Sodium Bicarbonate (NaHCO₃)

Properties of Sodium Bicarbonate:

• White crystalline powder
• Odorless
• Soluble in water
• Slightly alkaline taste
• Decomposes at high temperatures
• Chemical formula: NaHCO₃

Preparation (Solvay Process):

• Prepared industrially by-passing carbon dioxide and ammonia through a concentrated sodium chloride (brine) solution.
• Sodium bicarbonate precipitates out and is then filtered, washed, and dried.

Uses of Sodium Bicarbonate:

• As a systemic antacid to treat acid indigestion, heartburn, and upset stomach.
• As a leavening agent in baking.
• As an odor neutralizer and cleaning agent.
• In the management of metabolic acidosis and certain drug overdoses (under medical supervision).

Assay (Acid-Base Titration):

1. Prepare a Standard Solution: Dissolve a known amount of a strong acid, such as hydrochloric acid (HCl), in water to create a solution with a known concentration.
2. Sample Preparation: Weigh an accurate amount of NaHCO₃ and dissolve it in water.
3. Add Indicator: Add a pH indicator, such as phenolphthalein, to the NaHCO₃ solution. The indicator changes color at neutralization.
4. Titrate: Slowly add the standard HCl solution to the NaHCO₃ solution while stirring. NaHCO₃ reacts with HCl, forming water, carbon dioxide (CO₂), and sodium chloride (NaCl). The endpoint is reached when the indicator changes color.
5. Calculate Concentration: Measure the volume of HCl used in the titration to calculate the concentration or purity of NaHCO₃.

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