Question

THIS IS MY SECOND TIME POSTING THIS QUESTION. PLS MAKE SURE ANSWERS ARE CORRET

Ammonia, NH3, is a weak base with a Kb value of 1.8×10−5.

Part A What is the pH of a 0.490 M ammonia solution? Express your answer numerically to two decimal places.

Part B

What is the percent ionization of ammonia at this concentration?

Express your answer with the appropriate units

Answer #1

A)

the pH of [NH3] = 0.49 M should be calculated as follows:

NH3 + H2O <-> NH4++ OH-

Kb = [NH4+][OH-]/[NH3]

initially

[NH4+] = 0

[OH-] = 0

[NH3] = 0.49

in equilibrium

[NH4+] = +x

[OH-] = +x

[NH3] = 0.49 - x

substitute in Kb

Kb = [NH4+][OH-]/[NH3]

1.8*10^-5 = (x*x)/(0.49-x)

solve for x

x =[OH-] = 0.00296

pOH = -log(OH) = log(0.00296)

pOH = 2.5287

pH = 14-pOH = 14-2.5287

pH = 11.4713 --> 2 decimals --> 11.47

B)

Find % ionization of ammonia

% ioniazation = [NH4+] / [NH3]0 * 100%

substitute data

% ioniazation = 0.00296/0.49 * 100% = 0.6040816 % --> 0.6 %

Ammonia, NH3, is a weak base with a Kb value of
1.8×10−5.
Part A
What is the pH of a 0.490 M ammonia solution?
Express your answer numerically to two decimal places.
What is the percent ionization of ammonia at this
concentration?
Express your answer with the appropriate units.

Ammonia, NH3, is a weak base with a Kb value of
1.8×10−5.
Part A
What is the pH of a 0.480 M ammonia solution?
Express your answer numerically to two decimal places.
Part B
What is the percent ionization of ammonia at this
concentration?
Express your answer with the appropriate units.

Ammonia, NH3, is a weak base with a Kb value of
1.8×10−5.
A) What is the pH of a 0.280 M ammonia solution?
Express your answer numerically to two decimal places.
B) What is the percent ionization
of ammonia at this concentration?
Express your answer with the appropriate units.

QUESTION 22
± pH and Percent Ionization of a Weak Base
The degree to which a weak base dissociates is given by the
base-ionization constant, Kb. For the generic
weak base, B
B(aq)+H2O(l)⇌BH+(aq)+OH−(aq)
this constant is given by
Kb=[BH+][OH−][B]
Strong bases will have a higher Kb value. Similarly,
strong bases will have a higher percent ionization
value.
Percent ionization=[OH−] equilibrium[B] initial×100%
Strong bases, for which Kb is very large, ionize
completely (100%). For weak bases, the percent ionization changes
with...

The degree to which a weak base dissociates is given by the
base-ionization constant, Kb. For the generic
weak base, B
B(aq)+H2O(l)⇌BH+(aq)+OH−(aq)
this constant is given by
Kb=[BH+][OH−]/[B]
Strong bases will have a higher Kb value. Similarly,
strong bases will have a higher percent ionization
value.
Percent ionization=[OH−] equilibrium/[B] initial×100%
Strong bases, for which Kb is very large, ionize
completely (100%). For weak bases, the percent ionization changes
with concentration. The more dilute the solution, the greater the
percent ionization....

Ammonia, NH3, is a weak base with a Kb value of 1.8×10−5.What is
the pH of a 0.335 M ammonia solution?What is the percent ionization
of ammonia at this concentration?

Ammonia, NH3, is a weak base with a Kb value of
1.8×10−5.
A) What is the pH of a 0.340 M ammonia solution?
B)What is the percent ionization of ammonia at this
concentration?

PART A
Ammonia, NH3, is a weak base with a Kb value of
1.8×10−5 and a pH of 11.27. What is the percent ionization of
ammonia at this concentration?
PART B
Write a chemical equation for Sr(OH)2(aq)
showing how it is an acid or a base according to the Arrhenius
definition.
PART C
Find the pH of the following solutions of
mixtures of acid: 0.155 M in HNO2 and 8.5×10−2 M in
HNO3

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Part A What is the pH of a 0.270 M ammonia solution? Express
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Part B What is the percent ionization of ammonia at this
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