Question

A 35.2-mL, 1.66 M KMnO4 solution is mixed with 16.7 mL of 0.892 M KMnO4 solution. Calculate the concentration of the final solution.

Answer 1

Answer:

1.4128

Explanation:

n=v*c

Cmix=nfinal/vfinal

cmix =(58.432+14.8864)/51.9

cfinal =1.4128

Answer 2

Answer:

The concentration of the final solution is 1.41 M.

Explanation:

To solve this problem, we need to use the formula for dilution:

$C1V1 = C2V2$

where C1 is the initial concentration, V1 is the initial volume, C2 is the final concentration, and V2 is the final volume.

We can start by finding the initial amount of KMnO4 in each solution:

Initial amount in 1st solution = C1 x V1

Initial amount in 1st solution = C1 x V1Initial amount in 2nd solution = C2 x V2

We can then combine the two solutions and find the final concentration:

Final amount = Initial amount in 1st solution + Initial amount in 2nd solution

Final volume = V1 + V2

Using the given values, we can solve for the final concentration:

Initial amount in 1st solution = 1.66 M x 35.2 mL

= 58.432 mmol KMnO4

Initial amount in 2nd solution = 0.892 M x 16.7 mL

= 14.8784 mmol KMnO4

Final amount = 58.432 mmol KMnO4 + 14.8784 mmol KMnO4

= 73.3104 mmol KMnO4

Final volume = 35.2 mL + 16.7 mL

= 51.9 mL

$final \: concentration = \frac{final \: amount}{final \: volume}$

$final \: concentration = \frac{73.3104mmol}{51.9ml}$

= 1.41 M

Therefore, the concentration of the final solution is 1.41 M.

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