600 mL of 0.04 M HCl is mixed with 400 mL of 0.02 M H2SO4. Find out the pH of resulting solution (Nearest integer).
Correct Answer: 1.4
Solution and Explanation
To calculate the pH of the resulting solution, we need to find the total moles of H+ ions from both the acids, HCl and H2SO4, and then determine the concentration of H+ ions in the mixed solution.
Step 1: Calculate moles of H+ from HCl
Moles of HCl = M × V = 0.04 M × 0.600 L = 0.024 moles of H+
Step 2: Calculate moles of H+ from H2SO4
Since H2SO4 is a strong acid and dissociates to give 2 moles of H+ ions per mole of H2SO4, the moles of H+ from H2SO4 will be:
Moles of H+ = 0.02 M × 0.400 L × 2 = 0.016 moles of H+
Step 3: Calculate total moles of H+ in the solution
Total moles of H+ = 0.024 + 0.016 = 0.040 moles of H+
Step 4: Calculate the final volume of the solution
Total volume = 600 mL + 400 mL = 1000 mL = 1 L
Step 5: Calculate the concentration of H+ ions
[H+] = Total moles of H+ / Total volume = 0.040 moles / 1 L = 0.040 M
Step 6: Calculate the pH of the solution
pH = -log [H+] = -log (0.040) = 1.4
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