What is the pH of a 500 mL solution that is 0.128 M HA after you add 0.300 moles of NaA

What is the pH of a 500 mL solution that is 0.128 M HA after you add 0.300 moles of NaA (the salt form of the conjugate)?

pKa = 5.01

Solution

pKa of HA = 5.01

According Henderson -Hasselbalch equation

pH = pKa +log [salt]/[acid]

pH = pKa + log [A-]/[HA]

[A-] = 500/01000 x 0.30 = 0.15

[HA] =0.128

pH =5.01 + log (0.15/0.128)= 5.01 + 0.0689 = 5.0789

Hence, pH of the solution is 5.0

 

 

>>Having difficult problems and need solutions in few minutes? Contact us at chemistryexperts1@gmail.com<<

>Was this helpful, would like to support us?<<

<<click here to Donate>>

 

Leave a Reply

Fill in your details below or click an icon to log in:

WordPress.com Logo

You are commenting using your WordPress.com account. Log Out /  Change )

Google photo

You are commenting using your Google account. Log Out /  Change )

Twitter picture

You are commenting using your Twitter account. Log Out /  Change )

Facebook photo

You are commenting using your Facebook account. Log Out /  Change )

Connecting to %s