To half of it (500. mL), you add 0.0100mol of hydrogen ions without changing the volume. What is the pH of the final solution?
To half of what?
To find the pH of the final solution, we need to determine the concentration of hydrogen ions ([H+]) in the solution. We can use the solution's volume and the amount of hydrogen ions added to calculate the concentration.
Given:
Total volume of the solution = 1000 mL (or 1.0 L)
Volume of the added hydrogen ions = 500 mL (or 0.5 L)
Amount of hydrogen ions added = 0.0100 mol
First, we need to determine the concentration of the added hydrogen ions in moles per liter (Molarity or M). We can use the formula:
Concentration (M) = Amount of substance (mol) / Volume (L)
Concentration of hydrogen ions = 0.0100 mol / 0.5 L = 0.0200 M
Next, we need to find the combined concentration of hydrogen ions in the final solution. Since we didn't change the total volume (1.0 L), the concentration of the original solution remains the same. We can calculate it using the formula mentioned above:
Concentration of original solution = 0.0100 mol / 1.0 L = 0.0100 M
Now, to determine the combined concentration of hydrogen ions, we add the concentration of the original solution and the concentration of the added hydrogen ions:
Combined concentration of hydrogen ions = Concentration of original solution + Concentration of added hydrogen ions
= 0.0100 M + 0.0200 M
= 0.0300 M
Finally, we can calculate the pH of the solution using the formula:
pH = -log[H+]
pH = -log(0.0300) = 1.477
Therefore, the pH of the final solution is approximately 1.477.