Question

1. How many mL of a 0.103M NaOH solution are required to neutralize 10.00mL of a 0.198M HCI
solution?

Answer 1

Explanation:

1. How many mL of a 0.103M NaOH solution are required to neutralize 10.00mL of a 0.198M HCI

solution?

1245ml

Answer 2

The volume of NaOH reacted is 19.22 mL.

Given:

An 0.103M NaOH solution is reacted to neutralize 10.00mL of 0.198M HCI.

solution.

To Find:

The volume of NaOH reacted.

Solution:

To find the volume of NaOH reacted we will follow the following steps:

As we know,

At the equivalence point:

$M1V1(NaOH) = M2 V2( HCl)$

Also,

According to the question:

M1 = 0.103M

M2 = 0.198M

V2 = 10ml

Now,

In putting values we get,

$0.103 \times \: v1 = 0.198 \times 10$

$v1 = \frac{0.198 \times 10}{0.103} = 19.22ml$

Henceforth, the volume of NaOH reacted is 19.22 mL.

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