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)?

Expert Solution

queen_honey_blossom answered 2 years 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.

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.

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

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

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.*

Take 12.5 mL of 0.200 moles of aqueous Ammonia (NH3), whose Kb = 1.8 x 10-5,...

Take 12.5 mL of 0.200 moles of aqueous Ammonia (NH3), whose Kb = 1.8 x 10-5, and Titrate with 0.100 mol HCl, calculate PH at 5 mL HCl, 10 mL , 15 mL, 20 mL, 24.5mL, 25mL, 25.5mL, 30mL 40.0 mL, abd 50 mL HCl. Graph the solution with hoizontal axis being the PH up to 14 and The y-axis being mL HCl.

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

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

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

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

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

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Take 12.5 mL of 0.200 moles of aqueous Ammonia (NH3), whose Kb = 1.8 x 10-5,...

NH3 is a weak base (Kb = 1.8 × 10–5) and so the salt NH4Cl acts...

NH3 is a weak base (Kb = 1.8 × 10–5) and so the salt NH4Cl acts...

NH3 is a weak base (Kb = 1.8 × 10–5) and so the salt NH4Cl acts...

NH3 is a weak base (Kb = 1.8 × 10–5) and so the salt NH4Cl acts...