l 2. Determine the mole fraction of zinc(II) sulfite in a 4.22 M aqueous solution of...

l

2. Determine the mole fraction of zinc(II) sulfite in a 4.22 M aqueous solution of zinc(II) sulfite. The density of the solution is 1.01 g mL^-1.
answer is not 0.0699

Expert Solution

4.22M aqueous solution of zinc(II) sulfite

4.22mole/L aqueous solution of zinc(II) sulfite

1liter of solution contains 4.22moles of zinc(II) sulfite

1000ml of solution contains 4.22moles of zinc(II) sulfite

mass of solution = volume * density

= 1000*1.01 = 1010g

mass of solute (zinc(II) sulfite) = no of moles* gram molar mass

= 4.22*145.22 = 612.82g

mass of solvent (water) = 1010-612.82 = 397.18g

no of moles of H2O = 397.18/18 = 22.065moles

mole fraction of zinc(II) sulfite = no of moleszinc(II) sulfite/zinc(II) sulfite+ no of moles of H2O

= 4.22/4.22+22.065

= 4.22/26.285 = 0.1605 >>>> answer

queen_honey_blossom answered 8 months ago

The mole fraction of an aqueous solution of magnesium sulfite is 0.29. Calculate the molarity (in...

The mole fraction of an aqueous solution of magnesium sulfite is 0.29. Calculate the molarity (in mol/L) of the magnesium sulfite solution, if the density of the solution is 1.38 g mL-1. Determine the mole fraction of magnesium bromide in a 5.51 M aqueous solution of magnesium bromide. The density of the solution is 1.17 g mL-1.

If you have a 2.14 m aqueous solution of NaHCO3, what is the mole fraction of...

If you have a 2.14 m aqueous solution of NaHCO3, what is the mole fraction of NaHCO3?

The molality of an aqueous sodium nitrate solution is 2.81 m. What is the mole fraction...

The molality of an aqueous sodium nitrate solution is 2.81 m. What is the mole fraction of NaNO3? The molar mass of NaNO3 is 85.00 g/mol; the molar mass of water is 18.02 g/mol. 0.0506 0.239 0.00281 0.193 0.0482

The mole fraction of potassium phosphate, K3PO4, in an aqueous solution is 8.11x10-2

The mole fraction of potassium phosphate, K3PO4, in an aqueous solution is 8.11x10-2 The percent by mass of potassium phosphate in the solution is _______ %. The mole fraction of ammonium sulfide, (NH4)2S, in an aqueous solution is 3.42x10-2 The percent by mass of ammonium sulfide in the solution is _______ %.

The mole fraction of glucose in an aqueous solution is 0.015. The density of the solution...

The mole fraction of glucose in an aqueous solution is 0.015. The density of the solution is 1.05 g/mL. Calculate the molarity and molality of the solution.

A) Calculate the concentration of zinc (II) ions in a solution containing 0.20 M hexaammine zinc(II)...

A) Calculate the concentration of zinc (II) ions in a solution containing 0.20 M hexaammine zinc(II) ion and 0.0116 M ammonia at equilibrium. The Kf of [Zn(NH3)4]^2+ is 2.8*10^9. B) Calculate the solubility of lead (II) sulfate in a 0.0034 M solution of sodium sulfate. The Ksp for lead(II) sulfate is 1.83*10^-8.

You are asked to prepare an aqueous solution of ethylene glycol (HOCH2CH2OH) with a mole fraction...

You are asked to prepare an aqueous solution of ethylene glycol (HOCH2CH2OH) with a mole fraction of 0.192. a) If you use 645 g of water, what mass (in g) of ethylene glycol should you use? b) What is the molality of the resulting solution?

An aqueous solution of C6H12O6 has a mole fraction of 0.0445 for C6H12O6 in water. Calculate...

An aqueous solution of C6H12O6 has a mole fraction of 0.0445 for C6H12O6 in water. Calculate the Molarity of the solution. The density of the solution is 1.09 g/mL

Upon mixing 0.050 L of 0.010 M aqueous solution of mercury (II) nitrate with 0.020 L...

Upon mixing 0.050 L of 0.010 M aqueous solution of mercury (II) nitrate with 0.020 L of 0.10 M aqueous solution of sodium sulfide, a precipitate of mercury (II) sulfide forms. A) Write a balanced molecular equation of this reaction. B) Determine the theoretical yield of mercury (II) sulfide formed from the limiting reagent. C) Calculate the % yield of product when 0.082 grams of mercury (II) sulfide is isolated.

In a 59.0-g aqueous solution of methanol, CH4O, the mole fraction of methanol is 0.120. What...

In a 59.0-g aqueous solution of methanol, CH4O, the mole fraction of methanol is 0.120. What is the mass of each component? Mass of (g) CH4O? Mass (g) of H2O?

Question