Question

Describe the preparation of 100 mL 0.050 M and 100 mL 0.0050 M phosphate buffer (both having pH = 6.5) using solid NaH2PO4·2H2O and solid Na2HPO4·2H2O. For H2PO4- ⇌ HPO4 2-, Ka = 6.32 × 10-8 Afterward, write the balanced net ionic equation describing the phosphate buffer system and explain with the use of balanced net ionic equations how the phosphate buffer resisted a drastic change in pH upon the addition of: a. 0.20 M NaOH b. 0.20 M HCl

Name: describe the preparation of 100 ml 0050 m and 100 ml 00050 m phosphate buffer both having ph 65 using solid nah2po42h2o and solid na2hpo42h2o for h2po4 hpo4 2 ka 632 10 8 after which write t 47552
Uploaded: 2022-12-14T06:36:50-08:00
Duration: 3 min 36 s
Channel: Sri K
Description: describe the preparation of 100 ml 0050 m and 100 ml 00050 m phosphate buffer both having ph 65 using solid nah2po42h2o and solid na2hpo42h2o for h2po4 hpo4 2 ka 632 10 8 after which write t 47552

          Describe the preparation of 100 mL 0.050 M and 100 mL 0.0050 M phosphate buffer (both having pH = 6.5) using solid NaH2PO4·2H2O and solid Na2HPO4·2H2O.
For H2PO4- ⇌ HPO4 2-, Ka = 6.32 × 10-8
Afterward, write the balanced net ionic equation describing the phosphate buffer system and explain with the use of balanced net ionic equations how the phosphate buffer resisted a drastic change in pH upon the addition of:
a. 0.20 M NaOH
b. 0.20 M HCl

Added by Natalie M.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Sri K

12/14/2022

Step 1

Preparation of 0.050 M phosphate buffer: First, we need to calculate the amount of NaH2PO4·2H2O and Na2HPO4·2H2O needed. The pKa of H2PO4- is the negative logarithm of Ka, which is 7.2. Using the Henderson-Hasselbalch equation, pH = pKa + log([A-]/[HA]), where Show more…

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Describe the preparation of 100 mL 0.050 M and 100 mL 0.0050 M phosphate buffer (both having pH = 6.5) using solid NaH2PO4·2H2O and solid Na2HPO4·2H2O. For H2PO4- ⇌ HPO4 2-, Ka = 6.32 × 10-8 Afterward, write the balanced net ionic equation describing the phosphate buffer system and explain with the use of balanced net ionic equations how the phosphate buffer resisted a drastic change in pH upon the addition of: a. 0.20 M NaOH b. 0.20 M HCl