do both please as they are the part of the same question.. Part BFor 300.0 mL of a buffer solution that is 0.245 M in HCHO2 and 0.300 M in KCHO2, calculate the initial pH and the final pH after adding 0.029 mol of NaOH ( K.(HCHO2) = 1.8 x 10 4)Express your answers to two decimal places. Enter your answers numerically separated by a comma.pHmital: PHnmal = 3.82,3.94SubmitPrevious Answers Request AnswerX Incorrect; Try Again; 2 attempts remainingTo find the initial pH of a buffer solution, use the Henderson-Hasselbalch equation,pH = pK, + log-[base][acid|where (base] and Jacid] are the concentrations of the conjugate base and acid, respectively. Then, to find the pH of the final solution, calculate the numbers of moles of HCHO2 and CHO2 after the addition of NaOH There willbe 0.029 fewer moles of the acid and 0.029 more moles of the base after addition of the strong base. Substitute these values into the Henderson-Hasselbalch equation.Part CFor 300.0 mL of a buffer solution that is 0.280 M in CH3CH2NH2 and 0.220 M in CH3CH2NH3CI, calculate the initial pH and the final pH after adding 0.029 mol of NaOH ( KL (CH3CH2NH2) = 5.6 x 10 4.)Express your answers to two decimal places. Enter your answers numerically separated by a comma.pHinitial pHfinal =SubmitRequest Answer

Name: do both please as they are the part of the same question.. Part BFor 3
Uploaded: 2022-10-14T12:35:01.000Z
Channel: Bartleby
Description: do both please as they are the part of the same question.. Part BFor 300.0 mL of a buffer solution that is 0.245 M in HCHO2 and 0.300 M in KCHO2, calculate the initial pH and the final pH after adding 0.029 mol of NaOH ( K.(HCHO2) = 1.8 x 10 4)Expres