you are to make a buffer of pH = 4.33 using HNO2 and NaNO2 what ratio of NO2- to HNO2 is required?
To make a buffer of pH 4.33 using HNO2 and NaNO2, we need to find the ratio of NO2- to HNO2 required. To do this, we can use the Henderson-Hasselbalch equation, which states:
pH = pKa + log ([A-] / [HA])
In this case, HNO2 acts as the acid (HA) and NO2- acts as its conjugate base (A-). The pKa value for HNO2 is given as 3.4.
Rearranging the equation, we have:
[A-] / [HA] = 10^(pH - pKa)
Now, let's plug in the values: pH = 4.33 and pKa = 3.4
[A-] / [HA] = 10^(4.33 - 3.4)
[A-] / [HA] = 10^0.93
Using a calculator, we find 10^0.93 ≈ 8.68
So, the required ratio of NO2- to HNO2 is approximately 8.68.