a) Describe in detail how you would prepare a 1-liter solution of 100 mM sodium phosphate buffer with a pH of 8.0 using 6 M HCl? The pKa value of sodium phosphate is approximately 7.2. The MW of dibasic sodium phosphate Na2HPO4 is 141.96 g/mol.

b) Calculate the final concentration of monobasic sodium phosphate, NaH2PO4 (conjugate acid), once youâve prepared the buffer. 3.

answer

watching

321

views

For unlimited access to Homework Help, a Homework+ subscription is required.

You have 0 free answers left.
Get unlimited access to 3.8 million step-by-step answers.

Get unlimited access

Already have an account? Log in

Keith LeannonLv2

14 Aug 2019

Unlock all answers

Get 1 free homework help answer.

Already have an account? Log in

Join us on Discord

Chemistry Study Group

Join now

Related questions

You need to prepare 5 liters of 2 M sodium phospate buffer, pH 7.4. You have stocks of 1 M monobasic sodium phosphate (NaH₂PO₄) and 1 M dibasic sodium phosphste (Na₂HPO₄). How much of each stock solution should be combined to make this buffer? The pKa of monobasic sodium phosphate is 6.82.

You need to prepare a buffer for biochemistry lab. The required solution is 0.5Msodium phosphate, pH 7.0. Use the Henderson-Hasselbalch equation to calculate the number of moles and grams of moobasic sodium phosphate ( NaH2PO4) and dibasic sodium phosphate ( Na2HPO4) necessary to make 1 liter of solution. The pKa for this buffer is 7.21