How to Calculate the pH of 0.001 M NaCl?

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SUMMARY

The pH of a 0.001 M NaCl solution is ideally 7, as sodium chloride is a strong electrolyte that dissociates completely in water without affecting the pH. The reaction NaCl + H2O does not lead to the formation of significant amounts of HCl or NaOH that would alter the pH. While ionic strength and activity coefficients are relevant in buffer preparation, they do not significantly impact the pH in this specific case of NaCl solutions.

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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.
 
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Sodium Chloride is a strong electrolyte meaning it will disassociate completely in solution.
Strong electrolytes will not affect the pH of the solution as the acids / bases they form are also strong electrolytes.

A NaCl solution of any concentration should have (ideally) a pH of 7.


NaCl (aq) + H2O (l) ---> HCl (aq) + NaOH (aq)
HCl (aq) + NaOH (aq) --> NaCl (aq) + H2O (l)
 
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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.
 
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.

It is an important factor in every solution containing ions. Even if it doesn't change numerical value of pH in this case, you can't assume that addition of neutral salt never changes pH of the solution.
 

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