainty in vol Na2CO3 Add absolute uncertainty for final + initial= (0.05 + 0.05) = ± 0.10

Average Vol Na2CO3 ± uncertainty= 26.4 + 26.4 = (26.4± 0.10)cm3

2

Data Collection Data Processing

Error Analysis

% Uncertainty - burette

Absolute uncertainty vol x 100% Average vol added= 0.10 x 100% 26.4 = 0.38%

% Uncertainty - pipette

± 0.03Absolute uncertainty vol x 100% Average vol added= 0.03 x 100% 25.00 = 0.12%

Na2CO3

HCI

Conc HCI=(0.211±0.001)M(Absolute uncertainty)

Standardization of (ACID) with standard (BASE)

Vol Na2CO3

Average vol Na2CO3 = 26.4 + 26.4 = 26.4cm3

2

Vol Na2CO3

Fin vol = (29.50 ± 0.05)Ini vol = (3.10 ± 0.05)

Na2CO3 vol = (26.40 ± 0.10)

Uncertainty in vol Na2CO3 Add absolute uncertainty for final + initial= (0.05 + 0.05) = ± 0.10

Average Vol Na2CO3 ± uncertainty= 26.4 + 26.4 = (26.4± 0.10)cm3

2

Data Collection Data Processing

Error Analysis

% Uncertainty - burette

Absolute uncertainty vol x 100% Average vol added= 0.10 x 100% 26.4 = 0.38%

% Uncertainty - pipette

± 0.03

Total % Uncertainty = % uncertainty burette + % uncertainty pipette = 0.38% + 0.12%

= 0.5%

Conc HCI = 0.211 ± 0.5%( % uncertainty)

Absolute uncertainty vol x 100% Average vol added= 0.03 x 100% 25.00 = 0.12%

0.5 x 0.211 = 0.001100 (% Absolute uncertainty)

Conc ± uncertainty % Error

Lit value - HCI = 0.200MExpt value – HCI = 0.211MDifference = 0.011% Error – Difference x 100% Literature value 0.011 x 100% = 5.5%0.200

Na2CO3

HCI

NaOHM = ? V = 25.0ml

KHPM = 0.100MV = 26.4 ml

KHP + NaOH → NaKP + H2OM = 0.100M M = ? V = 26.40ml V = 25.0ml

Mole ratio – 1: 1

HCI M = ? V = 25.0ml

Na2CO3 + 2HCI → 2NaCI + H2O + CO2

M = 0.100M M = ?V = 26.4ml V = 25.0ml

Mole ratio – 1: 2

Sample Titration Calculation

Calculation Calculation

Standardization of (BASE) with standard (ACID) Standardization of (ACID) with standard (BASE)

Na2CO3

M = 0.100MV = 26.4 ml

NaOHM = ? V = 25.0ml

KHPM = 0.100MV = 26.4 ml

KHP + NaOH → NaKP + H2OM = 0.100M M = ? V = 26.40ml V = 25.0ml

Mole ratio – 1: 1

Moles of Acid = MV = (0.100 x 0.0264) = 2.64 x 10-3

Mole ratio (1 : 1)• 1 mole acid neutralize 1 mole base• 2.64 x 10-3 acid neutralize 2.64 x 10-3 baseMoles of Base = M x V = M x 0.025M x 0.025 = 2.64 x 10-3

M = 0.106M

M aVa = 1Mb Vb 10.1 x 26.40 = 1M x 25.0 1M b = 0.106M

HCI M = ? V = 25.0ml

Na2CO3 + 2HCI → 2NaCI + H2O + CO2

M = 0.100M M = ?V = 26.4ml V = 25.0ml

Mole ratio – 1: 2

Using mole ratio Using formula

Moles of Base = MV = (0.100 x 0.0264)

= 2.64 x 10-3

Mole ratio (1 : 2)• 1 mole base neutralize 2 mole acid• 2.64 x 10-3 base neutralize 5.28 x 10-3 acidMoles of Acid = M x V = M x 0.025M x 0.025 = 5.28 x 10-3

M = 0.211M

M bVb = 1Ma Va 20.1 x 26.4 = 1Ma x 25.0 2Ma = 0.211M

Using formulaUsing mole ratio

Sample Titration Calculation

Calculation Calculation

Standardization of (BASE) with standard (ACID) Standardization of (ACID) with standard (BASE)

