Ans 14 :
Density = mass / volume
1.00 g/mL = m / 455 mL
m = 455 g
mass of solution = mass of water + mass of Fe(NO3)3
= 455 g + 14.5 g
= 469.5 g
Now one mole of Fe(NO3)3 weighing 241.86 grams has 55.845 g of Fe iron and 186.0147 g of nitrate
so 14.5 g of Fe(NO3)3 will have : ( 14.5 g x 55.845 g ) / 241.86 g = 3.348 g iron
and : (14.5 g x 186.0147 g ) / 241.86 g = 11.152 g of nitrate
so mass percent of iron = ( mass iron / mass solution ) x 100
= (3.348 g / 469.5 g ) x 100
= 0.713 %
mass percent of nitrate = ( mass nitrate / mass solution ) x 100
= (11.152 g / 469.5 g ) x 100
= 2.38 %
14. If a solution is made by dissolving 14.5 g of Fe(NO3)3 in 455 ml of...
14. If a solution is made by dissolving 14.5 g of Fe(NO3)3 in 455 ml of water, what is the mass percent of iron and nitrate in this solution? Assume 1.00 g/ml density of the water. 4 pts
Determine the molality of a solution made by dissolving 0.134 moles of glucose in 471 mL of water. Assume the density of water is 1.00 g/mL. Determine the molality of a solution made by dissolving 28.1 g of CH3OH in 513 g of H20.
Calculate the percent by mass of a solution made by dissolving 34.0g of NH3 in 2.00 x 10^3 mL of water. (molar mass NH3 = 17.04 g/mol, density of H20 = 1.00 g/mL).
If 2.63 g Fe(NO3), is dissolved in enough water to make exactly 460 mL of solution, what is the molar concentration of nitrate ion? M of Fe(NO3)3=241.86 g/mole
If 1.25 g Fe(NO3)3 is dissolved in enough water to make exactly 397 mL of solution, what is the molar concentration of nitrate ion?
Calculate the vapor pressure of a solution made by dissolving 94.5 g of urea (molar mass= 60.06 g/mol) in 214.5 mL of water at 35°C (Hint: The vapor pressure of pure water at 35°C is given in the table below. Assume the density of the solution is 1.00 g/mL.) What is the magnitude of vapor-pressure lowering? mmHg
a. A 10 ml calibration solution is made by mixing 5 mL of 0.200 M Fe(NO3)3, 1.50 mL of 2.00X10-3 M KNCS, 1 mL of 0.100 M nitric acid and 2.50 mL H20. What is the final concentration of only the NCS-ion? b. If 1.00 ml of this solution is then diluted to a final volume of 25.00 ml with DI water. What is the new concentration of NCS?
Determine the molality of a solution made by dissolving 0.239 moles of glucose in 546 mL of water. Assume the density of water is 1.00 g/mL. m glucose
A solution is made by dissolving 14 g of silver nitrate, AgNO3, in enough water to make exactly 250 mL of solution. Calculate the concentration (molarity) of AgNO3 in mol/L (M)
3. A solution is prepared by dissolving 12.5 g of glucose (CHarO%) in 100.0 g of water. a. What is the concentration of that solution in percent glucose by mass? b. What is the concentration of that solution in mola lity (m)? c. You measured the density of the final solution to be 1.06 g/m L. What is the concentration of the solution in molarity (M)? 4. Calculate the molarity of a 50% sulfuric acid solution by mass. The density...