LAB 142 Data Table 2: Concentration (Normality) of the Unknown Diprotic Acid Sol

Question

LAB 142 Data Table 2: Concentration (Normality) of the Unknown Diprotic Acid Solution Trial 3 Trial 2 Volume of Unknown ! Solution Pipetted mL)n Pipette Final Buret Reading (mL) 34.9m m/23 Initial Buret Reading (mL) mL r R Volume of Sodium &|Hydroxide Added |-lo (mL) Normality of Sodium week) (eq/L) Normality of Un- known Diprotic Acid Solution (eq/L) Average Normality of Unknown Diprotic Acid Solut From Trials 1, 2, and 3 (eq/L) ii. Answer the following question using the space below. What is normality? If the unknown diprotic acid in this experiment is H2SO4, what is the molarity of the H SO(ag) as determined by you experimentally? WtOS of Sointion Be certain to plot and attach the strong acid-strong base titration curve from Part0.

Explanation / Answer

To get the molarity, this is the equation to use:
M = moles/V

Now, the expression of Normality:
N = n° eq / V

And n° equivalent: n°eq = mass/EW

Finally EW = MW/F
Where F depends on the compound, in the case of acid, is the number of hydrogens so:
EW = MW/n°H

Let's calculate the molecular weight and then, equivalence weight of the H2SO4:
MW = 2*1 + 32 + 4*16 = 98 g/mol
EW = 98 / 2 = 49 g/eq

This means that the relation between one and the other is just by a factor of two.

So if the normality is 0.114 eq/L just multiply by 2 to get the molarity:
M = 0.114 eq/L * 1 mol/2 eq = 0.057 mol/L

Hope this helps

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