Solutions of piperazine are basic (Kb1 =5.4×10-5 ; Kb2 =2.2×10-9 ). What is the pH of...

Question

Question

Solutions of piperazine are basic (Kb1 =5.4×10-5 ; Kb2 =2.2×10-9 ). What is the pH of a 0.0185 M solution of piperazine?

Answer 1

Answer #1

to draw ICE table.

then using ka1 to find OH- concentration.

then again to draw ICE table..

and using ka2 to find OH- concentration.

add total OH- then calculate pOH.

Answer 2

Similar Homework Help Questions

Calculate the pH for a 0.100 M Na2CO3 solution with a Kb1 of 2.1 x 10-4...

Calculate the pH for a 0.100 M Na2CO3 solution with a Kb1 of 2.1 x 10-4 and a Kb2 of 2.2 x 10-8
14. Drawn below are the structures of three diprotic weak bases: HN HN NH N Piperazine...

14. Drawn below are the structures of three diprotic weak bases: HN HN NH N Piperazine Kb = 5.3 x 10-5 Kb2 = 4.5 x 10-9 1-methylpiperazine Kb1 = 3.7 x 10-5 Kb2 = 1.7 x 10-9 1,4-dimethylpiperazine Koi = 1.4 x 10-5 Kb2 = 4.3 x 10-10 (vii) Determine the pH of a solution formed by dissolving 4.3 g of piperazine (86.14 g/mole) to make a solution with a final volume of 500 mL (viii) Determine the concentration of...
Quinine occurs naturally in the bark of the cinchona tree. For centuries it was the only...

Quinine occurs naturally in the bark of the cinchona tree. For centuries it was the only treatment for malaria. Quinine contains two weakly basic nitrogen atoms, with Kb1 = 3.3×10-6 and Kb2 = 1.4×10-9 at 25°C. Calculate the pH of a 0.0136 M solution of quinine in water.

Quinine occurs naturally in the bark of the cinchona tree. For centuries it was the only...

Quinine occurs naturally in the bark of the cinchona tree. For centuries it was the only treatment for malaria. Quinine contains two weakly basic nitrogen atoms, with Kb1 = 3.3×10-6 and Kb2 = 1.4×10-9 at 25°C. Calculate the pH of a 0.0131 M solution of quinine in water.
If the Kb of a weak base is 5.4 × 10-6, what is the pH of...

If the Kb of a weak base is 5.4 × 10-6, what is the pH of a 0.25 M solution of this base? If the Kb of a weak base is 5.4 x 106, what is the pH of a 0.25 M solution of this base? Number
What is the pH of the following solutions

What is the pH of the following solutions? 1)a solution that is 5.4?10−2 M in HClO4 and 3.0?10−2 M in HCl 2)a solution that is 1.80% HCl by mass (Assume a density of 1.01g/mL for the solution.) Please help! I am so confused!

Activity #2 Calculate the pH of the following basic solutions. 1. Calculate the pH and pOH...

Activity #2 Calculate the pH of the following basic solutions. 1. Calculate the pH and pOH of a 0.200 M Ca(OH)2 2. Calculate the equilibrium concentrations for [OH-], [HB+), and [B], the pH and pOH for a 0.200 M pyridine solution. (CsH5N) Kb = 1.4 X 10-9 3. Calculate the equilibrium concentrations for [OH-], [HB], and [B], the pH and pOH for a 0.200 M methylamine. (CH3NH2) Kb = 4.4 X 10-4 4. Calculate the equilibrium concentrations for [OH-], [HB+],...
Determine the pH of water solutions with the following characteristics. Classify each solution as acidic, basic,...

Determine the pH of water solutions with the following characteristics. Classify each solution as acidic, basic, or neutral. H+) -5.2 x 10-M pH = The solution is b ) = 5.3 x 10-12 M pH = The solution is OH") -5.2 x 10 M pH = The solution is a OH") = 5.3 x 10-40 M pH = The solution is
Determine the pH of water solutions with the following characteristics. Classify each solution as acidic, basic,...

Determine the pH of water solutions with the following characteristics. Classify each solution as acidic, basic, or neutral. a H) = 2.5 x 10-'M pH = The solution is b(OH) = 2.5 x 10-M pH = The solution is [OH-] = [H] PH = The solution is a [] =2.5 x 10-2M pH = The solution is

If the K_b of a weak base is 2.2 times 10^-6, what is the pH of...

If the K_b of a weak base is 2.2 times 10^-6, what is the pH of a 0.31 M solution of this base? pH =