the volume of water that must be added to a mixture of 250 ml of 0.6 M HCL and 750 ml of 0.2 M HCL to obtain 0.25 M solution of HCL
Answers
No. of moles of 0.6M HCl = 0.15
No. of moles of 0.2M HCl = 0.15
let V be the volume(in ml) of the 0.25M solution. No of moles present = 0.15+0.15 = 0.3
0.3*1000/v(ml) = 0.25 M
v = 1.2 lit.
Final answer: The volume of water to be added to obtain a final solution is .
Given that: We are given a mixture of of and of .
To find: We have to find the volume of water that must be added to a mixture of of and of to obtain solution of .
Explanation:
- When two solutions of the same compound but they differ in molarity and volumes are added to obtain a new solution.
- Let and are the molarity and volume of the solutions of same compound being mixed. And and are the molarity and volume of the final solution being formed.
- Here, two solutions of of different molarity and volume are mixed to form a new solution.
=
=
=
=
=
= ?
- Substitute these values in:
- Total volume of the final solution =
- The volume of the solution initially mixed,
- The volume of water we need to add to the initial solution to make the final solution =
=
=
- Hence, the volume of water to be added to obtain a final solution is .
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