Αποτελέσματα Αναζήτησης
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:
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.
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`
Epsom salt (MgSO 4 ·7H 2 O) is a heptahydrate of magnesium sulfate: within one mole of magnesium sulfate heptahydrate are seven moles of water. This water can be driven off by heat to form the anhydrous (dehydrated) ionic compound, magnesium sulfate.
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.
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 (\(\ce{MgSO4*7H2O}\)).
By solving this we will get $ n = 10 $ . The hydrated salt was $ N{a_2}S{O_4}.10{H_2}O $ . So, option D is correct. Note Sodium sulphate is used as a thermal storage.
