The mass of dextrose = (1/25)*248 = 9.92 g
The molar mass of dextrose = 180.2 g/mol
No. of moles of dextrose = mass of dextrose/molar mass of dextrose
= 9.92 g/(180.2 g/mol)
= 0.05505 mol
Therefore, the no. of moles of dextrose = 0.05505 mol
an aqueous solution of fructose( mw180.2) contains 1 in 25 of dextrose. if the density of...
A aqueous dextrose solution having a density of 1.04g/mL freezes at -1.15 C. Find the osmotic pressure of this solution at 25 degree C.
You make 1L of an aqueous solution that contains 35g of fructose (C6H12O6). A. What is the molarity of fructose in this solution? B. How many litres of water would you have to add to this solution to reduce the molarity you calculated in Part A by a factor of two?
A 5% dextrose IV fluid contains 35 mEq of K^+ per liter of solution. If a patient receives 260 mL of the IV solution, how many moles of K^+ were deliver Express your answer using two significant figures. n_K^+ = mol
An aqueous solution at 25 ∘C is 12.7 % HNO3 by mass and has a density of 1.059 g/mL. What is the pH of the solution? Use the Henderson-Hasselbalch equation to determine the moles of H+added to the solution, resulting in a pH=7.24
How many milliliters of a 12.5% dextrose solution contain 25 grams of dextrose? O A. 1,000 mL O B. 200 ml O c. 10,000 ml OD. 1562.5 ml
An aqueous solution has a density of 1.68 g/mL and contains 80.9% sugar by mass. How many kilograms of sugar are contained in 1.80 gallons of this solution? (1 gallon = 3.785 L) 5.09 kg 3.70 kg 9.26 kg 6.02 kg 2.45 kg
An aqueous solution of orthophosphoric acid, H3PO4, has a measured density of 1.2089 g/mL and is 5.257 molal. How many moles of H3PO4 are there in one liter of this solution? 1) 0.4261 moles O2) 4.194 moles O 3) 4.349 moles 4) 5.152 moles 5) 6.355 moles
1. An aqueous solution contains 0.395 M hydrocyanic acid. Calculate the pH of the solution after the addition of 5.99×10-2 moles of sodium hydroxide to 255 mL of this solution. (Assume that the volume does not change upon adding sodium hydroxide) pH = 2. An aqueous solution contains 0.302 M acetic acid. Calculate the pH of the solution after the addition of 2.56×10-2 moles of potassium hydroxide to 125 mL of this solution. (Assume that the volume does not change...
1. An aqueous solution contains 0.395 M hydrocyanic acid. Calculate the pH of the solution after the addition of 5.99×10-2 moles of sodium hydroxide to 255 mL of this solution. (Assume that the volume does not change upon adding sodium hydroxide) pH = 2. An aqueous solution contains 0.302 M acetic acid. Calculate the pH of the solution after the addition of 2.56×10-2 moles of potassium hydroxide to 125 mL of this solution. (Assume that the volume does not change...
You measure out 4.9 mL of an aqueous ethylenediamine (H2NCH2CH2NH2) solution. This aqueous solution has a density of 0.950 g/mL and is 25.0% by mass ethylenediamine. How many moles of ethylenediamine are in the 4.9 mL?