Answer:
Molar concentration of the Fe³⁺ in the unknown solution is 8.01x10⁻⁵M.
Explanation:
When you make a calibration curve in a spectrophotographic analysis you are applying the Lambert-Beer law that states the concentration of a compound is directely proportional to its absorbance:
A = E*l*C
<em>Where A is absorbance, E is molar absorption coefficient, l is optical path length and C is molar concentration</em>
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Using the equation of the line you obtain:
y = 4541.6X + 0.0461
<em>Where Y is absorbance and X is concentration -We will assume concentration is given in molarity-</em>
As absorbance of the unknown is 0.410:
0.410 = 4541.6X + 0.0461
X = 8.01x10⁻⁵M
<h3>Molar concentration of the Fe³⁺ in the unknown solution is 8.01x10⁻⁵M.</h3>
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A: The Equator To The Poles
The answer is 2.135 mol/Kg
Given that molarity is 2M, that is, 2 moles in 1 liter of solution.
Density of solution is 1.127 g/ml
Volume of solution is 1L or 1000 ml
mass of solution (m) = density × volume
m₁ = density × volume = 1.127 × 1000 = 1127 g
mass of solute, m₂ = number of moles × molar mass
m₂ = 2 × 95.211
m₂ = 190.422 g
mass of solvent = m₁ - m₂
= 1127 - 190.422
= 936.578 g
= 0.9366 Kg
molality = number of moles of solute / mass of solvent (in kg)
= 2 / 0.9366
= 2.135 mol/Kg
Hydrogen bonding is a type of intermolecular forces of attraction in which hydrogen atom is bonded to one of the most electronegative atoms. This gives a partial positive charge to hydrogen atom and a partial negative charge to the electronegative atom involved in the bonding. The electronegative atoms that can form hydrogen bonding are fluorine (F), nitrogen (N), and oxygen (O).
Therefore the correct option is,
A) NH3
One mole contains 6.02×10²³
If x mole contains 3.131×10²⁴
x = 3.131×10²⁴
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6.02×10²³
x = 0.52×10²⁴¯²³
x = 0.52×10¹
x = 5.2moles....
Hope this helped...?
