g, follow these steps:

Calculate the amount of urea:

The solution contains 6% urea by mass. Thus, the mass of urea is:

$ \text{Urea} = 1000 \, \text{g} \times \frac{6}{100} = 60 \, \text{g} $

The molar mass of urea (CH₄N₂O) is calculated using the atomic masses, which are:

Carbon (C): 12 u

Nitrogen (N): 14 u

Oxygen (O): 16 u

Hydrogen (H): 1 u

Therefore, the molar mass of urea is:

$ \text{Molar mass of urea} = 12 + (4 \times 1) + (2 \times 14) + 16 = 60 \, \text{g/mol} $

Convert the mass of urea to moles:

$ \text{Moles of urea} = \frac{60 \, \text{g}}{60 \, \text{g/mol}} = 1 \, \text{mol} $

Calculate the volume of water:

The remaining mass of the solution is water:

$ \text{Water} = 1000 \, \text{g} - 60 \, \text{g} = 940 \, \text{g} $

Using the density of water (1 g/mL), convert this mass to volume:

$ \text{Volume of water} = \frac{940 \, \text{g}}{1 \, \text{g/mL}} = 940 \, \text{mL} = 0.94 \, \text{L} $

Calculate the concentration of the urea solution:

The concentration in molarity ($ \text{mol/L} $) is given by:

$ \text{Concentration} = \frac{\text{Moles of urea}}{\text{Volume of solution in liters}} = \frac{1 \, \text{mol}}{0.94 \, \text{L}} = 1.0638 \, \text{M} $

Rounding to three significant figures gives:

$ \text{Concentration} \approx 1.064 \, \text{mol/L} $

Therefore, the concentration of the urea solution is approximately $1.064 \, \text{mol/L}$.

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