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1.25 g of a solid dibasic acid is completely neutralized by 25mL of 0.25 molar Ba(OH)2 solution Molecular mass of the acid is a) 100 b)150 c)120 d)200?
Most Upvoted Answer
1.25 g of a solid dibasic acid is completely neutralized by 25mL of 0....
**Given Information:**
- 1.25 g of a solid dibasic acid is completely neutralized by 25 mL of 0.25 molar Ba(OH)2 solution.
**To Find:**
- Molecular mass of the acid.
**Solution:**
**Step 1: Calculate the number of moles of Ba(OH)2:**
Given volume of Ba(OH)2 solution = 25 mL = 0.025 L
Molarity of Ba(OH)2 solution = 0.25 mol/L
Number of moles of Ba(OH)2 = Molarity × Volume
= 0.25 mol/L × 0.025 L
= 0.00625 mol
**Step 2: Calculate the number of moles of the acid:**
From the balanced chemical equation of the neutralization reaction, we know that 1 mole of Ba(OH)2 reacts with 2 moles of the dibasic acid.
Therefore, the number of moles of the dibasic acid = 0.00625 mol × 2
= 0.0125 mol
**Step 3: Calculate the molecular mass of the acid:**
Molecular mass = Mass / Moles
Given mass of the acid = 1.25 g
Number of moles of the acid = 0.0125 mol
Molecular mass of the acid = 1.25 g / 0.0125 mol
= 100 g/mol
**Answer:**
- The molecular mass of the acid is 100 g/mol.
- Therefore, the correct option is (a) 100.
- 1.25 g of a solid dibasic acid is completely neutralized by 25 mL of 0.25 molar Ba(OH)2 solution.
**To Find:**
- Molecular mass of the acid.
**Solution:**
**Step 1: Calculate the number of moles of Ba(OH)2:**
Given volume of Ba(OH)2 solution = 25 mL = 0.025 L
Molarity of Ba(OH)2 solution = 0.25 mol/L
Number of moles of Ba(OH)2 = Molarity × Volume
= 0.25 mol/L × 0.025 L
= 0.00625 mol
**Step 2: Calculate the number of moles of the acid:**
From the balanced chemical equation of the neutralization reaction, we know that 1 mole of Ba(OH)2 reacts with 2 moles of the dibasic acid.
Therefore, the number of moles of the dibasic acid = 0.00625 mol × 2
= 0.0125 mol
**Step 3: Calculate the molecular mass of the acid:**
Molecular mass = Mass / Moles
Given mass of the acid = 1.25 g
Number of moles of the acid = 0.0125 mol
Molecular mass of the acid = 1.25 g / 0.0125 mol
= 100 g/mol
**Answer:**
- The molecular mass of the acid is 100 g/mol.
- Therefore, the correct option is (a) 100.
Community Answer
1.25 g of a solid dibasic acid is completely neutralized by 25mL of 0....
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1.25 g of a solid dibasic acid is completely neutralized by 25mL of 0.25 molar Ba(OH)2 solution Molecular mass of the acid is a) 100 b)150 c)120 d)200?
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1.25 g of a solid dibasic acid is completely neutralized by 25mL of 0.25 molar Ba(OH)2 solution Molecular mass of the acid is a) 100 b)150 c)120 d)200? for Class 11 2024 is part of Class 11 preparation. The Question and answers have been prepared according to the Class 11 exam syllabus. Information about 1.25 g of a solid dibasic acid is completely neutralized by 25mL of 0.25 molar Ba(OH)2 solution Molecular mass of the acid is a) 100 b)150 c)120 d)200? covers all topics & solutions for Class 11 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 1.25 g of a solid dibasic acid is completely neutralized by 25mL of 0.25 molar Ba(OH)2 solution Molecular mass of the acid is a) 100 b)150 c)120 d)200?.
1.25 g of a solid dibasic acid is completely neutralized by 25mL of 0.25 molar Ba(OH)2 solution Molecular mass of the acid is a) 100 b)150 c)120 d)200? for Class 11 2024 is part of Class 11 preparation. The Question and answers have been prepared according to the Class 11 exam syllabus. Information about 1.25 g of a solid dibasic acid is completely neutralized by 25mL of 0.25 molar Ba(OH)2 solution Molecular mass of the acid is a) 100 b)150 c)120 d)200? covers all topics & solutions for Class 11 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 1.25 g of a solid dibasic acid is completely neutralized by 25mL of 0.25 molar Ba(OH)2 solution Molecular mass of the acid is a) 100 b)150 c)120 d)200?.
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