What is the pH of a solution formed by mixing equal volumes of 0.1 M HCl and 0.1

What is the pH of a solution formed by mixing equal volumes of 0.1 M HCl and 0.1 M NaOH?

What is the pH of a solution formed by mixing equal volumes of 0.1 M HCl and 0.1 M NaOH?

Step 1: Identify the substances being mixed. We have 0.1 M HCl (a strong acid) and 0.1 M NaOH (a strong base).
Step 2: Understand that HCl and NaOH will react with each other. HCl donates protons (H+) and NaOH donates hydroxide ions (OH-).
Step 3: When HCl and NaOH mix, they neutralize each other. The reaction is: HCl + NaOH → NaCl + H2O.
Step 4: Since we are mixing equal volumes of both solutions, they will completely neutralize each other.
Step 5: After the neutralization, the resulting solution contains only water and NaCl, which does not affect the pH.
Step 6: The pH of pure water is 7, which is neutral.

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