Question

A sample of 7.60 L of NH3 (ammonia) gas at 22 ∘C and 735 torr is
bubbled into a 0.450 L solution of 0.400 *M* HCl
(hydrochloric acid).

The *K*b value for NH3 is 1.8×10−5.

Assuming all the NH3 dissolves and that the volume of the solution remains at 0.450 L , calculate the pH of the resulting solution. Express your answer numerically to two decimal places.

Answer #1

**poH of basic buffer = pkb+ log(NH4+/NH3)**

**pkb of NH3 = -log(1.8*10^-5) = 4.75**

** no of mol of HCl taken = 0.45*0.4 = 0.18
mol**

** no of mol of NH4Cl = 0.18
mol**

** no of mol of NH3 taken = PV/RT**

**
= ((735/760)*7.6)/(0.0821*295)**

**
= 0.303 mol**

**no of mol of NH3 unreacted = 0.303-0.18 = 0.123
mol**

**
pOH = 4.75 + log(0.18/0.123)**

** = 4.915**

**pH = 14-4.915 = 9.085**

**answer: 9.08**

A sample of 7.80 L of NH3 (ammonia) gas at 22 ∘C and 735 torr is
bubbled into a 0.450 L solution of 0.400 M HCl (hydrochloric acid).
The Kb value for NH3 is 1.8×10−5.
Assuming all the NH3 dissolves and that the volume of the
solution remains at 0.450 L , calculate the pH of the resulting
solution.
Express your answer numerically to two decimal places.
Thanks!

A sample of 7.50 L of NH3 (ammonia) gas at 22 ∘C and 735 torr is
bubbled into a 0.450 L solution of 0.400 M HCl (hydrochloric acid).
The Kb value for NH3 is 1.8×10−5.
Assuming all the NH3 dissolves and that the volume of the
solution remains at 0.450 L , calculate the pH of the resulting
solution.

A sample of 7.70 L of NH3 (ammonia) gas at 22 ∘C and 735 torr is
bubbled into a 0.350 L solution of 0.400 M HCl
(hydrochloric acid).
The Kb value for NH3 is 1.8×10−5.
Part A:
Assuming all the NH3 dissolves and that the volume of the
solution remains at 0.350 L , calculate the pH of the resulting
solution.

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.
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.

How many grams of dry NH4Cl need to be added to 1.80 L of a
0.400 M solution of ammonia, NH3, to prepare a buffer solution that
has a pH of 8.60? Kb for ammonia is 1.8×10−5. Express your answer
with the appropriate units.

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

How many grams of dry NH4Cl need to be added to 2.50 L of a
0.700 M solution of ammonia, NH3, to prepare a buffer
solution that has a pH of 8.56? Kb for ammonia is
1.8×10−5.
Express your answer numerically in grams to three significant
figures.

An 80.0 mL sample of 0.200 M ammonia is titrated with 0.100M
hydrochloric acid. Kb for ammonia is 1.8 x 10-5. Calculate the pH
of the solution at each of the following points of the titration:
a. before the addition of any HCl. ______________ b. halfway to the
equivalence point.______________ c. at the equivalence
point._________________ d. after the addition of 175 mL of 0.100M
HCl.____________

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