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4.0 g of NaOH and 4.9 g of H2SO4 are dissolved in water and volume is made up to 250 mL. The pH of this solution is :- (1)7.0(2)1.0(3)2.0(4)12.0 Correct Answer: 1?
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4.0 g of NaOH and 4.9 g of H2SO4 are dissolved in water and volume is ...
It's a case of neutralisation of a SA with a SB.. in this case the pH is always 7...here data is given only to confuse you
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4.0 g of NaOH and 4.9 g of H2SO4 are dissolved in water and volume is ...
Calculation of moles of NaOH and H2SO4:
Moles of NaOH = 4.0 g / 40 g/mol = 0.1 mol
Moles of H2SO4 = 4.9 g / 98 g/mol = 0.05 mol
Determine the limiting reactant:
Since NaOH has higher moles than H2SO4, H2SO4 is the limiting reactant.
Calculating the concentration of H2SO4:
Concentration of H2SO4 = moles / volume
= 0.05 mol / 0.25 L
= 0.2 M
Calculating the pH of the solution:
H2SO4 is a strong acid and completely dissociates in water to give H+ ions and HSO4- ions.
H2SO4 → 2H+ + SO4-2
The H+ ions from H2SO4 as well as the OH- ions from NaOH will react to form water.
H+ + OH- → H2O
Therefore, the remaining H+ ions will determine the pH of the solution.
[H+] = 2 x [H2SO4]
= 2 x 0.2 M
= 0.4 M
pH = -log[H+]
= -log(0.4)
= 0.4
Since pH is negative logarithm of hydrogen ion concentration, the pH of the solution is 0.4 which is closest to answer option 2 (1.0). Therefore, the correct answer is option 2.
Moles of NaOH = 4.0 g / 40 g/mol = 0.1 mol
Moles of H2SO4 = 4.9 g / 98 g/mol = 0.05 mol
Determine the limiting reactant:
Since NaOH has higher moles than H2SO4, H2SO4 is the limiting reactant.
Calculating the concentration of H2SO4:
Concentration of H2SO4 = moles / volume
= 0.05 mol / 0.25 L
= 0.2 M
Calculating the pH of the solution:
H2SO4 is a strong acid and completely dissociates in water to give H+ ions and HSO4- ions.
H2SO4 → 2H+ + SO4-2
The H+ ions from H2SO4 as well as the OH- ions from NaOH will react to form water.
H+ + OH- → H2O
Therefore, the remaining H+ ions will determine the pH of the solution.
[H+] = 2 x [H2SO4]
= 2 x 0.2 M
= 0.4 M
pH = -log[H+]
= -log(0.4)
= 0.4
Since pH is negative logarithm of hydrogen ion concentration, the pH of the solution is 0.4 which is closest to answer option 2 (1.0). Therefore, the correct answer is option 2.
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4.0 g of NaOH and 4.9 g of H2SO4 are dissolved in water and volume is made up to 250 mL. The pH of this solution is :- (1)7.0(2)1.0(3)2.0(4)12.0 Correct Answer: 1?
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4.0 g of NaOH and 4.9 g of H2SO4 are dissolved in water and volume is made up to 250 mL. The pH of this solution is :- (1)7.0(2)1.0(3)2.0(4)12.0 Correct Answer: 1? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about 4.0 g of NaOH and 4.9 g of H2SO4 are dissolved in water and volume is made up to 250 mL. The pH of this solution is :- (1)7.0(2)1.0(3)2.0(4)12.0 Correct Answer: 1? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 4.0 g of NaOH and 4.9 g of H2SO4 are dissolved in water and volume is made up to 250 mL. The pH of this solution is :- (1)7.0(2)1.0(3)2.0(4)12.0 Correct Answer: 1?.
4.0 g of NaOH and 4.9 g of H2SO4 are dissolved in water and volume is made up to 250 mL. The pH of this solution is :- (1)7.0(2)1.0(3)2.0(4)12.0 Correct Answer: 1? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about 4.0 g of NaOH and 4.9 g of H2SO4 are dissolved in water and volume is made up to 250 mL. The pH of this solution is :- (1)7.0(2)1.0(3)2.0(4)12.0 Correct Answer: 1? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 4.0 g of NaOH and 4.9 g of H2SO4 are dissolved in water and volume is made up to 250 mL. The pH of this solution is :- (1)7.0(2)1.0(3)2.0(4)12.0 Correct Answer: 1?.
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