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The molarity of orthophosphoric acid having purity of 70% by weight and specific gravity 1.54 would be
- a)11M
- b)22 M
- c)33 M
- d)44 M
Correct answer is option 'A'. Can you explain this answer?
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The molarity of orthophosphoric acid having purity of 70% by weight an...
70% by weight 70gm H3PO4 → 100gm solution / sample
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The molarity of orthophosphoric acid having purity of 70% by weight an...
Calculation of Molarity of Orthophosphoric Acid:
Given Data:
Purity of Orthophosphoric Acid = 70% by weight
Specific Gravity of Orthophosphoric Acid = 1.54
Step 1: Calculation of Mass of Pure Orthophosphoric Acid
Let us assume the total mass of Orthophosphoric Acid to be 100 g.
Therefore, the mass of pure Orthophosphoric Acid (H3PO4) = 70 g (given purity is 70%)
Step 2: Calculation of Volume of Orthophosphoric Acid
As we know, Density = Mass/Volume
Therefore, Volume of Orthophosphoric Acid = Mass/Density
= 70/1.54
= 45.45 mL
Step 3: Calculation of Molarity of Orthophosphoric Acid
Molarity = Number of moles of solute/Volume of solution (in liters)
As the molecular weight of Orthophosphoric Acid is 98 g/mol, the number of moles of solute can be calculated as follows:
Number of moles of solute = Mass of solute/Molecular weight of solute
= 70/98
= 0.714 mol
Therefore, Molarity of Orthophosphoric Acid = 0.714/0.04545
= 15.69 M
However, the above calculated molarity is for pure Orthophosphoric Acid. But as the given Orthophosphoric Acid is only 70% pure, the actual molarity of the solution would be 70% of 15.69 M.
Actual Molarity of Orthophosphoric Acid = 0.7 × 15.69
= 11 M
Hence, the correct option is (a) 11 M.
Given Data:
Purity of Orthophosphoric Acid = 70% by weight
Specific Gravity of Orthophosphoric Acid = 1.54
Step 1: Calculation of Mass of Pure Orthophosphoric Acid
Let us assume the total mass of Orthophosphoric Acid to be 100 g.
Therefore, the mass of pure Orthophosphoric Acid (H3PO4) = 70 g (given purity is 70%)
Step 2: Calculation of Volume of Orthophosphoric Acid
As we know, Density = Mass/Volume
Therefore, Volume of Orthophosphoric Acid = Mass/Density
= 70/1.54
= 45.45 mL
Step 3: Calculation of Molarity of Orthophosphoric Acid
Molarity = Number of moles of solute/Volume of solution (in liters)
As the molecular weight of Orthophosphoric Acid is 98 g/mol, the number of moles of solute can be calculated as follows:
Number of moles of solute = Mass of solute/Molecular weight of solute
= 70/98
= 0.714 mol
Therefore, Molarity of Orthophosphoric Acid = 0.714/0.04545
= 15.69 M
However, the above calculated molarity is for pure Orthophosphoric Acid. But as the given Orthophosphoric Acid is only 70% pure, the actual molarity of the solution would be 70% of 15.69 M.
Actual Molarity of Orthophosphoric Acid = 0.7 × 15.69
= 11 M
Hence, the correct option is (a) 11 M.
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The molarity of orthophosphoric acid having purity of 70% by weight and specific gravity 1.54 would bea)11Mb)22 Mc)33 Md)44 MCorrect answer is option 'A'. Can you explain this answer?
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