Open Question
Find the percent ionization of a 0.337 m HF solution. the ka for hf is 3.5 × 10-4. What would you expect the percent ionization to be for the same concentration of hydrochloric acid (HCl)? Explain.
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17. Acid and Base Equilibrium
pH of Weak Acids
Multiple Choice
Which of the following is the correct pH of a solution formed by mixing 1.3 L of 0.45 M HCl with 5.5 L of 1.95 M HI?
A
0.30
B
0.15
C
0.70
D
1.20
Verified step by step guidance1
Step 1: Calculate the moles of HCl in the solution. Use the formula \( \text{moles} = \text{volume} \times \text{molarity} \). For HCl, \( \text{moles of HCl} = 1.3 \text{ L} \times 0.45 \text{ M} \).
Step 2: Calculate the moles of HI in the solution using the same formula. For HI, \( \text{moles of HI} = 5.5 \text{ L} \times 1.95 \text{ M} \).
Step 3: Add the moles of HCl and HI together to find the total moles of hydrogen ions \( \text{H}^+ \) in the solution, since both HCl and HI are strong acids and dissociate completely.
Step 4: Calculate the total volume of the solution by adding the volumes of HCl and HI solutions: \( \text{total volume} = 1.3 \text{ L} + 5.5 \text{ L} \).
Step 5: Determine the concentration of \( \text{H}^+ \) ions in the solution by dividing the total moles of \( \text{H}^+ \) by the total volume of the solution. Then, calculate the pH using the formula \( \text{pH} = -\log[\text{H}^+] \).
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