Question
In: Chemistry
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.
Solutions
Expert Solution
Given the mixture of basic buffer.
It is (NH3+ NH4Cl).Mixture of weak base and a salt containing its conjugate acid.
a) When an acid is added for example HCl,then it reacts with the base and the equation is as follows:
NH3 (aq) + HCl(aq) ----------------> NH4Cl(aq)
net ionic equation is: H3O+ (aq) + NH3 (aq) ---------------> H2O(l) + NH4+ (aq)
when a base is added, for example NaOH ,it reacts with the salt and the equtaion is as shown below:
NH4Cl (aq) + NaOH (aq) ------------> NaCl(aq) + H2O(l) + NH3 (aq)
net ionic equation is: NH4+ (aq) + OH- (aq) -------------> NH3 (aq) + H2O(l)
b) pH of a buffer solution can be obtained by using Handerson Hesselbalch equation.
pH = 14 - pOH
= 14 - [pKb + log[salt]/[base]]
= 14 - [-log (1.8x10^-5) + log (2/1)]
= 8.95
queen_honey_blossom answered 2 years agoRelated Solutions
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
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)?
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.*
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
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.
A 130.0 mL buffer solution is 0.110 M in NH3 and 0.135 M in NH4Br. (Kb...
A 130.0 mL buffer solution is 0.110 M in NH3 and 0.135 M in
NH4Br. (Kb of NH3 is 1.76×10−5.)
a.)What mass of HCl can this buffer neutralize before the pH
falls below 9.00?
b.)If the same volume of the buffer were 0.255 M in NH3 and
0.400 M in NH4Br, what mass of HCl could be handled before the pH
falls below 9.00?
A 130.0 mL buffer solution is 0.110 M in NH3 and 0.135 M in NH4Br. (Kb...
A 130.0 mL buffer solution is 0.110 M in NH3 and 0.135 M
in NH4Br. (Kb of NH3 is 1.76×10−5.)
a.)What mass of HCl can this buffer neutralize before the pH
falls below 9.00?
I already did this and got 0.101 g, which is right, but I am
struggling to answer Part B.
b.)If the same volume of the buffer were 0.255 M in NH3
and 0.400 M in NH4Br, what mass of HCl could be handled before the
pH...
A 130.0 mL buffer solution is 0.110 M in NH3 and 0.135 M in NH4Br. (Kb...
A 130.0 mL buffer solution is 0.110 M in NH3 and 0.135 M in
NH4Br. (Kb of NH3 is 1.76×10−5.)
If the same volume of the buffer were 0.255 M in NH3 and
0.400 M in NH4Br, what mass of HCl could be handled before the pH
falls below 9.00?
Please help me figure out the answer! I am on my last attempt. I
have entered the following answers and these are NOT correct:
0.0916, 0.0915, 0.094, 0.101, 0.999, 0.0999,...
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