Class 11 Exam  >  Class 11 Questions  >  25.3 g of sodium carbonate, Na2CO3 is dissolv... Start Learning for Free
25.3 g of sodium carbonate, Na2CO3 is dissolved in enough water to make 250 mL of solution. If sodium carbonate dissociates completely, molar concentration of sodium ions, Na+ and carbonate ions, are respectively. (At. mass of carbon = 40) 
  • a)
    0.477 M and 0.477 M
  • b)
    0.955 M and 1.910 M
  • c)
    1.910 M and 0.955 M
  • d)
    1.90 M and 1.910 M
Correct answer is option 'C'. Can you explain this answer?
Verified Answer
25.3 g of sodium carbonate, Na2CO3 is dissolved in enough water to mak...

= 2.53/106   2.59 × 10-2  5.9 × 10-2
0.238 × 0.25          = 1.18 × 10-3

250 ml - 0.238

= 0.955

0.955  0.955 
View all questions of this test
Most Upvoted Answer
25.3 g of sodium carbonate, Na2CO3 is dissolved in enough water to mak...
Free Test
Community Answer
25.3 g of sodium carbonate, Na2CO3 is dissolved in enough water to mak...

= 2.53/106   2.59 × 10-2  5.9 × 10-2
0.238 × 0.25          = 1.18 × 10-3

250 ml - 0.238

= 0.955

0.955  0.955 
Attention Class 11 Students!
To make sure you are not studying endlessly, EduRev has designed Class 11 study material, with Structured Courses, Videos, & Test Series. Plus get personalized analysis, doubt solving and improvement plans to achieve a great score in Class 11.
Explore Courses for Class 11 exam

Top Courses for Class 11

25.3 g of sodium carbonate, Na2CO3 is dissolved in enough water to make 250 mL of solution. If sodium carbonate dissociates completely, molar concentration of sodium ions, Na+and carbonate ions, are respectively.(At. mass of carbon = 40)a)0.477 M and 0.477 Mb)0.955 M and 1.910 Mc)1.910 M and 0.955 Md)1.90 M and 1.910 MCorrect answer is option 'C'. Can you explain this answer?
Question Description
25.3 g of sodium carbonate, Na2CO3 is dissolved in enough water to make 250 mL of solution. If sodium carbonate dissociates completely, molar concentration of sodium ions, Na+and carbonate ions, are respectively.(At. mass of carbon = 40)a)0.477 M and 0.477 Mb)0.955 M and 1.910 Mc)1.910 M and 0.955 Md)1.90 M and 1.910 MCorrect answer is option 'C'. Can you explain this answer? 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 25.3 g of sodium carbonate, Na2CO3 is dissolved in enough water to make 250 mL of solution. If sodium carbonate dissociates completely, molar concentration of sodium ions, Na+and carbonate ions, are respectively.(At. mass of carbon = 40)a)0.477 M and 0.477 Mb)0.955 M and 1.910 Mc)1.910 M and 0.955 Md)1.90 M and 1.910 MCorrect answer is option 'C'. Can you explain this answer? covers all topics & solutions for Class 11 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 25.3 g of sodium carbonate, Na2CO3 is dissolved in enough water to make 250 mL of solution. If sodium carbonate dissociates completely, molar concentration of sodium ions, Na+and carbonate ions, are respectively.(At. mass of carbon = 40)a)0.477 M and 0.477 Mb)0.955 M and 1.910 Mc)1.910 M and 0.955 Md)1.90 M and 1.910 MCorrect answer is option 'C'. Can you explain this answer?.
Solutions for 25.3 g of sodium carbonate, Na2CO3 is dissolved in enough water to make 250 mL of solution. If sodium carbonate dissociates completely, molar concentration of sodium ions, Na+and carbonate ions, are respectively.(At. mass of carbon = 40)a)0.477 M and 0.477 Mb)0.955 M and 1.910 Mc)1.910 M and 0.955 Md)1.90 M and 1.910 MCorrect answer is option 'C'. Can you explain this answer? in English & in Hindi are available as part of our courses for Class 11. Download more important topics, notes, lectures and mock test series for Class 11 Exam by signing up for free.
Here you can find the meaning of 25.3 g of sodium carbonate, Na2CO3 is dissolved in enough water to make 250 mL of solution. If sodium carbonate dissociates completely, molar concentration of sodium ions, Na+and carbonate ions, are respectively.(At. mass of carbon = 40)a)0.477 M and 0.477 Mb)0.955 M and 1.910 Mc)1.910 M and 0.955 Md)1.90 M and 1.910 MCorrect answer is option 'C'. Can you explain this answer? defined & explained in the simplest way possible. Besides giving the explanation of 25.3 g of sodium carbonate, Na2CO3 is dissolved in enough water to make 250 mL of solution. If sodium carbonate dissociates completely, molar concentration of sodium ions, Na+and carbonate ions, are respectively.(At. mass of carbon = 40)a)0.477 M and 0.477 Mb)0.955 M and 1.910 Mc)1.910 M and 0.955 Md)1.90 M and 1.910 MCorrect answer is option 'C'. Can you explain this answer?, a detailed solution for 25.3 g of sodium carbonate, Na2CO3 is dissolved in enough water to make 250 mL of solution. If sodium carbonate dissociates completely, molar concentration of sodium ions, Na+and carbonate ions, are respectively.(At. mass of carbon = 40)a)0.477 M and 0.477 Mb)0.955 M and 1.910 Mc)1.910 M and 0.955 Md)1.90 M and 1.910 MCorrect answer is option 'C'. Can you explain this answer? has been provided alongside types of 25.3 g of sodium carbonate, Na2CO3 is dissolved in enough water to make 250 mL of solution. If sodium carbonate dissociates completely, molar concentration of sodium ions, Na+and carbonate ions, are respectively.(At. mass of carbon = 40)a)0.477 M and 0.477 Mb)0.955 M and 1.910 Mc)1.910 M and 0.955 Md)1.90 M and 1.910 MCorrect answer is option 'C'. Can you explain this answer? theory, EduRev gives you an ample number of questions to practice 25.3 g of sodium carbonate, Na2CO3 is dissolved in enough water to make 250 mL of solution. If sodium carbonate dissociates completely, molar concentration of sodium ions, Na+and carbonate ions, are respectively.(At. mass of carbon = 40)a)0.477 M and 0.477 Mb)0.955 M and 1.910 Mc)1.910 M and 0.955 Md)1.90 M and 1.910 MCorrect answer is option 'C'. Can you explain this answer? tests, examples and also practice Class 11 tests.
Explore Courses for Class 11 exam

Top Courses for Class 11

Explore Courses
Signup for Free!
Signup to see your scores go up within 7 days! Learn & Practice with 1000+ FREE Notes, Videos & Tests.
10M+ students study on EduRev