How do you neutralize pH of a solution by not knowing concentration [closed]








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If I had a pH 10 in a 100ml solution of water and 93% sodium hydroxide how much mg/l of 93% sulfuric acid would we need to use to reach a pH of 4.


From my dated college chem books and a lot of google searching i know


1.) One mole of sulfuric acid will neutralize two moles of sodium hydroxide, as follows:


$$\ce{2NaOH + H2SO4 → Na2SO4 + 2H2O}$$ (the result is two water and one salt) 


2.) 1 Gallon = 3785.41 mL or 378.541 L


3.) pH + POH = 14


4.) In one minutes time we will have 100 gallons or 378541ml (100 gallons \* 3785.41 = 378541 mL)


5.) pH = 10 (of our water/sodium hydroxide solution.) 


6.) The hydronium ion concentration can be found from the pH by the reverse of the mathematical operation employed to find the pH.



```
 10^(-pH) = hydronium ion concentration

 hydronium ion concentration = 10^-10 = 1e-10 M or 0.0000000001 mol/l

 378.541 L * 0.0000000001 mol/l = 3.78541e-8 moles

 we need a hydronium ion concentration of 10^-4 which is 0.0001 mol/l

```

**How do i put this all together?**


