NaHCO3

NaHCO3 is sodium bicarbonate (also called baking soda). Key points - Formula and name: NaHCO3; sodium hydrogen carbonate. - Structure: Na+ cation and the bicarbonate (HCO3−) anion. - Molar mass: about 84.01 g/mol. - Physical form: white, crystalline powder; soluble in water. - Basicity: in water, solution is mildly basic (pH ~8.3 for modest concentrations). Important reactions - Thermal decomposition (when heated): 2 NaHCO3(s) → Na2CO3(s) + CO2(g) + H2O(g) - Reaction with acids (e.g., in baking or lab titrations): NaHCO3 + HCl → NaCl + CO2 + H2O (1:1 molar ratio of NaHCO3 to CO2 produced) - Buffering: participates in the carbonic acid/bicarbonate buffering system (CO2/H2CO3 ⇌ HCO3− ⇌ CO3^2− in solution) Common uses - Baking/leavening agent: releases CO2 to make dough rise. - Antacid: relieves heartburn by neutralizing stomach acid. - Cleaning agent and deodorizer; gentle abrasive and deodorizing action. - Fire suppression: small dry-chemical extinguishant uses. Safety - Low toxicity but can irritate eyes/skin; avoid inhalation of dust; follow standard lab/safety guidelines. Quick practice problems - Problem 1: How much CO2 is produced from heating 5.0 g of NaHCO3? Steps: Molar mass NaHCO3 ≈ 84.01 g/mol. Moles NaHCO3 = 5.0 / 84.01 ≈ 0.0595 mol. From the reaction 2 NaHCO3 → Na2CO3 + CO2 + H2O, 2 moles NaHCO3 give 1 mole CO2. CO2 moles = 0.0595 / 2 ≈ 0.0298 mol. Mass CO2 ≈ 0.0298 × 44.01 ≈ 1.31 g. - Problem 2: How many grams of NaHCO3 are needed to neutralize 50.0 mL of 1.00 M HCl? Moles HCl = 0.050 L × 1.00 M = 0.050 mol. Stoichiometry: 1:1 NaHCO3 to HCl, so 0.050 mol NaHCO3. Mass NaHCO3 ≈ 0.050 mol × 84.01 g/mol ≈ 4.20 g. Would you like a short flashcard set, or problems tailored to a specific course topic (stoichiometry, acid-base, or organic/inorganic)?