JEE Exam  >  JEE Questions  >  500 mL of 0.250 M Na2SO4 solution is added to... Start Learning for Free
500 mL of 0.250 M Na2SO4 solution is added to an aqueous solution of 15.00g of BaCl2 resulting in formation of white precipitate of BaSO4 .How many grams of BaSO4 are formed?
Verified Answer
500 mL of 0.250 M Na2SO4 solution is added to an aqueous solution of 1...
Na2SO4 + BaCl2 ---> BaSO4 + 2NaCl 

Na2SO4 : 0.5 L (0.25 mol/L) = 0.125 mol 

BaCl2 : 15 g (1 mol/208.23 g) = 0.072 mol 

Now, 

0.072 mol BaCl2 (1 mol BaSO4/1 mol BaCl2) (233.43 g BaSO4/ 1 mol BaSO4) = 16.8 g BaSO4 
This question is part of UPSC exam. View all JEE courses
Most Upvoted Answer
500 mL of 0.250 M Na2SO4 solution is added to an aqueous solution of 1...
Given:
- Volume of Na2SO4 solution = 500 mL
- Concentration of Na2SO4 solution = 0.250 M
- Mass of BaCl2 = 15.00 g

Required:
- Mass of BaSO4 formed

Solution:
Step 1: Calculate the number of moles of Na2SO4
- The volume of Na2SO4 solution is given as 500 mL, which is equivalent to 0.5 L.
- The concentration of Na2SO4 solution is given as 0.250 M.
- Therefore, the number of moles of Na2SO4 can be calculated using the formula:
Moles = Concentration × Volume
Moles = 0.250 mol/L × 0.5 L
Moles = 0.125 mol

Step 2: Calculate the number of moles of BaCl2
- The molar mass of BaCl2 can be calculated by adding the atomic masses of Barium (Ba) and Chlorine (Cl).
Molar mass of BaCl2 = (1 × Atomic mass of Ba) + (2 × Atomic mass of Cl)
Molar mass of BaCl2 = (1 × 137.33 g/mol) + (2 × 35.45 g/mol)
Molar mass of BaCl2 = 137.33 g/mol + 70.90 g/mol
Molar mass of BaCl2 = 208.23 g/mol
- The mass of BaCl2 is given as 15.00 g.
- Therefore, the number of moles of BaCl2 can be calculated using the formula:
Moles = Mass / Molar mass
Moles = 15.00 g / 208.23 g/mol
Moles = 0.072 moles

Step 3: Determine the limiting reactant
- To find the limiting reactant, we compare the moles of Na2SO4 and BaCl2.
- The balanced chemical equation for the reaction between Na2SO4 and BaCl2 is as follows:
Na2SO4 + BaCl2 → BaSO4 + 2 NaCl
- From the balanced equation, we can see that the stoichiometric ratio between Na2SO4 and BaSO4 is 1:1.
- Therefore, the limiting reactant will be the one with a smaller number of moles.
- In this case, Na2SO4 has 0.125 moles and BaCl2 has 0.072 moles.
- Hence, BaCl2 is the limiting reactant.

Step 4: Calculate the moles and mass of BaSO4 formed
- From the balanced equation, we can see that 1 mole of BaCl2 reacts to form 1 mole of BaSO4.
- Therefore, the number of moles of BaSO4 formed will be equal to the moles of BaCl2, which is 0.072 moles.
- The molar mass of BaSO4 can be calculated by adding the atomic masses of Barium (Ba), Sulfur (S), and Oxygen (O).
Molar mass of BaSO4 = (1 × Atomic mass
Explore Courses for JEE exam

Similar JEE Doubts

500 mL of 0.250 M Na2SO4 solution is added to an aqueous solution of 15.00g of BaCl2 resulting in formation of white precipitate of BaSO4 .How many grams of BaSO4 are formed?
Question Description
500 mL of 0.250 M Na2SO4 solution is added to an aqueous solution of 15.00g of BaCl2 resulting in formation of white precipitate of BaSO4 .How many grams of BaSO4 are formed? for JEE 2024 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about 500 mL of 0.250 M Na2SO4 solution is added to an aqueous solution of 15.00g of BaCl2 resulting in formation of white precipitate of BaSO4 .How many grams of BaSO4 are formed? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 500 mL of 0.250 M Na2SO4 solution is added to an aqueous solution of 15.00g of BaCl2 resulting in formation of white precipitate of BaSO4 .How many grams of BaSO4 are formed?.
Solutions for 500 mL of 0.250 M Na2SO4 solution is added to an aqueous solution of 15.00g of BaCl2 resulting in formation of white precipitate of BaSO4 .How many grams of BaSO4 are formed? in English & in Hindi are available as part of our courses for JEE. Download more important topics, notes, lectures and mock test series for JEE Exam by signing up for free.
Here you can find the meaning of 500 mL of 0.250 M Na2SO4 solution is added to an aqueous solution of 15.00g of BaCl2 resulting in formation of white precipitate of BaSO4 .How many grams of BaSO4 are formed? defined & explained in the simplest way possible. Besides giving the explanation of 500 mL of 0.250 M Na2SO4 solution is added to an aqueous solution of 15.00g of BaCl2 resulting in formation of white precipitate of BaSO4 .How many grams of BaSO4 are formed?, a detailed solution for 500 mL of 0.250 M Na2SO4 solution is added to an aqueous solution of 15.00g of BaCl2 resulting in formation of white precipitate of BaSO4 .How many grams of BaSO4 are formed? has been provided alongside types of 500 mL of 0.250 M Na2SO4 solution is added to an aqueous solution of 15.00g of BaCl2 resulting in formation of white precipitate of BaSO4 .How many grams of BaSO4 are formed? theory, EduRev gives you an ample number of questions to practice 500 mL of 0.250 M Na2SO4 solution is added to an aqueous solution of 15.00g of BaCl2 resulting in formation of white precipitate of BaSO4 .How many grams of BaSO4 are formed? tests, examples and also practice JEE tests.
Explore Courses for JEE exam

Top Courses for JEE

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