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Neutralization Titration
Titration method using acid-base reactions.
Acid
Substance providing hydrogen ions in solution.
Base
Substance providing hydroxide ions in solution.
Conjugate Acid
Species formed when a base accepts a proton.
Conjugate Base
Species formed when an acid donates a proton.
pH
Negative logarithm of hydrogen ion concentration.
pKa
Negative logarithm of the acid dissociation constant.
Buffer
Solution resisting changes in pH upon addition of acid/base.
Standard VS
Standard volume solution used in titrations.
Indicator
Substance that changes color at a specific pH.
Arrhenius Concept
Acids produce H+; bases produce OH- in water.
Brønsted-Lowry Concept
Acids donate protons; bases accept protons.
Lewis Acid
Substance that accepts electron pairs in reactions.
Lewis Base
Substance that donates electron pairs in reactions.
Equivalence Point
Point in titration where acid equals base.
Hydronium Ion Concentration
Concentration of H3O+ in solution.
Strong Acid
Acid that completely dissociates in solution.
Weak Acid
Acid that partially dissociates in solution.
Strong Base
Base that completely dissociates in solution.
Weak Base
Base that partially dissociates in solution.
Titration
Technique to determine concentration of a solution.
Neutralization Reaction
Reaction between an acid and a base.
HCl
Hydrochloric acid, a strong acid.
H2SO4
Sulfuric acid, a strong diprotic acid.
NaOH
Sodium hydroxide, a strong base.
H2CO3
Carbonic acid, a weak acid.
NH4
Ammonium ion, a weak acid.
pH 7
Neutral pH, indicating equal H+ and OH-.
pH < 7
Acidic solution, higher H+ concentration.
pH > 7
Basic solution, higher OH- concentration.
Calculating pH
Using pH = -log[H+].
Strong Acid
Completely dissociates in solution, releasing H+ ions.
Strong Base
Completely dissociates in solution, releasing OH- ions.
Weak Acid
Partially dissociates in solution, equilibrium established.
Weak Base
Partially dissociates in solution, equilibrium established.
Neutralization Titration
Process of determining concentration through acid-base reaction.
Equivalence Point
Point where moles of acid equals moles of base.
Acid-Base Indicator
Substance that changes color at specific pH levels.
pH Range
Interval over which an indicator changes color.
Malachite Green
Indicator with color change from yellow to green.
Methyl Yellow
Indicator with color change from red to yellow.
Bromophenol Blue
Indicator with color change from yellow to blue.
Methyl Orange
Indicator with color change from pink to yellow.
Bromocresol Green
Indicator with color change from yellow to blue.
Methyl Red
Indicator with color change from red to yellow.
Bromocresol Purple
Indicator with color change from yellow to purple.
Bromothymol Blue
Indicator with color change from yellow to blue.
Phenol Red
Indicator with color change from yellow to red.
Cresol Red
Indicator with color change from yellow to red.
Thymol Blue
Indicator with color change from yellow to blue.
Phenolphthalein
Indicator with color change from colorless to red.
Thymolphthalein
Indicator with color change from colorless to blue.
Titrant
Solution of known concentration used in titration.
Analyte
Substance being analyzed in a titration.
Primary Standard
Highly pure substance used for standardization.
Standard Acid Solutions
Common acids used for titration standardization.
Hydrochloric Acid
Strong acid commonly used in titrations.
Sulfuric Acid
Strong acid used in various titration processes.
Normality (N)
Concentration unit equivalent to equivalents per liter.
Molarity (M)
Concentration unit equivalent to moles per liter.
Endpoint
Point in titration where reaction is complete.
Salmon Pink Endpoint
Color change indicating endpoint with methyl orange.
Chemical Reaction
Process where reactants transform into products.
1N NaOH
Normal solution concentration of sodium hydroxide.
Carbon dioxide-free water
Water free from dissolved CO2 for accurate results.
Weighing bottle
Container used for precise weighing of solids.
Drying at 120°C
Process to remove moisture from NaOH.
Saturated barium hydroxide solution
Used to prepare KOH standard solution.
Stoppered bottle
Container to prevent contamination during storage.
Polyolefin container
Type of container resistant to chemical reactions.
Dissolve 20 g NaOH
Initial step in preparing NaOH solution.
Dilute to 1L
Final step to achieve desired solution volume.
Primary standard
Substance of known concentration for titration.
Phenolphthalein indicator
Used to determine endpoint in acid-base titrations.
Light pink color
Indicates endpoint in titration with phenolphthalein.
Normality of HCl
Concentration measure for acid used in titration.
Weight of reagents
Amount needed to neutralize HCl solution.
Sulphuric acid solution
Acid used in titration with NaOH.
Equivalent volume
Volume of one solution that reacts with another.
Sodium carbonate
Base used in titration experiments.
Assay of Sodium Bicarbonate
Determination of purity of NaHCO3 sample.
Balanced chemical equation
Shows reactants and products in a chemical reaction.
Endpoint color transition
Color change indicating completion of titration.
Official requirement
Purity standards for sodium bicarbonate.
Volume required for titration
Amount of titrant needed for complete reaction.
Titer value
Concentration of titrant used in titration.
Standard deviation
Measure of variation in assay results.
Coefficient of variation
Standard deviation relative to the mean.
Precision/accuracy assessment
Evaluation of measurement reliability and correctness.
Assay of Sodium Hydroxide
Determination of purity of NaOH sample.
Mixed Indicators
Indicators providing sharp color contrast in pH changes.
Sodium Hydroxide Assay
Measures total alkali content in NaOH.
Official Requirement NaOH
NaOH must be 95.0-100.5% total alkali.
Chemical Reaction NaOH
2NaOH + H2SO4 → Na2SO4 + 2H2O.
Methyl Yellow
Indicator with pH range 2.9-4.0, red to yellow.
Bromophenol Blue
Indicator with pH range 3.0-4.6, yellow to blue.
Methyl Orange
Indicator with pH range 3.2-4.4, pink to yellow.
Bromocresol Green
Indicator with pH range 4.0-5.4, yellow to blue.
Methyl Red
Indicator with pH range 4.2-6.2, red to yellow.
Bromocresol Purple
Indicator with pH range 5.2-6.8, yellow to purple.
Note 
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