Question

A 0.401 g sample of KHP will be titrated with a NaOH solution with an assumed concentration of 0.100 M. Calculate the volume of NaOH that should neutralize the KHP sample.

For titrations, they normally give me the volume of the base, but they haven't done so in this question... so I have no idea where to start.
And thanks for your help!

Answer 1

Also ,unsure about the following question:

An empty beaker weighs 30.51 g.
a) When completely filled with water, the beaker and its contents have a total mass of 402.25 g. What volume does the beaker hold? Use d =1.00 g/mL as the density of water.
b) How much would the beaker and its contents weigh if it was completely filled with mercury? The density of mercury is d =13.5 g/mL.

The answers I got were a) 371.74 mL and b) 5049 g.

Thank you!

Answer 2

You have to realize, when you reach neutralization, the concentration of acid = concentration of base.
So write out the balanced equation for the reaction
Then since you're given concentration of the acid, you essentially have the base
Hope this helps!

Answer 3

As for number 2, it's a simple density conversion
You're given mass of the liquid, and also the density, solve for unknown using basic algebra.
Water has a very special density, 1mL of water is roughly 1g in mass, keep that in mind for future questions

Answer 4

Yes, for # 2, I did do use the d=m/v formula to get the #s but wanted to double check (the numbers look too big)

Answer 5

as for the 1st one, I got help on it. I convert the given grams to moles acid and use that to find the volume (through Molarity =mol/L). Then I just match the protonicity or w/e it's called and go on from there.

Thank you!

Answer 6

For #2, both your numbers are correct :)

Answer 7

oh, ok thank you!!!