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An organic acid containing carbon, oxygen and hydrogen only has molar mass of 132 g. 6.6 g of this acid require 80 mL 1.25 M NaOH for complete neutralisation. How many carboxylic groups are present in one molecule of this acid?
- a)1
- b)2
- c)3
- d)4
Correct answer is option 'B'. Can you explain this answer?
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Verified Answer
An organic acid containing carbon, oxygen and hydrogen only has molar ...
Let us consider organic acid as ‘A’.
Moles of A = mass of A/Molar mass = 6.6/132 = 0.05
Molarity of NaOH = 1.25M
And volume of NaOH = 80 mL
Therefore, moles of NaOH = molarity × Volume
= 1.25×80×10-3 = 0.1 moles.
SO, 0.05 moles of A requires 0.1 moles of NaOH
1 mole of acid requires x moles of NaOH
x = 0.1/0.05×1 = 2
So for neutralisation of 1 mole of A, we need 2 moles of NaOH. Therefore given acid is dibasic and contains 2 -COOH groups.
Moles of A = mass of A/Molar mass = 6.6/132 = 0.05
Molarity of NaOH = 1.25M
And volume of NaOH = 80 mL
Therefore, moles of NaOH = molarity × Volume
= 1.25×80×10-3 = 0.1 moles.
SO, 0.05 moles of A requires 0.1 moles of NaOH
1 mole of acid requires x moles of NaOH
x = 0.1/0.05×1 = 2
So for neutralisation of 1 mole of A, we need 2 moles of NaOH. Therefore given acid is dibasic and contains 2 -COOH groups.
Most Upvoted Answer
An organic acid containing carbon, oxygen and hydrogen only has molar ...
Given: Molar mass of organic acid = 132 g/mol
Mass of acid required for neutralisation = 6.6 g
Volume of NaOH used for neutralisation = 80 mL
Concentration of NaOH = 1.25 M
To find: Number of carboxylic groups present in one molecule of acid
Step 1: Calculate the number of moles of NaOH used for neutralisation
Moles of NaOH = Concentration of NaOH x Volume of NaOH used = 1.25 x 0.08 = 0.1 mol
Step 2: Use the balanced chemical equation to find the number of moles of acid used for neutralisation
NaOH + HX → NaX + H2O
1 mol of NaOH reacts with 1 mol of acid (HX)
0.1 mol of NaOH will react with 0.1 mol of acid
Step 3: Calculate the molar mass of the acid
Molar mass = Mass of acid used / Number of moles of acid used
132 = 6.6 / 0.1
Number of moles of acid used = 0.05 mol
Step 4: Find the molecular formula of the acid
Molecular formula mass = Molar mass / Number of moles
Molecular formula mass = 132 / 0.05 = 264
Possible molecular formulas are C6H5COOH, C7H6O2, C8H7COOH, C9H8O2
Out of these, only C7H6O2 has 2 carboxylic groups (COOH)
Therefore, the answer is option (B) 2 carboxylic groups.
Mass of acid required for neutralisation = 6.6 g
Volume of NaOH used for neutralisation = 80 mL
Concentration of NaOH = 1.25 M
To find: Number of carboxylic groups present in one molecule of acid
Step 1: Calculate the number of moles of NaOH used for neutralisation
Moles of NaOH = Concentration of NaOH x Volume of NaOH used = 1.25 x 0.08 = 0.1 mol
Step 2: Use the balanced chemical equation to find the number of moles of acid used for neutralisation
NaOH + HX → NaX + H2O
1 mol of NaOH reacts with 1 mol of acid (HX)
0.1 mol of NaOH will react with 0.1 mol of acid
Step 3: Calculate the molar mass of the acid
Molar mass = Mass of acid used / Number of moles of acid used
132 = 6.6 / 0.1
Number of moles of acid used = 0.05 mol
Step 4: Find the molecular formula of the acid
Molecular formula mass = Molar mass / Number of moles
Molecular formula mass = 132 / 0.05 = 264
Possible molecular formulas are C6H5COOH, C7H6O2, C8H7COOH, C9H8O2
Out of these, only C7H6O2 has 2 carboxylic groups (COOH)
Therefore, the answer is option (B) 2 carboxylic groups.
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An organic acid containing carbon, oxygen and hydrogen only has molar mass of 132 g. 6.6 g of this acid require 80 mL 1.25 M NaOH for complete neutralisation. How many carboxylic groups are present in one molecule of this acid?a)1b)2c)3d)4Correct answer is option 'B'. Can you explain this answer?
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