It looks to me that you haven't learnt the ionic product of water yet. This is a constant at constant tenperature, Kw=1×10^-14mol^2dm^-6 at 298k. Kw=[OH-][H+]. If you know the concentration of H+ in solution, you can rearrange the Kw formula to find [OH-].
It looks to me that you haven't learnt the ionic product of water yet. This is a constant at constant tenperature, Kw=1×10^-14mol^2dm^-6 at 298k. Kw=[OH-][H+]. If you know the concentration of H+ in solution, you can rearrange the Kw formula to find [OH-].
From the first part of the question, it doesn't give you the conc of H+. And yes i have done the ionic product of water. I got an A* at a-level and I am studying chemistry at Oxford.
It looks to me that you haven't learnt the ionic product of water yet. This is a constant at constant tenperature, Kw=1×10^-14mol^2dm^-6 at 298k. Kw=[OH-][H+]. If you know the concentration of H+ in solution, you can rearrange the Kw formula to find [OH-].
to be fair you will have to use it but the first step requires the knowledge of what i said
From the first part of the question, it doesn't give you the conc of H+. And yes i have done the ionic product of water. I got an A* at a-level and I am studying chemistry at Oxford.
It has just occurred to me that I have replied to the wrong person, ignore me.
Is this right : kW= [H+][OH-] 10^-14 = 0.02 x [h+] [h+] = 10^-14 / 0.02 = 5x10^-3
Almost! You are getting the concentration of the HO- and H+ mixed up. The question says there are 0.02 moles of NaOH which means there are how many moles of HO- ions? (Hint: NaOH completely dissociates in water as it is a strong base) now that we have the conc. of H+, use the pH formula to work out pH.
Do not look at the spoiler until you are sure you have the answer!
Question 1 I believe you have the correct answer, though I would write 1.70 as 2d.p is generally the accepted form.