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 calculation Titration

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 Titration Complexometric titration

Neutralization

Indicator pH sensor Conductometric

Changes colour (end point) at equivalent point

Indicator pKa pH range

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

Video on conductometric

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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 near Very 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

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

? ?

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 204.22g Step 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 106g Step 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

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 recorded Step 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 KHP

Average vol KHP = 26.4 + 26.4 = 26.4cm3

2

Vol KHP Fin vol = (29.50 ± 0.05) Ini vol = (3.10 ± 0.05) KHP vol = (26.40 ± 0.10)

Uncertainty in vol KHP Add 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 = 0.001 100 (% Abs uncertainty)

Conc NaOH=0.106 ± 0.001M (Absolute uncertainty)

Conc ± uncertainty % Error

Lit value - NaOH = 0.100M Expt value– NaOH = 0.106M Difference = 0.006 % Error – Difference x 100% Literature value

0.006 x 100% = 6%

0.100

KHP

NaOH

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 = 0.001 100 (% Absolute uncertainty)

Conc ± uncertainty % Error

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

0.200

Na2CO3

HCI

NaOH

M = ? V = 25.0ml

KHP M = 0.100M V = 26.4 ml

KHP + NaOH → NaKP + H2O M = 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 base Moles of Base = M x V = M x 0.025 M x 0.025 = 2.64 x 10-3

M = 0.106M

M aVa = 1 Mb Vb 1 0.1 x 26.40 = 1 M x 25.0 1

M 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 acid Moles of Acid = M x V = M x 0.025 M x 0.025 = 5.28 x 10-3

M = 0.211M

M bVb = 1 Ma Va 2 0.1 x 26.4 = 1 Ma x 25.0 2

Ma = 0.211M

Using formula Using mole ratio

Sample Titration Calculation

Calculation Calculation

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

Na2CO3 M = 0.100M V = 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 stdNa2CO3

Click here for expt 4.2

Standardization NaOH with primary std KHP Click 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 simulation Click here on titration simulation

Video on Titration

Click here titration simulation Click here titration simulation Click here titration simulation

Simulation on Titration

Click here titration NaOH /HCI Click here titration video