Question

the following solutions of NaOH are mixed together 20.ML of 3.0N, 40.mL of 2.0N, 60.mL of 1.0N, 80. mL of 4.0 N, and 100. mL of 5.0 N. what is the volume and normality of the final solution

Answer 1

The volume of the final solution is 300 mL, and the normality of the final solution is 3.40 N.

Step-by-step explanation:

To find the volume and normality of the final solution, we need to calculate the total amount of moles of NaOH in each solution and then combine them.

Step 1: Calculate the amount of moles for each solution.

• 20 mL of 3.0 N NaOH:

Moles = Volume (L) x Normality

= 0.020 L x 3.0 N

= 0.060 moles

• 40 mL of 2.0 N NaOH:

Moles = Volume (L) x Normality

= 0.040 L x 2.0 N

= 0.080 moles

• 60 mL of 1.0 N NaOH:

Moles = Volume (L) x Normality

= 0.060 L x 1.0 N

= 0.060 moles

• 80 mL of 4.0 N NaOH:

Moles = Volume (L) x Normality

= 0.080 L x 4.0 N

= 0.320 moles

• 100 mL of 5.0 N NaOH:

Moles = Volume (L) x Normality

= 0.100 L x 5.0 N

= 0.500 moles

Step 2: Calculate the total moles of NaOH by summing up the moles from each solution.

Total moles of NaOH = 0.060 + 0.080 + 0.060 + 0.320 + 0.500

= 1.020 moles

Step 3: Calculate the total volume of the final solution.

Total volume of the final solution = 20 mL + 40 mL + 60 mL + 80 mL + 100 mL

= 300 mL or 0.300 L

Step 4: Calculate the normality of the final solution.

Normality = Total moles of NaOH / Total volume of the solution (L)

= 1.020 moles / 0.300 L

= 3.40 N

Therefore, the volume of the final solution is 300 mL, and the normality of the final solution is 3.40 N.