| << Chapter < Page | Chapter >> Page > |
What are the mole fractions of H 3 PO 4 and water in a solution of 14.5 g of H 3 PO 4 in 125 g of water?
(a) Outline the steps necessary to answer the question.
(b) Answer the question.
What are the mole fractions of HNO 3 and water in a concentrated solution of nitric acid (68.0% HNO 3 by mass)?
(a) Outline the steps necessary to answer the question.
(b) Answer the question.
(a) Find number of moles of HNO
3 and H
2 O in 100 g of the solution. Find the mole fractions for the components.
(b) The mole fraction of HNO
3 is 0.378. The mole fraction of H
2 O is 0.622.
Calculate the mole fraction of each solute and solvent:
(a) 583 g of H 2 SO 4 in 1.50 kg of water—the acid solution used in an automobile battery
(b) 0.86 g of NaCl in 1.00 10 2 g of water—a solution of sodium chloride for intravenous injection
(c) 46.85 g of codeine, C 18 H 21 NO 3 , in 125.5 g of ethanol, C 2 H 5 OH
(d) 25 g of I 2 in 125 g of ethanol, C 2 H 5 OH
Calculate the mole fraction of each solute and solvent:
(a) 0.710 kg of sodium carbonate (washing soda), Na 2 CO 3 , in 10.0 kg of water—a saturated solution at 0 °C
(b) 125 g of NH 4 NO 3 in 275 g of water—a mixture used to make an instant ice pack
(c) 25 g of Cl 2 in 125 g of dichloromethane, CH 2 Cl 2
(d) 0.372 g of histamine, C 5 H 9 N, in 125 g of chloroform, CHCl 3
(a) (b) (c) (d)
Calculate the mole fractions of methanol, CH 3 OH; ethanol, C 2 H 5 OH; and water in a solution that is 40% methanol, 40% ethanol, and 20% water by mass. (Assume the data are good to two significant figures.)
What is the difference between a 1 M solution and a 1 m solution?
In a 1 M solution, the mole is contained in exactly 1 L of solution. In a 1 m solution, the mole is contained in exactly 1 kg of solvent.
What is the molality of phosphoric acid, H 3 PO 4 , in a solution of 14.5 g of H 3 PO 4 in 125 g of water?
(a) Outline the steps necessary to answer the question.
(b) Answer the question.
What is the molality of nitric acid in a concentrated solution of nitric acid (68.0% HNO 3 by mass)?
(a) Outline the steps necessary to answer the question.
(b) Answer the question.
(a) Determine the molar mass of HNO 3 . Determine the number of moles of acid in the solution. From the number of moles and the mass of solvent, determine the molality. (b) 33.7 m
Calculate the molality of each of the following solutions:
(a) 583 g of H 2 SO 4 in 1.50 kg of water—the acid solution used in an automobile battery
(b) 0.86 g of NaCl in 1.00 10 2 g of water—a solution of sodium chloride for intravenous injection
(c) 46.85 g of codeine, C 18 H 21 NO 3 , in 125.5 g of ethanol, C 2 H 5 OH
(d) 25 g of I 2 in 125 g of ethanol, C 2 H 5 OH
Calculate the molality of each of the following solutions:
(a) 0.710 kg of sodium carbonate (washing soda), Na 2 CO 3 , in 10.0 kg of water—a saturated solution at 0°C
(b) 125 g of NH 4 NO 3 in 275 g of water—a mixture used to make an instant ice pack
(c) 25 g of Cl 2 in 125 g of dichloromethane, CH 2 Cl 2
(d) 0.372 g of histamine, C 5 H 9 N, in 125 g of chloroform, CHCl 3
(a) 6.70 10 −1 m ; (b) 5.67 m ; (c) 2.8 m ; (d) 0.0358 m
Notification Switch
Would you like to follow the 'Ut austin - principles of chemistry' conversation and receive update notifications?
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|