1. Glucose (C6H12O6, M= 180.16 g/mol) solutions are commercially available. A concentrated sample of an aqueous glucose solution has a density of 1.25 g/mL and contains 55.0 % glucose by mass at 20 °C
a) What is the molarity of this glucose solution?
b) What is the molality of this solution?
c) What is the mole fraction of glucose in this solution?
please like the answer and comment thank you?
1. Glucose (C6H12O6, M= 180.16 g/mol) solutions are commercially available. A concentrated sample of an aqueous...
Commercially available aqueous solutions of glucose (C6H12O6) are typically labeled as having a concentration of 5%(w/v). This means that a 100 mL sample of the solution contains 5 g of C6H12O6. a. How many moles of glucose are in a 4.16 mL sample of a 5%(w/v) solution? Hint: first calculate the mass of glucose in the 4.16 mL sample given that a 100 mL sample contains 5 g of glucose; then convert mass to grams. NG 2 b. If you...
An aqueous solution of glucose is 17.5% C6H12O6 by mass and has a density of 1.10 g/mL. What is the molarity and molality of the solution? What is the mole fraction of glucose?
A solution is prepared by dissolving 28.4 g of glucose (C6H12O6) in 1.00 x 102 mL of acetone (C3H6O) at 25 °C. The final volume of the solution is 118 mL. The density of glucose and acetone are 1.54 g/mL and 0.785 g/mL, respectively. Calculate the following quantities: a.) Molarity b.) Molality c.) Mass Percent d.) Mole Fraction
What are the molarity, molality, X of a 6.56% by mass glucose (C6H12O6, MM=180g/mol) solution? The density of the solution is 1.03g/mL.
7. What is the mole fraction of urea, CH4N2O, in an aqueous solution that is 46% urea by mass? 8. What volume of a 0.850 M solution of CaCl2 contains 1.28 g of solute? 9. The volume of a 27.0% (by mass) solution is 162.9 mL. The density of the solution is 1.128 g/mL. What is the mass of solute in this solution? 10. Concentrated sodium hydroxide is 19.4 M and has a density of 1.54 g/mL. What is the...
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
Glucose solutions used for intravenous medical applications are typically 5.00 % (m/m) Glucose dissolved in water. What is the molarity associated with a typical 5.00 % Glucose solution. Molar Mass (Glucose) = 180.16 g/mol; Density of normal glucose solution = 1.01 g/mL 0.280 M b) 0.364 M c) 2.75 M d) 3.57 M e) 9.09 M
Calculate the molarity of the two solutions. The first solution contains 0.550 mol of NaOH in 2.95 L of solution. molarity: The second solution contains 19.1 g of NaCl in 627 mL of solution. molarity: Calculate the molality of a solution formed by adding 7.00 g NH,Cl to 14.0 g of water. molality: m NH C1 What is the mole fraction of solute in a 3.69 m aqueous solution? Xsolute = 0.06 An aqueous sodium acetate, NaC,H,O, , solution is...
1a. An aqueous solution has a Molarity of 1.632 M. The density of the solution is (1.150x10^0) g/mL and the solute has a molar mass of (1.33x10^2) g/mol. What is the molality of this solution? 1b. An aqueous solution has a mass percent of solute of 18.4%. The density of the solution is (1.400x10^0) g/mL and the solute has a molar mass of (1.77x10^2) g/mol. What is the molality of this solution? 1c. An aqueous solution has a molality of...
an aqueous solution of sucrose (C6H12O6 molar mass = 180.16g/mol) is 3.928m and has a density of 1.240 g/ml. What is the molarity of the solution (use dimensional analysis)