If 2.0 mL of concentrated H2SO4 is diluted with distilled water to 250 mL in a volumetric flask, what is the resulting concentration in units of molarity and normality? What is the volume of the solution in (5) that should be diluted with distilled water to make a 0.025 N solution of sulfuric acid?

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dfrincon99 dfrincon99 · Answer 1 · 2019-10-14T03:37:34+02:00

Answer:

[tex]8*10^{-3} M[/tex]

[tex]1.6*10^{-2} N[/tex]

160 ml of water are needed to dilute the 2ml of [tex]H_{2} SO_{4}[/tex] to 0.025N

Explanation:

concentrated [tex]H_{2} SO_{4}[/tex] = 98% w/v = 1 M

2ml of concentrated [tex]H_{2} SO_{4}[/tex] have:

1M*0.002L = [tex]2*10^{-3} Moles[/tex]

When diluted to 250ml, the concentration becomes:

M=moles solute/volumen solution

[tex]\frac{2*10^{-3} Moles}{0.250L} = 8*10^{-3} M[/tex]

N=(moles solute*#eq) /(volumen solution)

[tex]\frac{2*10^{-3} Moles*2eq}{0.250L} = 1.6*10^{-2} N[/tex]

for the 0.025N solution

we take the same moles of [tex]H_{2} SO_{4}[/tex] = [tex]2*10^{-3} Moles[/tex]

then we find the volume:

N=(moles solute*#eq) /(volumen solution)

(volumen solution)=(moles solute*#eq) /N

[tex]\frac{2*10^{-3} Moles*2eq}{2.5*10^{-2} N} = 0.160L =160ml[/tex]