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Mole fraction of nh3 in the solution is 11.33%.
What is mole?
The International System of Units uses the mole (symbol: mol) as the unit of substance amount (SI). How so many elementary entities of a particular substance are present in an object or sample is determined by the quantity of that substance. There are precisely 6.02214076×10^23 elementary entities in a mole.
NH3(g) + H2O(l) = NH4OH (aq)
The molar mass of NH3 is 17.031 g/mol.
The NH3:NH4OH mole ratio is 1: 1.
Mol of NH3 = 15 g/(17.031 g/mol) = 0.88 mol, which produces (1/1) x 0.88 mol of NH4OH = 0.88 mol of NH4OH/250 g of water.
The mass of the solution is calculated as 15g + 250 g = 265 g.
Given that the density of NH4OH is 0.974 g/mL, the resulting solution contains 0.88 mol of NH4OH/265 g: 0.974 g/mL or 0.88 mol/272.0739mL.
Then, mol of NH4OH in 100mL solution = (100mL/272.0739mL) x 0.88 mol = 0.3234 mol of NH4OH/100mL solution...
……. [A]
The molar mass of NH4OH is 35.04 g/mol.
As a result, the mass of NH4OH = 0.3234 mol x 35.04 g/mol = 11.33 g of NH4OH/100mL or 11.33% (m/v).
As stated in [A], one mol of NH4OH equals 0.3234mol/100mL solution or (1000mL/100mL) x 0.3234 mol equals 3.234 mol NH4OH/L or 3.234 M.
Because NH4OH is a monoprotic base, molarity equals normality, so the resulting solution's normality = 3.234 N rounded up to 3.23 N.
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