Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: Buddy_123 on February 12, 2021, 08:09:03 PM
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Is there a way to use the ice table to find the pH of 0.1 NaCl?
I know that the strong acid (HCl) and strong base (NaOH) means that it is neutral so the pH is 7. But I'm not sure how I'd show that using the Ice table.
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The pH of a salt solution is low, 5
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The pH correction related to the ionic strength of the solution is outside the ICE table. For a 0.1 M NaCl solution, this correction will be negligible. Read an advanced physical chemistry textbook.
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The pH of a salt solution is low, 5
Show your calculations.
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The pH of a salt solution is low, 5
Show your calculations.
Dissolve salt in water, measure pH.
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The pH of a salt solution is low, 5
Show your calculations.
Dissolve salt in water, measure pH.
Did that just now and I got pH ~6.5
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The pH of a salt solution is low, 5
Show your calculations.
Dissolve salt in water, measure pH.
Did that just now and I got pH ~6.5
Because it depends on water more than on salt)
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The pH of a salt solution is low, 5
Show your calculations.
Dissolve salt in water, measure pH.
Did that just now and I got pH ~6.5
Because it depends on water more than on salt)
The water I used was distilled and had a measured pH, on a recently calibrated pH meter, of ~7.1 before I added the salt and ~6.5 afterwards.
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Maybe I was exaggerating a little when I said 5, but on the whole salt reduces pH. Could be to do with additional absorption of CO2 from the atmosphere. The saline solution we use measures 5.5. How much salt did you add?
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How much salt did you add?
Enough to make 0.1M NaCl
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May be due to some impurity in the salt.
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May be due to some impurity in the salt.
It was >99% NaCl sold by a reputable chemical lab supplier.