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Chemistry
8 October, 14:07
What is the density of 53.4 wt aqueous naoh?
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Coleman Winters
8 October, 14:33
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Missing question: what is the density of 53.4 wt% aqueous NaOH if 16.7 mL of the solution diluted to 2.00L gives 0.169 M NaOH?
Answer is: density is 1.52 g/mL.
c₁ (NaOH) = ?; molarity of concentrated sodium hydroxide.
V₁ (NaOH) = 16.7 mL; volume of concentrated sodium hydroxide.
c₂ (NaOH) = 0.169 M; molarity of diluted sodium hydroxide.
V₂ (NaOH) = 2.00 L · 1000 mL/L = 2000 mL; volume of diluted sodium hydroxide.
Use equation: c₁V₁ = c₂V₂.
c₁ = c₂V₂ / V₁.
c₁ = 0.169 M · 2000 mL / 16.7 mL.
c₁ (NaOH) = 20.23 M.
m (NaOH) = 20.23 mol · 40 g/ml.
m (NaOH) = 809.53 g.
The mass fraction is the ratio of one substance (in this example sodium hydroxide) with mass to the mass of the total mixture (solution).
Make proportion: m (NaOH) : m (solution) = 53.4 g : 100 g.
m (solution) = 1516 g in one liter of solution.
d (solution) = 1516 g/L = 1.52 g/mL.
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