A buffered solution contains 0.25 M NH3 (Kb = 1.8 x 10-5 ) and 0.40 M...

A buffered solution contains 0.25 M NH3 (Kb = 1.8 x 10-5 ) and 0.40 M NH4Cl.

a. Calculate the pH of this solution.

b. Calculate the pH of the solution that results when 0.20 mole of gaseous HCl is added to 1.0 L of the buffered solution from part a

Expert Solution

queen_honey_blossom answered 1 year ago

A buffer solution contains 1.00 M NH3 (Kb = 1.8  10-5 ) and 2.00 M...

A buffer solution contains 1.00 M NH3 (Kb = 1.8  10-5 ) and 2.00 M NH4Cl. (a) Write the net ionic equations to show how this buffer solution neutralizes the added H + and OH- . (b) Calculate the pH of this buffer solution.

In a titration of a 250mL solution of 0.05M ammonia (NH3) (Kb=1.8 * 10^-5) with a...

In a titration of a 250mL solution of 0.05M ammonia (NH3) (Kb=1.8 * 10^-5) with a concentrated (0.2M) solution of HCL, calculate the following: 1. What is the initial pH before adding HCL? 2. What is the pH of the system after adding 20mL of the 0.2 M HCL? 3. What is the pH at equivalence? *I have the answers, I really need to know how to do the work to get to the answers.*

Consider the titration of 60.0 mL of 0.100 M NH3 Kb= 1.8 x 10^-5 with 0.150...

Consider the titration of 60.0 mL of 0.100 M NH3 Kb= 1.8 x 10^-5 with 0.150 M HCl. Calculate the pH after the following volumes of titrant have been added: 40.5 mL & 60.0 mL

Calculate the pH of a 0.50 M NH4Cl solution (for NH3, Kb = 1.8 x 10-5). Write the net ionic equation for the reaction.

General Chemistry Calculate the pH of a 0.50 M NH4Cl solution (for NH3, Kb = 1.8 x 10-5). Write the net ionic equation for the reaction.

Calculate the [OH-] and pH of a 0.01 M solution of ammonia (Kb= 1.8 x 10^-5)

A buffer is made by combining 5.55 g of NH3 (Kb = 1.8 X 10-5) with...

A buffer is made by combining 5.55 g of NH3 (Kb = 1.8 X 10-5) with 4.78 g of HCl and diluting to a volume of 750.0 mL. a. What is the pH? b. What is the pH after adding 60.0 mL of 2.00 M HBr(aq)? c. What is the pH after adding 120.0 mL of 2.00 M HBr(aq)?

Given that Ka for HCN is 4.9×10−10 and Kb for NH3 is 1.8×10−5 , calculate Kb...

Given that Ka for HCN is 4.9×10−10 and Kb for NH3 is 1.8×10−5 , calculate Kb for CN− and Ka for NH4+ . Enter the Kb value for CN− followed by the Ka value for NH4+ , separated by a comma, using two significant figures.

Part A: A 75.0-mL volume of 0.200 M NH3 (Kb=1.8×10−5 ) is titrated with 0.500 M...

Part A: A 75.0-mL volume of 0.200 M NH3 (Kb=1.8×10−5 ) is titrated with 0.500 M HNO3 . Calculate the pH after the addition of 28.0 mL of HNO3 . Part B: A 52.0-mL volume of 0.35 M CH3COOH (Ka=1.8×10−5 ) is titrated with 0.40 M NaOH . Calculate the pH after the addition of 33.0 mL of NaOH . Please Explain Steps

Part C Consider the titration of 50.0 mL of 0.20 M NH3 (Kb=1.8×10−5) with 0.20 M...

Part C Consider the titration of 50.0 mL of 0.20 M NH3 (Kb=1.8×10−5) with 0.20 M HNO3. Calculate the pH after addition of 50.0 mL of the titrant at 25 ∘C. Part D A 30.0-mL volume of 0.50 M CH3COOH (Ka=1.8×10−5) was titrated with 0.50 M NaOH. Calculate the pH after addition of 30.0 mL of NaOH at 25 ∘C.

A 35.0 mL sample of 0.150 M ammonia (NH3, Kb=1.8×10−5) is titrated with 0.150 M HNO3....

A 35.0 mL sample of 0.150 M ammonia (NH3, Kb=1.8×10−5) is titrated with 0.150 M HNO3. Calculate the pH after the addition of each of the following volumes of acid. Express your answer using two decimal places. A. 0.0 mL B. 17.5 mL C. 35.0 mL D. 80.0 mL

Question