High School

Enter your answer in the provided box.

A quantity of [tex]2.00 \times 10 \, \text{mL}[/tex] of [tex]0.526 \, \text{M HCl}[/tex] is mixed with [tex]2.00 \times 10^2 \, \text{mL}[/tex] of [tex]0.263 \, \text{M Ba(OH)}_2[/tex] in a constant-pressure calorimeter of negligible heat capacity.

(Ensure to include any continuation or specific question details that might be relevant.)

Answer :

Final answer:

The final concentration of the resulting solution is approximately 0.266 M.

Explanation:

To calculate the final concentration of the resulting solution, we can use the formula:

C1V1 + C2V2 = C3V3

Where:

  • C1 is the concentration of the first solution (0.526 M)
  • V1 is the volume of the first solution (2.00 x 10 mL)
  • C2 is the concentration of the second solution (0.263 M)
  • V2 is the volume of the second solution (2.00 x 102 mL)
  • C3 is the final concentration of the resulting solution (unknown)
  • V3 is the volume of the resulting solution (unknown)

First, we need to convert the volumes to liters:

  • V1 = 2.00 x 10 mL = 2.00 x 10-3 L
  • V2 = 2.00 x 102 mL = 2.00 x 10-1 L

Now we can substitute the values into the formula:

(0.526 M)(2.00 x 10-3 L) + (0.263 M)(2.00 x 10-1 L) = C3V3

Simplifying the equation:

0.001052 + 0.0526 = C3V3

0.053652 = C3V3

Since the calorimeter has negligible heat capacity, the volume of the resulting solution is the sum of the volumes of the two solutions:

V3 = V1 + V2 = 2.00 x 10-3 L + 2.00 x 10-1 L = 2.02 x 10-1 L

Now we can solve for C3:

0.053652 = C3(2.02 x 10-1 L)

Dividing both sides by 2.02 x 10-1 L:

C3 = 0.053652 / (2.02 x 10-1 L)

Calculating the final concentration:

C3 ≈ 0.266 M

Learn more about calculating the final concentration of a solution after mixing here:

https://brainly.com/question/13992045

#SPJ14

Other Questions