Checking to see if I did this right?

Titration of HN03 titrated with NaOH
ending result is 1.38.

Titration A, endpoint pH = 8 is pKa or pKb= 1.38x106=5.861 and

Titration of NH03 titrated with KOH ending results 1.54.

Titration B, endpoint pH = 7 is KaorKb=
Ka=1.54x105

Beats me. I don't know what you're describing.

To check if you did this right, let's break down the information and calculations you provided.

In titration A, you titrated HNO3 with NaOH, and the ending result of the titration is pH = 1.38. You then calculated pKa or pKb using the equation 1.38 x 10^6 = 5.861.

To verify this calculation, you need to determine if the value of pKa or pKb is within the expected range for HNO3. Nitric acid (HNO3) is a strong acid, so its pKa is extremely low and the pKb is not applicable. Checking reference tables or literature sources for the pKa of HNO3, you will find that it is actually around -1.3.

Therefore, the calculated value of 5.861 for pKa seems incorrect. It is much higher than the expected value for HNO3 pKa.

Now let's move on to titration B, where you titrated NH3 with KOH, and the ending result of the titration is pH = 1.54. You calculated Ka using the equation 1.54 x 10^5.

To determine if this calculation is correct, you need to compare the calculated value to the expected range for NH3. Ammonia (NH3) is a weak base, so its Ka value is extremely small. The expected range for Ka of NH3 is in the range of 10^-34 or lower.

Therefore, the calculated value of 1.54 x 10^5 for Ka seems incorrect. It is much higher than the expected value for NH3 Ka.

In summary, the calculations for pKa and Ka in both titrations seem to be incorrect based on the expected values for HNO3 and NH3. It is recommended to review the equations and double-check your calculations to find the correct values.