Acid-Base Titration Help

[Pisiform]

---

Members don't see this ad.

Hey guys, I was just practicing few question from my undergrad book but I couldn't think of anyway of doing this. Although it has some tedious calculation and is least likely to show up on MCAT but still it bugs me:

Q - How many mL of 0.0850M NaOH is required to titrate 35mL of 0.0850M CH3COOH ? Ka = 1.8 * 10^-5

Answer: 35mL

All help is appreciated. Thanks

 

[IntelInside]

Hey guys, I was just practicing few question from my undergrad book but I couldn't think of anyway of doing this. Although it has some tedious calculation and is least likely to show up on MCAT but still it bugs me:

Q - How many mL of 0.0850M NaOH is required to titrate 35mL of 0.0850M CH3COOH ? Ka = 1.8 * 10^-5

Answer: 35mL

All help is appreciated. Thanks

If you look they are the same molarity therefore in order to titrate aka neutralize the acid all you have to do is add the same amount of base in this case

 

[Pisiform]

But isn't that its a strong base and weak acid. If it was strong acid and strong acid then it would be same!! ???

 

[IntelInside]

The pH will be greater than 7 obviously in this cause due to the fact that it is strong base/weak acid

For a strong:strong titration pH will be 7

 

[TwoPaddles]

But isn't that its a strong base and weak acid. If it was strong acid and strong acid then it would be same!! ???

Neutralization means mixing equal MOLE portions of an acid with a base, REGARDLESS of their concentrations and strengths.

 

[Dharma]

OP you may be thinking of making a buffered solution?