Purchase Solution

Solving for the pH of NH3

Not what you're looking for?

Ask Custom Question

You have a 0.1 M aqueous solution of NH3 to which you add an equal volume of 0.1 M AgNO3. The Kb is 1.80 x 10-5 and the K formation for [Ag(NH3)2]+ is 1.69 x 10 to the 7th. What is the pH of the original NH3 solution and what is the pH after the addition of AgNO3?

Purchase this Solution
Solution Summary

Solving for the pH of NH3 after a reaction with AgNO3 is provided.

Solution Preview

Please see the attached files.

You have a 0.1 M aqueous solution of NH3 to which you add an equal volume of 0.1 M AgNO3. The Kb is 1.80 x 10-5 and the K formation for [Ag(NH3)2]+ is 1.69 x 107.

What is the pH of the original NH3 solution and what is the pH after the addition of AgNO3?

Original solution is a ...

Purchase this Solution
Free BrainMass Quizzes
Match Elements with their Symbols

Elements are provided: choose the matching one- or two-letter symbol for each element.

General Chemistry - Classification of Matter

This test will assess your knowledge on the classification of matter which includes elements, compounds and mixtures.

Organic Chemistry Naming: Alkanes

This is a quiz which is designed to assist students with learning the nomenclature used to identify organic compounds. This quiz focuses on the organic compounds called Alkanes.

Functional groups in Organic Chemistry

You will be tested on the names of functional groups in Organic Chemistry. It is very important to know the functional groups to understand Organic reactions.

Periodic table

View More Free Quizzes
Related BrainMass Solutions

  • Volume of an acid required to change the pH of a buffer solution

    (Kb for ammonia 1.80e-5) 1.80 x10^-5 The equation to calculate the pH of a buffer solution is: pH = pKa - log [HA]/[A-] The most important thing here is to recognize what our buffer system is.

  • Buffer cacluation without Hasselbach

    The professor uses a pH meter and finds the solution given to him has a pH of 0.96 a) Find the H+ in the solution b) Find the Ka (Ionization constant) Question #2 A student mixes 3.0 mL of 0.20 M NH3 (aq) with 70.0 mL of 0.30 M NH4CL(aq).

  • Buffer Solution and Henderson-Hasselbalch (H-H)

    What is the pH of a solution prepared by mixing 50.00mL of 0.10 M NH3 with 25.00mL of 0.10 M NH4Cl? Assume that the volume of the solutions are additive and that Kb= 1.8 x 10 -5 for NH3. 14.

  • Determine the pH of a 1.0 L of the buffer that is 0.50 M in NH3 and 0.20 M in NH4Cl after the addition of 0.010 mol of NaOH.

    492957 Determining the pH of the Buffer Determine the pH of a 1.0 L of the buffer that is 0.50 M in NH3 and 0.20 M in NH4Cl after the addition of 0.010 mol of NaOH. Kb = 1.8 x 10^(-5) for NH3. The calculation should be in two parts.

  • Buffer NH3 and NH4Cl

    39969 Buffer NH3 and NH4Cl I am really having problems with this problem: Calculate the pH of the 0.20 M NH3 and 0.15 NH4Cl buffer. What is the pH of the buffer after the addition of 10.0 mL of 0.10 M HCl to 57.5 mL of the buffer.

  • pH of an Aqueous Solution That Contains NH3 and (NH4)2SO4

    91296 pH of an Aqueous Solution That Contains NH3 and (NH4)2SO4 What is the pH of an aqueous solution that contains 0.15M NH3 and 0.05M (NH4)2SO4? The Kb for NH3 is 1.8 x 10-5.

  • A study of pH - lab related

    Write the equation for the reaction between ammonia and hydrochloric acid. Calculate the pH of the solution after adding 4.00 mL of HCl. 3. Calculate the total volume of the solution at equivalence point. 4.

  • Acid-Base Reaction Problem

    We have pH so we have [H] in the above we also have [NH2] so all we have to solve for is [NH3] [NH3]= [H][NH2]/pKa= (10^(-4.2))(o.50)/(10^(-4.63)) [NH3] = 1.34577 M you can substitute this value back into the equation for pKa and see it yields

  • PH of a buffer system

    302647 PH of a buffer system (a) Calculate the pH of the 0.20 M NH3/0.18 M NH4Cl buffer.

View More Related Solutions