# SOLUTION TO MOLARITY OF SALT PRODUCED IN A REACTION

HERE IS THE DETAILED SOLUTION.

QUESTION👇🏼👇🏼👇🏼

What is the molarity of the salt produced in the reaction of 200ml of 0.1M HCl with 100ml of 0.5M KOH ?

*SOLUTION*👇🏼👇🏼👇🏼👇🏼

THE REACTION FOR THE EQUATION👇🏼

HCl + KOH–> KCl+H20

The salt formed is KCl.

So we are looking for the molarity or concentration of KCl according to the question.

From the balanced equation, mole ratio of HCl : KOH : KCl👉🏼 1 : 1 : 1

This👆🏽means that in the reaction between HCl and KOH, the moles of HCl and KOH to be mixed together should be equal amounts and the mole of the salt KCl they will form will still be equal to that same mole of each of HCl and KCl mixed in the reaction.

👉🏼HCl : KOH : KCl

👉🏼 1mol  :  1mol :  1mol

Remember, a certain quantity of HCl and a certain quantity of KOH were mixed together, and we are asked to find the molarity (concentration) of the salt(KCl) formed in the reaction.

REMEMBER👇🏼👇🏼👇🏼👇🏼

Molarity means Concentration

And we know tha👇🏼

👉🏼Conc = mole/Vol

*Therefore*👇🏼

👉🏼Mole= Conc x Vol

So, let us find out the mole of each of HCl and KOH that were mixed together in that reaction.

*FOR HCl*

Conc. = mole/ Vol

Conc = 0.1M

Vol = 200ml

Converting Volume to litre, we have👇🏼

= 200/1000

Vol = 0.2L

So,

mole = Conc x Vol

= 0.2×0.1= 0.02mol of HCl

*FOR KOH*

Conc. = mole/ Vol

Conc = 0.5M

Vol = 100ml

Converting Volume to litre, we have👇🏼

= 100/1000

Vol = 0.1L

So,

mole = Conc x Vol

= 0.5×0.1= 0.05mol of KOH.

It means that in the reaction, 0.02mol of HCl was mixed with 0.05mol of KOH, which is wrong because👇🏼

From the balanced equation, it should be👇🏼

1 : 1 : 1

1mol HCl will combine with 1mol KOH to produce 1mol KCl

So, it should be either 0.02mol of HCl to be mixed with 0.02mol of KOH

But in the reaction, 0.02mol HCl was mixed with 0.05mol KOH which is not balanced because the 0.05mol quantity of KOH that was added was in excess.

Therefore, in order to balance it, only 0.02 mol of KOH will react and not the 0.05mol that was added.

So, if 0.02mol HCl reacts with only 0.02mol KOH, therefore only 0.02 mol of the salt KCl will be produced.

Since we now know the mole of KCl formed and we know the Volume if it which is the volume of the products (total volume)👇🏼

We can now find the molarity of the salt KCl formed.

👇🏼👇🏼👇🏼👇🏼👇🏼👇🏼👇

mole of KCl = 0.02mol

Vol of KCl formed = Total volume of HCl and KOH mixed together👇🏼👇🏼

Total volume of products👇🏼

= 200+100=300ml

Converting to litre, we have👇🏼

Total Vol = 200ml + 100ml

= 300ml

Converting the total volume to litre, we have👇🏼

= 300/1000

= 0.3L

NOTE👇🏼

Conc = mole/Vol

Conc = Molarity

Molarity= mol/Vol

Conc = 0.02/0.3

THE CATALYST…08068113736.
= 0.0667M ✅

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Notify of Inline Feedbacks May 19, 2020 12:10 pm

This understandable and explicit.. May 15, 2020 6:05 am

Hmmm
I don't understand May 14, 2020 1:18 pm

Chat me up May 14, 2020 11:20 am

Still can't understand the solving 😔😔😔 May 12, 2020 10:13 pm

Awesome
Tactical tho May 12, 2020 5:46 pm

This type is the one futo usually set for its students!! May 12, 2020 12:55 pm

This involves high level of Chemistry knowledge 🤣🤣🤣🤣🤣 May 12, 2020 10:37 am

No May 12, 2020 9:25 am

Had it been the two moles are thesame, May 12, 2020 7:53 am

Wow May 12, 2020 7:26 am

Wow.. thanks May 12, 2020 7:18 am

Wow this is tactical

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