Acids and bases chemistry problems

[busted]

I am a little stuck on this question :

Solution A contains n moles of a weak acid HX. The addition of some sodium hydroxide to A neutralises one third of the HX present to produce Solution B.
In terms of the amount, n how many moles of HX are present in Solution B?
I think there are one third n moles.

It then asks to determine the ratio : ____(HX)_____
(X^-)
in solution B ... I AM TOTALLY STUCK WHAT TO DO HERE!

ANY HELP PLEASE

 

[Stevedye56]

Show how you got what you think is correct, then people will be able to help you understand more.

 

[Blueshift5]

Based on the information provided, it can be determined that the initial amount of HX in solution A was n moles. After the addition of sodium hydroxide, one third of the HX was neutralized, meaning that two thirds of the original amount of HX remains in solution B. Therefore, the amount of HX in solution B can be calculated as (2/3)n moles.

To determine the ratio of HX to X- in solution B, we need to know the molar ratio between HX and X-. This can be determined from the balanced chemical equation for the neutralization reaction between HX and sodium hydroxide. For example, if the reaction is:

HX + NaOH → NaX + H2O

Then the molar ratio between HX and X- is 1:1. This means that for every 1 mole of HX, 1 mole of X- is produced.

Therefore, the ratio of HX to X- in solution B is (2/3)n:(2/3)n, or simply 1:1. This means that for every 1 mole of HX, there is also 1 mole of X- present in solution B.

I hope this explanation helps you understand the problem better. If you have any further questions, please don't hesitate to ask.