to verify law of conservaticonservation of mass Na2SO+BACL2?
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Procedure:
Step 1: 100 mL distilled water is poured in two beakers (150 mL).
Step 2: The physical balance and a watch glass of known mass are used, weigh 7.2 g of BaCl2 .2H2O and dissolved in a beaker (150 mL) containing 100 mL distilled water.
Step 3: Similarly, 16.1 g of Na2SO4.10H2O is weighed in another watch glass of known mass and dissolved in another beaker (150 mL) containing 100 mL distilled water.
Step 4: The third beaker (250 mL) is taken and weighed using a spring balance and polythene bag.
Step 5: Both solutions of 150 mL beakers is mixed in the third beaker (250 mL). The contents are mixed using a glass stirrer.
Step 6: White precipitate of BaSO4 appears on mixing due to precipitation reaction.
Step 7: The beaker containing the reaction mixture is weighed again to determine the mass of the precipitation reaction products.
Step 8: The masses of before and after the chemical reaction are compared.
Step 1: 100 mL distilled water is poured in two beakers (150 mL).
Step 2: The physical balance and a watch glass of known mass are used, weigh 7.2 g of BaCl2 .2H2O and dissolved in a beaker (150 mL) containing 100 mL distilled water.
Step 3: Similarly, 16.1 g of Na2SO4.10H2O is weighed in another watch glass of known mass and dissolved in another beaker (150 mL) containing 100 mL distilled water.
Step 4: The third beaker (250 mL) is taken and weighed using a spring balance and polythene bag.
Step 5: Both solutions of 150 mL beakers is mixed in the third beaker (250 mL). The contents are mixed using a glass stirrer.
Step 6: White precipitate of BaSO4 appears on mixing due to precipitation reaction.
Step 7: The beaker containing the reaction mixture is weighed again to determine the mass of the precipitation reaction products.
Step 8: The masses of before and after the chemical reaction are compared.
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