A certain organic compound O has a solubility in acetone of 14.1g/L at 20.°C Calculate the...
A certain organic compound O has a solubility in acetone of 14.1g/L at 20.°C Calculate the mass of O required to prepare 50.mL of a saturated solution of O in acetone at this temperature. Round to 2 sig figs
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A certain organic compound O has a solubility in acetone of
14.1g/L at 20.°C Calculate the...
A certain molecular compound M has a solubility in acetonitrile of 0.212g/mL at 25.°C. Calculate the...
A certain molecular compound M has a solubility in acetonitrile of 0.212g/mL at 25.°C. Calculate the greatest mass of M that could be dissolved in 400.mL of acetonitrile at this temperature. You may assume the volume of the solution doesn't change as the M is dissolved.Be sure your answer has the correct unit symbol and 3 significant digits.
a. At a certain temperature, the solubility of potassium iodate, KIO3, is 36.8 g/L. Calculate its...
a. At a certain temperature, the solubility of potassium iodate, KIO3, is 36.8 g/L. Calculate its solubility product constant for this temperature. b. At a certain temperature, the solubility of cadmium fluoride, CdF2, is 0.185 mol/L. Calculate its solubility product constant for this temperature. c. At a certain temperature, the solubility product constant* of copper (II) iodate, Cu(IO3)2, is 4.08x10-8 M3. Calculate the solubility of this compound for this temperature.
At a certain temperature* (probably not 25 °C), the solubility of silver sulfate, Ag2SO4, is 0.012...
At a certain temperature* (probably not 25 °C), the solubility of silver sulfate, Ag2SO4, is 0.012 mol/L. Calculate its solubility product constant for this temperature. SIG. FIG. (required because number is small) Solubility product constants are very temperature sensitive. They are generally reported at 25°C. Not necessarily using this temperature allows me some flexibility. Answer: At a certain temperature, the solubility of potassium iodate, KIO3, is 36.1 g/L. Calculate its solubility product constant for this temperature. Answer: At a certain...
1. Compound X has a solubility in toluene of 18 mg per 100 mL at 20...
1. Compound X has a solubility in toluene of 18 mg per 100 mL at 20 °C, and a solubility of 0.64 g per 100 mL at 70 °C. You are given a sample of 0.48 g of compound X which is contaminated with 25 mg of compound Y. A. If compound Y is always soluble in toluene, describe in detail how you could separate Y from X. Would x now be pure? B. If compound Y has approximately the same values of...
At a certain temperature" (probably not 25 °C), the solubility of silver sulfate, Ag2SO4, is 0.013...
At a certain temperature" (probably not 25 °C), the solubility of silver sulfate, Ag2SO4, is 0.013 mol/L. Calculate its solubility product constant for this temperature. SIG. FIG. (required because number is small) *Solubility product constants are very temperature sensitive. They are generally reported at 25 °C. Not necessarily using this temperature allows me some flexibility, Answer: I
Consider 15 mL of an aqueous solution containing 2.0 g of an organic solute.If the distribution...
Consider 15 mL of an aqueous solution containing 2.0 g of an organic solute.If the distribution coefficient for the solute between ether and water is 20, calculate the percent of the compound that can be recovered with a single extraction with 26.8 mL of ether. (2 sig figs)
A chemist adds 975.0 mL of a 0.00988g/L magnesium fluoride solution to a flask. Calculate the...
A chemist adds 975.0 mL of a 0.00988g/L magnesium fluoride
solution to a flask. Calculate the mass in grams of magnesium
fluoride the chemist has added to the flask. round your answer to
three sig figs.
A chemist adds 975.0 mL of a 0.00988 g/L magnesium fluoride (MgF2) solution to a flask. Calculate the mass in grams of magnesium fluoride the chemist has added to the flask. Round your answer to 3 significant digits. x 5 ?
Q1: Part 1) The solubility product (Ksp) of AuCl3(s) is 3.2 × 10-25. Calculate the molar...
Q1: Part 1) The solubility product (Ksp) of AuCl3(s) is 3.2 × 10-25. Calculate the molar solubility of AuCl3(s) in pure water and with the molar solubility found, calculate the solubility of AuCl3(s) in units of mg AuCl3/mL in pure water. The molar mass of AuCl3 is equal to 303.33 g AuCl3/mol AuCl3. Part 2 )Calculate the molar solubility of AuCl3(s) in an aqueous 1.5 M NaCl solution. Q2: Calculate the pH of a solution if 75.0 mL of 0.195...
Ksp = 2.5x10-13 for Pb(103)2 at 25 °C. Calculate the molar concentration of iodate ions in...
Ksp = 2.5x10-13 for Pb(103)2 at 25 °C. Calculate the molar concentration of iodate ions in a saturated lead(II) iodate solution at 25°C using the assumption that the solution is ideal -- i.e. the activity coefficients are 1. (Your answer should be precise to three sig figs.) Submit Answer Tries 0/5 Still assuming an ideal solution, what mass of Pb(103)2 would be dissolved in 100. mL of saturated solution at 25 °C? (Your answer should be precise to three sig...
8-12 U uturucu Ur unsaturated? A compound has a solubility in water of 40 g/L at...
8-12 U uturucu Ur unsaturated? A compound has a solubility in water of 40 g/L at 0°C. If 62 g of this compound is added to 1.5 L of water at 0°C, is the resulting solution saturated or unsaturated?
At a certain temperature* (probably not 25 °C), the solubility of silver sulfate, Ag2SO4, is 0.012 mol/L. Calculate its solubility product constant for this temperature. SIG. FIG. (required because number is small) Solubility product constants are very temperature sensitive. They are generally reported at 25°C. Not necessarily using this temperature allows me some flexibility. Answer: At a certain temperature, the solubility of potassium iodate, KIO3, is 36.1 g/L. Calculate its solubility product constant for this temperature. Answer: At a certain...
At a certain temperature" (probably not 25 °C), the solubility of silver sulfate, Ag2SO4, is 0.013 mol/L. Calculate its solubility product constant for this temperature. SIG. FIG. (required because number is small) *Solubility product constants are very temperature sensitive. They are generally reported at 25 °C. Not necessarily using this temperature allows me some flexibility, Answer: I
A chemist adds 975.0 mL of a 0.00988g/L magnesium fluoride
solution to a flask. Calculate the mass in grams of magnesium
fluoride the chemist has added to the flask. round your answer to
three sig figs.
A chemist adds 975.0 mL of a 0.00988 g/L magnesium fluoride (MgF2) solution to a flask. Calculate the mass in grams of magnesium fluoride the chemist has added to the flask. Round your answer to 3 significant digits. x 5 ?
Ksp = 2.5x10-13 for Pb(103)2 at 25 °C. Calculate the molar concentration of iodate ions in a saturated lead(II) iodate solution at 25°C using the assumption that the solution is ideal -- i.e. the activity coefficients are 1. (Your answer should be precise to three sig figs.) Submit Answer Tries 0/5 Still assuming an ideal solution, what mass of Pb(103)2 would be dissolved in 100. mL of saturated solution at 25 °C? (Your answer should be precise to three sig...
8-12 U uturucu Ur unsaturated? A compound has a solubility in water of 40 g/L at 0°C. If 62 g of this compound is added to 1.5 L of water at 0°C, is the resulting solution saturated or unsaturated?
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