Question

Ammonia, NH3, is a weak base with a *K*b 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.

Answer #1

A)

Lets write the dissociation equation of NH3

NH3 +H2O -----> NH4+ + OH-

0.48 0 0

0.48-x x x

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

Kb = x*x/(c-x)

Assuming small x approximation, that is lets assume that x can be ignored as compared to c

So, above expression becomes

Kb = x*x/(c)

so, x = sqrt (Kb*c)

x = sqrt ((1.8*10^-5)*0.48) = 2.939*10^-3

since c is much greater than x, our assumption is correct

so, x = 2.939*10^-3 M

So, [OH-] = x = 2.939*10^-3 M

we have below equation to be used:

pOH = -log [OH-]

= -log (2.939*10^-3)

= 2.53

we have below equation to be used:

PH = 14 - pOH

= 14 - 2.53

= 11.47

Answer: 11.47

B)

% dissociation = (x*100)/c

= 2.939*10^-3*100/0.48

= 0.6124 %

Answer: 0.612 %

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.
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.

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?

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
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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

Ammonia, NH3, is a weak base with a Kb value of 1.8×10−5. What
is the percent ionization of a 0.175 M ammonia solution?

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....

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

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...

Part A What is the pH of a 0.270 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.

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