the mole ratio of acid: salt in production of an acidic buffer solution is between 1/10 to 10/1. 

5mol HCOOH + 5mol KOH isn't a buffer solution, why? 

1mol HCOOH + 1mol HCOOK is a buffer solution, why?

 

Edited October 18, 20205 yr by mundane

What happens if you mix both. In first case what do you get and in second case what do you get. Compare the two results.

 

A buffer solution is an equilibrium mixture of either a (weak) acid and its conjugate base or a (weak) base and its conjugate acid.

So firstly you need to identify the acids, bases and conjugates in the two situations and whether they are strong or weak ?

Have you done this ?

Pudue University migh help you here

https://chemed.chem.purdue.edu/genchem/topicreview/bp/ch17/mixtures.php

Edited October 19, 20205 yr by studiot

On 10/17/2020 at 8:52 PM, mundane said:

the mole ratio of acid: salt in production of an acidic buffer solution is between 1/10 to 10/1. 

5mol HCOOH +Tell us more about what your goals are regarding buffers, then we can maybe get to some conclusion.  5mol KOH isn't a buffer solution, why? 

1mol HCOOH + 1mol HCOOK is a buffer solution, why?

 

Who said that the above is true?? I make buffers every day. Tell us what your goals are regarding buffers then we can get somewhere.  

 

Quote

A buffer solution (more precisely, pH buffer or hydrogen ion buffer) is an aqueous solution consisting of a mixture of a weak acid and its conjugate base, or vice versa

 

On 10/18/2020 at 3:52 AM, mundane said:

the mole ratio of acid: salt in production of an acidic buffer solution is between 1/10 to 10/1. 

5mol HCOOH + 5mol KOH isn't a buffer solution, why? 

1mol HCOOH + 1mol HCOOK is a buffer solution, why?

 

In first case will be a neutralization reaction between a weak acid and a strong base

5 mol HCOOH+5mol KOH=5 mol HCOOK+5 mol HOH    

Products are a salt (a conjugate  base  of a weack acid )and water

6 mol HCOOH+5 mol KOH=1 mol HCOOH+5 mol HCOOK+5 mol HOH  is a buffer solution