indicate the concentration of each ion presentin the solution formed by mixing 20mL of .1M HCL and 10mL of .22 M HCL
moles soln 1 = M x L = ?
moles soln 2 = M x L = ?
M mixture = total moles/total L
Then split that up between H^+ and Cl^- for the ions. Depending upon your teacher, you may want to use H3O^+ and not H^+.
Post your work if you get stuck.
To determine the concentration of each ion present in the solution formed by mixing 20 mL of 0.1 M HCl and 10 mL of 0.22 M HCl, you need to consider the following steps:
1. Determine the initial moles of HCl in each solution:
- Moles of HCl in 20 mL of 0.1 M HCl = 0.1 M x 0.02 L = 0.002 moles
- Moles of HCl in 10 mL of 0.22 M HCl = 0.22 M x 0.01 L = 0.0022 moles
2. Calculate the total moles of HCl in the final solution by summing up the moles from each solution:
- Total moles of HCl = 0.002 moles + 0.0022 moles = 0.0042 moles
3. Determine the total volume of the final solution by summing up the volumes of each solution:
- Total volume = 20 mL + 10 mL = 30 mL
4. Calculate the concentration of the final solution by dividing the total moles of HCl by the total volume of the solution:
- Concentration of the final solution = 0.0042 moles / 0.03 L = 0.14 M
Therefore, the concentration of each ion (H+ and Cl-) in the solution formed by mixing 20 mL of 0.1 M HCl and 10 mL of 0.22 M HCl is 0.14 M. Since HCl is a strong acid and fully dissociates in water, the concentration of the H+ ion is also 0.14 M, and the concentration of the Cl- ion is also 0.14 M.