What is the pH of a solution made by mixing 100.0 mL of 0.10 M HNO_{3}, 50.0 mL of 0.20 M HCl, and 100.0 mL of water? Assume that the volumes are additive. Enter your answer with two decimal places.

a. 0.87

b. 2.70

c. 3.50

d. 1.10

e. 0.52

We're being asked to calculate the pH of a solution made by mixing 100.0 mL of 0.10 M HNO3, 50.0 mL of 0.20 M HCl, and 100.0 mL of water.

• **pH**

▪ pH stands for the negative logarithmic function of hydronium ion concentration**▪** can be calculated using the following equation:

$\overline{){\mathbf{pH}}{\mathbf{=}}{\mathbf{-}}{\mathbf{log}}{\mathbf{}}\left[{\mathbf{H}}^{\mathbf{+}}\right]}$

Take note that: **[H ^{+}] = [H_{3}O^{+}]**

We're going to calculate the pH of the solution using the following steps:

**Step 1.** Calculate the total moles of H_{3}O^{+} ions in the solution.**Step 2. **Calculate the total volume of the solution (in L).**Step 3.** Calculate the total concentration of H_{3}O^{+} ions in the solution.**Step 4. **Calculate the pH of the solution.

Strong Acid-Base Calculations

Strong Acid-Base Calculations

Strong Acid-Base Calculations

Strong Acid-Base Calculations

Strong Acid-Base Calculations