FOR MORE PRACTICE 13.5 solution is 1.03 g/ml.) what is the mo ality ofa 10.5% by...
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what is the mass of 5. The mass ofa 14.4% (by mass) solution is 892 g. The density ofthe solution is 1.264 g mL the water in this solution? a. 8 g b.0g c. 10.4g d. 2 g e. 9.65 g
2013x10 39 : 2013kg Mass percent A glucose IV solution is 5.0 % 5.0 g of glucose 100 g solution Question 6. What is the mass of glucose (in kg) present in a 5.0 % glucose solution? (5.00) Question 7. A soft drink contains 11.5% sucrose (C12H2201 )by mass. What volume of the soft drink solutions in milliliters contains 85.2 g of sucrose? (Assume a density 1.04 g/mL.) [7.12E2 ml solution] Question 8. A glucose solution is 3.25% glucose by...
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...
What is the molarity of a 14.5% by mass glucose (C6H12O6) solution? (The density of the solution is 1.03 g/mL.)
Calculate the osmotic pressure at 298 K of the solutions that contain: 10.5 g of MgCl_2 in 150 mL of solution. 0.650 M NaCI solution. 7.5 % glucose (non-electrolyte) by mass in water. Density of solution is 1.01 g mL^-1
1. in run 1, you mix 8.1 mL of the 43 g/L MO solution (MO molar mass is 327.33 g/mol), 2.89 mL of the 0.040 M SnCl22 in 2 M HCl solution, 5.46 mL of 2.0M HCl solution, and 3.47 mL of 2.0M NaCl solution. What is the [MO]? a. In run 1, you mix 8.1 mL of the 43 g/L MO solution (MO molar mass is 327.33 g/mol), 2.89 mL of the 0.040 M SnCl22 in 2.0 M HCl...
(a) What is the density in units of g/mL ofa liquid with a mass of40.75 μg that occupies a volume of292 x 10-8 L? (b) Determine the mass in kg of 6.3 x 10 nL of the liquid.
8. Which beaker contains more dissolved glucose particles? Solution A Solution B 50.0 mL of 1.25 M glucose solution. 50.0 mL of 25 % (m/m) glucose solution. Molar Mass Glucose - 180.156 g/mol Density of 25% solution = 1.56 g/mL
The density of mercury is 13.5 g/mL and the density of water is 1.00 g/mL. If a mercury barometer reads 787 mmHg, what is the barometric pressure in centimeters of water (cmH2O)?
A calorimeter contains 26.0 mL of water at 13.5 ∘C . When 2.50 g of X (a substance with a molar mass of 51.0 g/mol ) is added, it dissolves via the reaction X(s)+H2O(l)→X(aq) and the temperature of the solution increases to 30.0 ∘C . Calculate the enthalpy change, ΔH, for this reaction per mole of X. Assume that the specific heat of the resulting solution is equal to that of water [4.18 J/(g⋅∘C)], that density of water is 1.00...