What is the concentration (in M) of H+ present in the solution formed by mixing 20 mL of 0.100 M HCl and 10.0 mL of 0.500 M HCl
moles H+=.02*.10+.01*.50
volume= .03liters
concentration= moles/liters
To find the concentration of H+ in the solution formed by mixing the two solutions, we need to use the concept of "mole proportion" and the volume of the mixed solution.
First, let's determine the number of moles of H+ in each solution. To do this, multiply the volume of each solution by its concentration:
Number of moles of H+ in 20 mL of 0.100 M HCl:
Moles = Volume (L) x Concentration (M)
Moles = (20 mL / 1000 mL/L) x 0.100 M
Moles = 0.002 mol
Number of moles of H+ in 10.0 mL of 0.500 M HCl:
Moles = Volume (L) x Concentration (M)
Moles = (10.0 mL / 1000 mL/L) x 0.500 M
Moles = 0.005 mol
Now, let's calculate the total moles of H+ in the mixed solution by adding the moles of H+ from each of the solutions:
Total moles of H+ = Moles from 0.100 M HCl + Moles from 0.500 M HCl
Total moles of H+ = 0.002 mol + 0.005 mol
Total moles of H+ = 0.007 mol
Finally, to determine the concentration of H+ in the mixed solution, divide the total moles of H+ by the total volume of the mixed solution:
Concentration (M) = Total moles of H+ / Total volume (L)
The total volume of the mixed solution is the sum of the volumes of the two solutions:
Total volume = 20 mL + 10.0 mL = 30.0 mL
Converting this to liters:
Total volume (L) = 30.0 mL / 1000 mL/L = 0.030 L
Now we can calculate the concentration of H+ in the mixed solution:
Concentration (M) = 0.007 mol / 0.030 L
Concentration (M) = 0.233 M
Therefore, the concentration of H+ in the solution formed by mixing 20 mL of 0.100 M HCl and 10.0 mL of 0.500 M HCl is 0.233 M.