This reaction asks for dissolving 0.85 g of kl to 1.2 mL of water. If the...
13 A solution is prepared by dissolving 10.98 g of MgCl2 in 646 mL of water. The total mass of the solution is 656.98 g. and the total volume is 651 mL. a What is the mass-mass percent concentration of MgCl2 in the solution? Show your work. b What is the mass-volume percent concentration of MgCl2 in the solution? Show your work. c What is the molarity of the MgCl2 in the solution? Show your work.
what is the molarity of a solution made by dissolving 673.9 g of KI in 741 mL of water? (MM KI = 166.00 g/mol)
Dissolving 5.57 g of CaCl2 in enough water to make 288 mL of solution causes the temperature of the solution to increase by 3.77 oC. Assume the specific heat of the solution and density of the solution are the same as water′s (about 4.18 J/goC and 1.00 g/cm3, respectively) Calculate ΔH per mole of CaCl2 (in kJ) for the reaction under the above conditions. Hint given in feedback Aside, the ΔH per mole for dilution depends on the process. For...
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...
A solution is prepared by dissolving 20.2 mL of methanol (CH3OH) in 100.0 mL of water at 25 ∘C. The final volume of the solution is 118 mL. The densities of methanol and water at this temperature are 0.782 g/mL and 1.00 g/mL, respectively. For this solution, calculate mole percent M=4.18 m=4.93 percent by mass= 13.6% mole fraction= 8.15*10^-2
A solution is prepared by dissolving 29.2 g of glucose (C6H12O6) in 355 g of water. The final volume of the solution is 376 mL . For this solution, calculate each of the following. A.) molarity B.) moality C. ) percent by mass D.) mole fraction E.) mole percent
A 2.550×10−2M solution of NaCl in water is at 20.0∘C. The sample was created by dissolving a sample of NaCl in water and then bringing the volume up to 1.000 L. It was determined that the volume of water needed to do this was 999.3 mL . The density of water at 20.0∘C is 0.9982 g/mL. A) Calculate the molality of the salt solution. B) Calculate the mole fraction of salt in this solution. C) Calculate the concentration of the...
A solution is prepared by dissolving 28.4 g of glucose (C6H12O6) in 355 g of water. The final volume of the solution is 384 mL . Calculate the solution concentration in each unit. PART A mole fraction x= PART B mole percent = %
QUESTION 5 A solution is prepared by dissolving 5.0 g NaCl in 45.0 mL of water. The molar mass of NaCl is 58.5 g/mol and the density of water is 1.0 g/mL. What is the percent NaCl in the solution? O a. 5.0% b. 11% O C. 10% O d.58.5% Oe. None of these
A solution is made by dissolving 13.2 g of HCl in 774.7 mL of water. Calculate the pH of the solution. Assume that the volume of the solution not change with the addition of HCl.