Respuesta :
Answer:
The pH is greater than the pKa. There is more conjugate base than acid in solution. The answer is [HCHO2] < [NaCHO2]
Explanation:
Step 1: Data given
pKa of HCHO2 = 3.74
pH = 3.89 (HCHO2/NaCHO2)
This buffer contains formic acid ( CHOOH ), a weak acid ; and HCOONa ( the salt of its conjugate base, the formate anion, HCOO-)
Step 2: Calculate [HCOO-]/[HCOOH]
pH = pKa + log [HCOO-]/[HCOOH]
3.89 = 3.74 + log[HCOO-]/[HCOOH]
log[HCOO-]/[HCOOH] = 0.15
[HCOO-]/[HCOOH] = 10^-0.15 = 1.41
This means in the buffer there is 1.41 times more HCOO- (HCOONa) as HCOO (HCOOH) so [HCOONa] > [HCOOH]
The pH is greater than the pKa. There is more conjugate base than acid in solution. The answer is [HCHO2] < [NaCHO2]
The study of chemicals and bonds is called chemistry. The pKa is the pH value at which a chemical species will accept or donate a proton.
The correct answer is The pH is greater than the pKa.
The data is given as follow:-
- pKa of HCHO2 = 3.74
- pH = 3.89 (HCHO2/NaCHO2)
Buffer solution
- The buffer solution is defined as the solution which has the constant ph and it can not change.
- This buffer contains formic acid ( CHOOH ), a weak acid; and HCOONa ( the salt of its conjugate base, the formate anion, HCOO-)
The calculation is as follows:-
[tex]pH = pKa + log \frac{[HCOO^-]}{[HCOOH]}\\3.89 = 3.74 + log\frac{[HCOO^-]}{[HCOOH]}\\log\frac{[HCOO^-]}{[HCOOH]} = 0.15\\\frac{[HCOO-]}{[HCOOH]} \\\\= 10^{-0.15} = 1.41\\[/tex]
This means in the buffer there is 1.41 times more HCOO- (HCOONa) as HCOO (HCOOH) so [HCOONa] > [HCOOH]. The pH is greater than the pKa. There is more conjugate base than acid in the solution. The answer is [tex][HCHO_2] < [NaCHO_2].[/tex]
Hence, the correct answer is mentioned above.
For more information about the question, refer to the link:-
https://brainly.com/question/491373
