If you know that sodium bicarbonate has a solubility of 8.4 g in 100g water at 18 °C I. Calculate (a) the molarity and (b) the molality of 8.4 g of Sodium bicarbonate in water II. if you had 200 mls of water, what is the minimum amount of Sodium bicarbonate that you will require to achieve supersaturation? III. If 150 mls of a stock solution of sodium bicarbonate having a concentration of 0.5 M was diluted to 300 mls. What will be the final concentration of the diluted solution?
If you know that sodium bicarbonate has a solubility of 8.4 g in 100g water at 18 °C I. Calculate (a) the molarity and (b) the molality of 8.4 g of Sodium bicarbonate in water II. if you had 200 mls of water, what is the minimum amount of Sodium bicarbonate that you will require to achieve supersaturation? III. If 150 mls of a stock solution of sodium bicarbonate having a concentration of 0.5 M was diluted to 300 mls. What will be the final concentration of the diluted solution?
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter11: Properties Of Solutions
Section: Chapter Questions
Problem 70E: The vapor pressures of several solutions of water-propanol (CH3CH2CH2OH) were determined at various...
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If you know that sodium bicarbonate has a solubility of 8.4 g in 100g water at 18 °C
I. Calculate (a) the molarity and (b) the molality of 8.4 g of Sodium bicarbonate in water
II. if you had 200 mls of water, what is the minimum amount of Sodium bicarbonate that
you will require to achieve supersaturation?
III. If 150 mls of a stock solution of sodium bicarbonate having a concentration of 0.5 M was
diluted to 300 mls. What will be the final concentration of the diluted solution?
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What is the equation used in step 3 (mass of solute)
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