acids bases buffers and indicators
How do you work out the pH of a solution from its concentration and vice versa?
For example
what is the pH of a solution of Sodium Hydroxide of 0.015 moldm⁻³?
For example
what is the pH of a solution of Sodium Hydroxide of 0.015 moldm⁻³?
So you have NaOH —> OH- + Na+
Since you have [NaOH], you can work out [OH-] using the ratios.
Then you need to use the ionisation of water equation: Kw = [H+][OH-]
Kw is a constant value (1x10^-14) so you can rearrange the equation to find [H+].
Then use pH = -log([H+]) to find the answer
I hope this helps!
Since you have [NaOH], you can work out [OH-] using the ratios.
Then you need to use the ionisation of water equation: Kw = [H+][OH-]
Kw is a constant value (1x10^-14) so you can rearrange the equation to find [H+].
Then use pH = -log([H+]) to find the answer
I hope this helps!
Original post by Chopinnocturne31
So you have NaOH —> OH- + Na+
Since you have [NaOH], you can work out [OH-] using the ratios.
Then you need to use the ionisation of water equation: Kw = [H+][OH-]
Kw is a constant value (1x10^-14) so you can rearrange the equation to find [H+].
Then use pH = -log([H+]) to find the answer
I hope this helps!
Since you have [NaOH], you can work out [OH-] using the ratios.
Then you need to use the ionisation of water equation: Kw = [H+][OH-]
Kw is a constant value (1x10^-14) so you can rearrange the equation to find [H+].
Then use pH = -log([H+]) to find the answer
I hope this helps!
Hi thank you so much! that's what I thought too but its a multiple choice questions with answers
12.2
12.8
13.2
13.8
so im a bit confused on how they got these answers but maybe I'm doing it wrong.
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