Ask questions and get helpful responses.

Chemistry

A buffer was prepared by mixing 1.00 mol of ammonia 𝑁𝐻3 πΎπ‘Ž =
5.8 Γ— 10βˆ’10 and 1.00 mol of ammonium chloride 𝑁𝐻4𝐢𝑙 to form an
aqueous solution with a total volume of 1.00 liter. To 500 mL of this
solution was added 30.0 mL of 1.00 M π‘π‘Žπ‘‚π». What is the resulting
pH of the final solution?

  1. 👍
  2. 👎
  3. 👁
  4. ℹ️
  5. 🚩
  1. The initial buffer solution is 1L of 1 M NH3 + 1M NH4Cl and you take 500 mL of that solution and add NaOH to it. In the second solution you have 0.5 L consisting of 0.5 mol NH3 and 0.5 mol NH4Cl. You add 30 mL of 1 M NaOH which is 0.03 x 1 = 0.03 mol OH^-.
    ................NH4^+ + OH^- ==> NH3 + H2O
    I...............0.5............0.................0.5....................
    add........................0.03..................................
    C...........-0.03.......-0.03.............+0.03
    E...........0.47.............0................0.53
    Plug the E line into the Henderson-Hasselbalch equation and solve for pH.
    Post your work if you get stuck.

    1. 👍
    2. 👎
    3. ℹ️
    4. 🚩
    👤
    DrBob222
  2. WHAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAAA

    1. 👍
    2. 👎
    3. ℹ️
    4. 🚩
  3. dddddddddddaa

    1. 👍
    2. 👎
    3. ℹ️
    4. 🚩
  4. Thank u veryy helpfull

    1. 👍
    2. 👎
    3. ℹ️
    4. 🚩

Respond to this Question

First Name

Your Response

Still need help? You can ask a new question.