Gen Chem!

[sshah92]

If 99% of the H+ ions in a solution of pH 1.3 were neutralized, what would be the final pH?

Eh?

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[Jepstein30]

If 99% of the H+ ions in a solution of pH 1.3 were neutralized, what would be the final pH?

Eh?

1) What is the concentration of H+ ions in a solution of pH 1.3?
2) Now take .01 (1%) of that since the other 99% are neutralized
3) Convert back to pH

Confusing terminology but you should be able to do the above! Post if you need more help.

 

[sshah92]

Thank you! For some reason I blanked on converting pHs to concentrations but this was actually rather simple haha

 

[sakabato93]

If 99% of the H+ ions in a solution of pH 1.3 were neutralized, what would be the final pH?

Eh?

If 99% of an acidic solution's hydronium ions were neutralized, it means that it went from a 100% to 1% hydronium ions, in other word, the amount of hydronium ions is decreased by a factor of 100 (10^(-2)). Since pH is -log[H+], the pH is changed by 2 (-log(10^(-2))= 2). The pH will go up by 2.