### Problem 18: Calculate the Following Dilutions- **Calculate the final volume:** - 125 mL solution made from 15.0 mL of 3.01 M HCl.- **Calculate the concentration:** - How many mL solution will be made if 5.00 mL of 6.10 M HCl is used to make a 0.103 M solution?- **Calculate the starting volume:** - 50.0 mL of a 3.00 M solution of HCl is made from how many mL of a 12.1 M HCl solution.- **Determine the starting volume for desired concentration:** - How many mL of a 1.00 M solution will make 25.0 mL of a 0.0100 M solution?### Note:For each calculation, remember to use the formula for dilution:\[ C_1 \times V_1 = C_2 \times V_2 \]Where:- \( C_1 \) and \( C_2 \) are the initial and final concentrations,- \( V_1 \) and \( V_2 \) are the initial and final volumes.

Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question and specify the other subparts (up to 3) you’d like answered .In this question, dilution is made in the different solutions. The three subparts are given below : (a) calculation of molarity of 125 mL solution made from 15.0 mL of a 3.01 M HCl . (b) calculation of volume of solution will be made if 5.00 mL of 6.10 M HCl is used to make 0.103 M solution (c) calculation of volume of 12.1 M HCl solution is used when 50 mL of a 3.00 M solution is made .On dilution , concentration or volume of a solution can be obtained by using the following formula : M1V1 = M2V2 ................... (1) Where, M1 = Molarity of solution 1 V1 = Volume of solution 1 M2 = Molarity of solution 2 V2 = Volume of solution 2Calculation of molarity of 125 mL solution made from 15.0 mL of a 3.01 M HCl : Given values are : Volume of solution 1 = 15.0 mL Molarity of solution 1 = 3.01 M Volume of solution 2 = 125 mL Let the molarity of solution 2 = M2 Now, put the values in equation (1), M1V1 = M2V23.01 M × 15.0 mL = M2 × 125 mLM2 = 3.01 M × 15.0 mL125 mL M2 = 0.3612 M Thus, the molarity of given 125 mL solution is 0.3612 M . Calculation of volume of solution will be made if 5.00 mL of 6.10 M HCl is used to make 0.103 M solution : Given values are : Volume of solution 1 = 5.00 mL Molarity of solution 1 = 6.10 M Molarity of solution 2 = 0.103 M Let the volume of solution 2 = V2 Now, put the values in equation (1), M1V1 = M2V26.10 M × 5.00 mL =0.103 M × V2V2 = 6.10 M × 5.00 mL0.103 M V2 = 296.116 mL Thus, the volume of given 0.103 M solution obtained will be 296.116 mL .Calculation of volume of 12.1 M HCl solution is used when 50 mL of a 3.00 M solution is made : Given values are : Volume of solution 1 = 50 mL Molarity of solution 1 = 3.00 M Molarity of solution 2 = 12.1 M Let the volume of solution 2 = V2 Now, put the values in equation (1), M1V1 = M2V23 M × 50 mL =12.1 M × V2V2 = 3 M × 50 mL12.1 M V2 = 12.3967 mL Thus, the volume of given 12.1 M solution obtained will be 12.3967 mL .Part (a) : The molarity of given 125 mL solution is 0.3612 M . Part (b) : The volume of given 0.103 M solution obtained will be 296.116 mL . Part (c) : The volume of given 12.1 M solution obtained will be 12.3967 mL .

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18. Calculate the following dilutions. 125 mL solution made from 15.0 mL of 3.01 M HCI How many mL solution will me made if 5.00 mL of 6.10 M HCI is used to make a 0.103 M solution? 50.0 mL of a 3.00 M solution of HCl is made from how many mL of a 12.1 M HCl solution. How ml of a 1.00 M solution will make 25.0 mL of a .0100 M many solution?

18. Calculate the following dilutions. 125 mL solution made from 15.0 mL of 3.01 M HCI How many mL solution will me made if 5.00 mL of 6.10 M HCI is used to make a 0.103 M solution? 50.0 mL of a 3.00 M solution of HCl is made from how many mL of a 12.1 M HCl solution. How ml of a 1.00 M solution will make 25.0 mL of a .0100 M many solution?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

### Problem 18: Calculate the Following Dilutions

- **Calculate the final volume:**
- 125 mL solution made from 15.0 mL of 3.01 M HCl.

- **Calculate the concentration:**
- How many mL solution will be made if 5.00 mL of 6.10 M HCl is used to make a 0.103 M solution?

- **Calculate the starting volume:**
- 50.0 mL of a 3.00 M solution of HCl is made from how many mL of a 12.1 M HCl solution.

- **Determine the starting volume for desired concentration:**
- How many mL of a 1.00 M solution will make 25.0 mL of a 0.0100 M solution?

### Note:

For each calculation, remember to use the formula for dilution:

\[ C_1 \times V_1 = C_2 \times V_2 \]

Where:
- \( C_1 \) and \( C_2 \) are the initial and final concentrations,
- \( V_1 \) and \( V_2 \) are the initial and final volumes.

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