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AdnamaLeigh
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How do you calculate the pH of 0.001 M NaCl? I was thinking of doing NaCl + H2O ---> HCl + NaOH but I don't know where to go from there if that's even the right step.
mrjeffy321 said:A NaCl solution of any concentration should have (ideally) a pH of 7.
GCT said:The topic of ionic strength is practical with buffer preparation, however, I don't believe that it's an important factor with regard to the pH in this situation.
To calculate the pH of 0.001 M NaCl, you need to use the formula pH = -log[H+], where [H+] is the concentration of hydrogen ions in the solution. Since NaCl is a strong electrolyte, it dissociates completely into Na+ and Cl- ions. Therefore, the concentration of [H+] in the solution is equal to the concentration of [Cl-].
The concentration of [H+] in a 0.001 M NaCl solution is also 0.001 M, as explained in the previous answer. This is because the concentration of [H+] is equal to the concentration of [Cl-] in a solution of a strong electrolyte like NaCl.
The pH of a solution is determined by the concentration of hydrogen ions. In a 0.001 M NaCl solution, the concentration of [H+] is 0.001 M, which is considered a very low concentration. At this concentration, the solution is considered neutral, with a pH of 7 on the pH scale.
No, the pH of a 0.001 M NaCl solution cannot change. Since NaCl is a strong electrolyte, it completely dissociates into its ions and does not undergo any chemical reactions to produce or consume hydrogen ions. Therefore, the concentration of [H+] remains constant at 0.001 M, resulting in a constant pH of 7.
The concentration of NaCl does not directly affect the pH of a solution. However, it indirectly affects the pH by altering the concentration of [H+] through the process of dissociation. A higher concentration of NaCl will result in a higher concentration of [H+], leading to a lower pH, and vice versa.