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The water present in the latter case is called water of hydration or water of crystallization. Common examples of minerals that exist as hydrates are gypsum (\(\ce{CaSO4*2H2O}\)), Borax (\(\ce{Na3B4O7*10H2O}\)) and Epsom salts (\(\ce{MgSO4*7H2O}\)).
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`
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:
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.
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 ...
Solution. Suggest Corrections. 25. Similar questions. Q. The hydrated salt, N a2SO4.nH2O undergoes 56 % loss in weight on heating and become anhydrous. The value of n will be: Q. The hydrated salt, N a2SO4.nH2O undergoes 56% loss in weight on heating and becomes anhydrous. The value of n (approx.) will be : Q.
Experiment two: 0.416 g of CoCl 2· nH 2 O was dissolved in water, and an excess of sodium hydroxide (NaOH) was added. The cobalt hydroxide salt was filtered and heated in a flame, forming 0.145 g of cobalt (III) oxide. Determine the value of 'n' from each experiment.
