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Question

If 500 ml of 0.2M NaCl solution is mixed with 200 ml of 0.16M NaCl solution and then diluted to one liter with water, what is the molarity of the resulting solution?

A
0.2M
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B
0.33M
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C
0.42M
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D
0.54M
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Solution

The correct option is B 0.42M
Two solutions are mixed, hence the molarity of the resulting solution is calculated using the formula-
M1V1 + M2V2 = M(V1+V2)
where M1 is 0.2M, V1 is 500ml, M2 is .16M and V2 is 200ml and M is the molarity of the resulting solution which is to be found out. Putting the values in the equation we get,
(0.2500) + (0.16200) = M(500+200)
From this, the value of M is obtained as 0.18M.
The solution was then diluted to one litre. We already had (500+200)ml that is 700ml. Thus to make it one litre, we added 300ml of water. And the new molarity has now become M′′
We will now use the formula MV=M′′V′′
M is 0.18M, V is 700ml, M′′ is to be found out and V′′ is 300ml
Putting these values in the above equation we get,
0.18700=M′′300
Thus, M′′ = 126300, which is equal to 0.42M
Option C is the correct answer.

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