Why does the solubility of sodium sulfate decahydrate decrease with increase in temperature?
Answers
Answer:
Because the solubility is inversly proportionaly to the temperature of substance
Answer:
Explanation:Due to the fact that this salt is found as a hydrated salt (first Na2SO4.10H20 and then as Na2SO4.7H2O, so, with the increase of temperature it looses moisture (water)). When the Na2SO4.10H2O is heated the solution of this compound decreases because a solid phase and a liquid phase are formed after the initial heating.
The solubility actually increased up to 32.4 degrees Celsius, then declines. This is explain by the following:
Sodium sulfate is naturally found as a decahydrate complex (has 10 water molecules in the crystal for every molecule of sodium sulfate). At 32.4 degress Celsium, the crystal breaks into a sulfate liquid phase and and an anydrous solid phase, or in other words, the extra molecules in the complex detach from the sodium sulfate part of the salt.