0.010 M NH4OH (1.0%)

Question

Question

science chemistry

Answer 1

Answer #1

Degree of dissociation(x) = 1/100 = 0.01

C = concentration of NH4OH = 0.01 M

NH4OH - WEAK base

[OH-] = CX

= 0.01*0.01

= 1*10^-4 M

pOH = -log(OH-)

= -log(1*10^-4)

= 4

pH = 14-pOH

= 14-4 = 10

[H3O+] = 10^-10

Add a comment

Answer 2

Similar Homework Help Questions

From 1.0 M NH4OH and 1.0 M NH4Cl reagent stock solutions prepare 100 mL of the...

From 1.0 M NH4OH and 1.0 M NH4Cl reagent stock solutions prepare 100 mL of the solutions described in the table and complete the table. Volume NH3 Volume NH4+ Solução [NH3]/[NH4+][NH3] + [NH4+] 1:1 0,10 1:1 0,20 1:10 0,20 10:1 0,20
From 1.0 M NH4OH and 1.0 M NH4Cl reagent stock solutions prepare 100 mL of the...

From 1.0 M NH4OH and 1.0 M NH4Cl reagent stock solutions prepare 100 mL of the solutions described in the table and complete the table. *STEP BY STEP* Volume NH3 | Volume NH4+ [NH3]/[NH4] [NH3] + [NH4] 1:1 0,10 1:1 0,20 0,20 1:10 10:1 0,20
2) A solid sphere of mass 1.0 kg and radius 0.010 m rolls with a speed...

2) A solid sphere of mass 1.0 kg and radius 0.010 m rolls with a speed of 10 m/s. How high up an inclined plane can it climb before coming to rest?

What is the minimum formation constant required to titrate 0.010 M Cd2 with 0.010 M EDTA,...

What is the minimum formation constant required to titrate 0.010 M Cd2 with 0.010 M EDTA, if the titration is followed by potentiometry? What is the minimum pH for titrating 0.010 M Cd2+ with 0.010 M EDTA?
A solution is 0.010 M in HCl and 0.010 M in NH4Cl. What is the molar...

A solution is 0.010 M in HCl and 0.010 M in NH4Cl. What is the molar concentration of NH3 at equilibrium? Kb(NH3) = 1.8 x 10-5 (Please explain the process in depth if possible)
You need to prepare 200 mL of a 0.4 M solution of ammonium hydroxide (NH4OH) You...

You need to prepare 200 mL of a 0.4 M solution of ammonium hydroxide (NH4OH) You have 80 mL of a 0.5 M NHOH solution and 40 mL of a 7.5% (w/v) NH4OH solution. What volume of 7.5% NHOH and water needs to be added to the 80 mL of 0.5 M NH4OH solution to make up 200 mL of 0.4 M NH4OH? Molar mass of NH4OH 35.04 g/mol % (weight / volume) means mass (in g) in volume (100...

For Mg(OH)2, Ksp = 6x 10-12 What will occur if 1.0 L of 0.010 M Mg(NO3),...

For Mg(OH)2, Ksp = 6x 10-12 What will occur if 1.0 L of 0.010 M Mg(NO3), is prepared at pH 10.00? Select one: a. Kp> . A precipitate will form. b. Q - Kp. No precipitate will form. c. Ko Q. No precipitate will form. d. Q> Kp. A precipitate will form. e. Q> Kg. No precipitate will form.
Prepare a series of 50 mL quinine standard solutions (10, 1.0, 0.10, 0.010, 0.0010μg/mL) by serial...

Prepare a series of 50 mL quinine standard solutions (10, 1.0, 0.10, 0.010, 0.0010μg/mL) by serial dilutionfrom the 100 μg/mL stock solution using0.05 M H2SO4as the diluent.
A solution contains 0.60 M NH4OH and 1.50 M NH4Cl. What is the maxiumum concentration of...

A solution contains 0.60 M NH4OH and 1.50 M NH4Cl. What is the maxiumum concentration of Mg2+ that can be present in such a solution without precipitating Mg(OH)2? (Ksp for Mg(OH)2 = 9.0 x 10^12; Kb fro NH4OH= 1.8 x 10^-5)

Solid NaI is slowly added to a solution that is 0.010 M in Cu+ and 0.010 M in Ag+.

Solid NaI is slowly added to a solution that is 0.010 M in Cu+ and 0.010 M in Ag+.(a) Which compound will begin to precipitate first?(b) Calculate [Ag+] when CuI just begins to precipitate.(c) What percent of Ag+ remains in solution at this point?