What is the pH of a solution formed by mixing 25 mL of 0.1 M HCl with 25 mL of 0
Practice Questions
Q1
What is the pH of a solution formed by mixing 25 mL of 0.1 M HCl with 25 mL of 0.1 M NaOH? (2020) 2020
7
1
14
0
Questions & Step-by-Step Solutions
What is the pH of a solution formed by mixing 25 mL of 0.1 M HCl with 25 mL of 0.1 M NaOH? (2020) 2020
Step 1: Identify the substances being mixed. We have HCl (hydrochloric acid) and NaOH (sodium hydroxide).
Step 2: Determine the concentrations and volumes of each solution. We have 25 mL of 0.1 M HCl and 25 mL of 0.1 M NaOH.
Step 3: Calculate the number of moles of HCl. Moles = concentration (M) × volume (L). For HCl: 0.1 M × 0.025 L = 0.0025 moles.
Step 4: Calculate the number of moles of NaOH. For NaOH: 0.1 M × 0.025 L = 0.0025 moles.
Step 5: Understand that HCl and NaOH react in a 1:1 ratio to neutralize each other. Since we have equal moles of both, they will completely neutralize.
Step 6: After neutralization, the solution will contain only water and salt (NaCl), which does not affect the pH.
Step 7: Conclude that the resulting solution is neutral, which has a pH of 7.
