Question

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.

Answer #1

(735 Torr)(7.50 Litres) = n (62.4 Torr-Litres/mol-K)(295 K)

0.29946 moles of NH3

find moles

0.450L solution of 0.400 M HCL = 0.180 moles of HCl

0.29946 moles of NH3 reacts with 0.180 moles of HCl producing 0.160
moles of NH4+ ion,

and leaving 0.1435 moles of NH3 behind

find molarities

0.160 moles of NH4+ / 0.400 L = 0.400 M NH4+

0.1435 moles of NH3 / 0.400 L = 0.359 M NH3

NH4OH --> NH4+ & OH-

Kb = [ NH4+] [OH-] / [NH4OH]

1.8 e-5 = [ 0.400] [OH-] / [ 0.359]

[OH-] = 1.61 e-5

pOH = 4.79

pH = 9.21

your answer is

pH = 9.21

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 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.

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 7.70 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.

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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.____________

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
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NH3 is titrated with 0.20 M HCl. What is the pH
of the solution after 15.00 mL of acid have been added to the
ammonia solution? (NH3 has Kb = 1.8
x 10–5)
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chloride is 1.6 x 10–10. (a) Calculate
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NaCl to 1.0 L of water; calculate the molar solubility of AgCl in
this salt water.

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0.400 M solution of ammonia, NH3, to prepare a buffer solution that
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with the appropriate units.

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impure NaOH requires 17.1 mL of 0.2370 M HCl for neutralization.
What is the percent of NaOH in the sample, by weight?_____% NaOH In
an acid-base titration, 20.54 mL of H2SO4 were used to neutralize
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A 50.0 mL sample of 0.150 M ammonia (NH3, Kb=1.8×10−5) is
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A. 0.0 mL
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C. 50.0 mL

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200.0 mL aliquot of this solution was added 10.0 mL of 10.0 M
sodium hydroxide. What was the resulting pH? Please show full work
with explanation. Thank you.

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