To prepare a solution of NaCl, you weight out 2.634 (±0.002) g and dissolve it in...

To prepare a solution of NaCl, you weight out 2.634 (±0.002) g and dissolve it in a volumetric flask whose volume is 100.00 (±0.08)mL. Express the molarity of the solution, along with its uncertainty, with an appropriate number of digits. [Molecular mass of NaCl, 58.443 (±0.001) g/mol].

Expert Solution

Find out the moles of NaCl weighed out = mass of NaCl weighed out/molar mass of NaCl = (2.634 g)/(58.443 g/mol) = 0.0451 mol.

Find out the molarity of the prepared NaCl solution as molarity = moles of NaCl/volume of solution in L = (0.0451 mol)/[(100.00 mL)*(1 L/1000 mL)] = (0.0451 mol)*(1000)/(100.00).(1 L) = 0.451 mol/L = 0.451 M

Next calculate the uncertainty in the measurement.

Uncertainty in mass weighed out = (0.002 g)/(2.634 g)

Uncertainty in molar mass of NaCl = (0.001 g/mol)/(58.443 g/mol)

Uncertainty in volume = (0.08 mL)/(100.00 mL)

Let the uncertainty in measurement of concentration is u(c) where c = 0.451 mol/L is the concentration.

Therefore,

[u(c)/c]² = (0.002/2.634)² + (0.001/58.443)² + (0.08/100.00)² = 1.2168*10^-3

===> [u(c)/c] = √(1.2168*10^-6) = 1.1031*10^-3

===> u(c) = 1.1031*10^-3*c = 1.1031*10^-3*0.451 M = 4.975*10^-4 M

The molar concentration of prepared NaCl is 0.451 0.0004975 M (ans).

queen_honey_blossom answered 11 months ago

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