Question
In: Chemistry
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)?
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
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.
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
as a weak acid. What is the pH of a solution that is 0.027 M in
NH4Cl at 25 °C?
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
as a weak acid. What is the pH of a solution that is 0.038 M in
NH4Cl at 25 °C?
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
as a weak acid. What is the pH of a solution that is 0.034 M in
NH4Cl at 25 °C?
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
as a weak acid. What is the pH of a solution that is 0.040 M in
NH4Cl at 25 °C?
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