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Enter your answer in the provided box. What mass of KI is dissolved in 600.0 g...
Enter your answer in the provided box. What mass of insulin must be dissolved in 39.0 mL of water to produce a solution with an osmotic pressure of 16.1 mmHg at 25°C? The molar mass of insulin is 5808 g/mol. answer in g.
Enter your answer in the provided box. A solution of 1.55 g of solute dissolved in 25.0 mL of H20 at 25°C has a boiling point of 100.850°C. What is the molar mass of the solute if it is a nonvolatile nonelectrolyte and the solution behaves ideally (d of H20 at 25°C = 0.997 g/mL)? g/mol
What mass of KI is dissolved in 700.0 g of a solution that is 65.0% KI by mass?
2 attempts left Check my work Enter your answer in the provided box. A solution of 1.15 g of solute dissolved in 25.0 mL of H20 at 25°C has a boiling point of 100.750°C. What is the molar mass of the solute if it is a nonvolatile nonelectrolyte and the solution behaves ideally (d of H20 at 25°C = 0.997 g/mL)? g/mol
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Enter your answer in the provided box. What is the molality of a solution containing 4.37g of urea [(NH2)2 CO] in 176.5 g of water? Be sure to answer all parts. A solution of 0.790 g of an organic compound in 100.0 g of benzene has a freezing point of 5.166°C. What are the molality of the solution and the molar mass of the solute? The normal freezing point of benzene is 5.500 C and the...
Enter your answer in the provided box. Calculate the composition of the following solution in mass/volume %: 40.0 g benzene per 1.00 x 102 mL % benzene Calculate the volume, in L, of water that must be added to dilute 22.9 mL of 10.5 M HCl to 0.0900 M HCl. Enter your answer in the provided box. L water
Enter your answer in the provided box. What mass of ethylene glycol must be added to 1545 g water to raise the boiling point to 104.7°C?
Enter your answer in the provided box. Report problem Hint Solution A 0.2639-g sample of a monoprotic acid neutralizes 52.25 mL of a 0.08015 M KOH solution. Calculate the molar mass of the acid. Guided Solution g/mol
Enter your answer in the provided box. An iron bar has a mass of 543 g. After the bar had been standing in air for a month, exactly one-eighth of the iron turned to rust (Fe2O3). Calculate the final mass of the iron bar and the rust.
Enter your answer in the provided box. What is the pH of 650.0 mL of an aqueous solution containing 0.135 g of HCI?