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A hydrated salt, Na 2 SO 4. nH 2 O undergoes 56% loss in weight on heating and become anhydrous. The value of n(approximately) will be : (PLEASE ANSWER IN A EASY TO UNDERSTAND MANNER)
1 Ιουν 2019 · The hydrated salt, `Na_(2)SO_(4)*nH_(2)O` undergoes `55.9%` loss in weight on heating and becomes anhydrous. The value of `n` will be: A. `5` B. `3` C. `7` D. `10`
7 Ιουν 2024 · The water of crystallisation is separated from the main formula by a dot when writing the chemical formula of hydrated compounds. E.g. hydrated copper (II) sulfate is CuSO 4∙ 5H 2 O. A compound which doesn’t contain water of crystallisation is called an anhydrous compound. E.g. anhydrous copper (II) sulfate is CuSO 4.
8 Ιουλ 2024 · Here, \( Na2SO4 \) is sodium sulfate and \( nH2O \) represents the water of hydration. Step 2: Calculate the molar mass of the components - The molar mass of \( Na2SO4 \): - Sodium (Na): \( 22.99 \, g/mol \times 2 = 45.98 \, g/mol \) - Sulfur (S): \( 32.07 \, g/mol \) - Oxygen (O): \( 16.00 \, g/mol \times 4 = 64.00 \, g/mol \) Total for ...
7 Ιουν 2024 · A compound that contains water of crystallisation is called a hydrated compound. The water of crystallisation is separated from the main formula by a dot when writing the chemical formula of hydrated compounds. E.g. hydrated copper (II) sulfate is CuSO 4∙ 5H 2 O.
2 Νοε 2023 · Salts that contain water within their structure are called hydrated salts. Anhydrous salts are those that contain no water in their structure. A common example is copper (II) sulfate which crystallises forming the salt hydrated copper (II) sulfate, which is blue.
What is the formula of the hydrate? Solution: 1) Determine mass of water driven off: 15.67 − 7.58 = 8.09 g of water. 2) Determine moles of MgCO 3 and water: MgCO 3 ---> 7.58 g / 84.313 g/mol = 0.0899 mol H 2 O ---> 8.09 g / 18.015 g/mol = 0.449 mol.