Na2CO3

M = 0.100MV = 26.4 ml

NaOHM = ? V = 25.0ml

KHPM = 0.100MV = 26.4 ml

KHP + NaOH → NaKP + H2OM = 0.100M M = ? V = 26.40ml V = 25.0ml

Mole ratio – 1: 1

Moles of Acid = MV = (0.100 x 0.0264) = 2.64 x 10-3

Mole ratio (1 : 1)• 1 mole acid neutralize 1 mole base• 2.64 x 10-3 acid neutralize 2.64 x 10-3 baseMoles of Base = M x V = M x 0.025M x 0.025 = 2.64 x 10-3

M = 0.106M

M aVa = 1Mb Vb 10.1 x 26.40 = 1M x 25.0 1M b = 0.106M

HCI M = ? V = 25.0ml

Na2CO3 + 2HCI → 2NaCI + H2O + CO2

M = 0.100M M = ?V = 26.4ml V = 25.0ml

Mole ratio – 1: 2

Using mole ratio Using formula

Moles of Base = MV = (0.100 x 0.0264)

= 2.64 x 10-3

Mole ratio (1 : 2)• 1 mole base neutralize 2 mole acid• 2.64 x 10-3 base neutralize 5.28 x 10-3 acidMoles of Acid = M x V = M x 0.025M x 0.025 = 5.28 x 10-3

M = 0.211M

M bVb = 1Ma Va 20.1 x 26.4 = 1Ma x 25.0 2Ma = 0.211M

Using formulaUsing mole ratio

Sample Titration Calculation

Calculation Calculation

Standardization of (BASE) with standard (ACID) Standardization of (ACID) with standard (BASE)

Na2CO3

M = 0.100MV = 26.4 ml

Click here Acid/Base calculation Click here Titration calculation

Video on Titration

Click here cal Na2CO3/HCI Click here cal NaOH/H2SO4

Titration for IA (DCP) assessment

Acid Base Titration

Standardization HCI with primary std Na2CO3

Click here for expt 4.2

Standardization NaOH with primary std KHPClick here or here for expt`

Titration bet NaOH with std HCI Click here for expt 4.2a

Titration bet HCI with std NaOH Click here for expt 4.2a

Determining water crystallization in hydrated Na2CO3 with std HCI Click here for expt 4.4

Determining ethanoic acid in vinegar with std NaOH Click here for expt 4.3

Determining acetylsalicylic acid in aspirin with std NaOH Click here or here for expt` Click here for more expt

Standardization Expt Acid/Base Titration Expt

Titration for IA (DCP) assessment

Acid Base Titration

Standardization HCI with primary std Na2CO3

Click here for expt 4.2

Standardization NaOH with primary std KHPClick here or here for expt`

Titration bet NaOH with std HCI Click here for expt 4.2a

Titration bet HCI with std NaOH Click here for expt 4.2a

Determining water crystallization in hydrated Na2CO3 with std HCI Click here for expt 4.4

Standardization KMnO4 with std ammonium iron(II) sulphate Click here for expt 4.5

Iron (II) determination with std KMnO4

Click here for expt 4.6

Hypochlorite (OCI-) in bleach with iodine/thiosulphate Click here for expt 4.8

Determining ethanoic acid in vinegar with std NaOH Click here for expt 4.3

Copper(II) determination in brass with iodine/thiosulphate Click here or here for expt` Click here for more expt

Standardization KI/I2 with std KIO3 Click here for expt 4.7 Click here for more expt

Determining acetylsalicylic acid in aspirin with std NaOH Click here or here for expt` Click here for more expt

Vit C determination with iodine/thiosulphate Click here or here for expt Click here more detail expt

Standardization Expt Acid/Base Titration Expt

Standardization Expt

Redox Titration Expt

Redox Titration

Standardization KI/I2

with std sodium thiosulphate Click here for expt 4.7 Iodine/thiosulphate (iodometric titration)

Click here on titration simulationClick here on titration simulation

Video on Titration

Click here titration simulationClick here titration simulation Click here titration simulation

Simulation on Titration

Click here titration NaOH /HCI Click here titration video

Acknowledgements

Thanks to source of pictures and video used in this presentation

Thanks to Creative Commons for excellent contribution on licenseshttp://creativecommons.org/licenses/

Prepared by Lawrence Kok

Check out more video tutorials from my site and hope you enjoy this tutorialhttp://lawrencekok.blogspot.com