Question

Addition of a small amount of an aqueous solution of sodium hydroxide to an aqueous solution...

Addition of a small amount of an aqueous solution of sodium hydroxide to an aqueous solution of ammonia will (please give explanation)

A.increase both the pH and Kb of ammonia.
B.increase the pH but will not affect Kb of ammonia.
C.decrease both the pH and Kb of ammonia.
D.decrease the pH but will not affect Kb of ammonia.
E.decrease the pH but will increase Kb of ammonia.


Homework Answers

Answer #1

answer : D.decrease the pH but will not affect Kb of ammonia.

NH4OH ------------------------> NH4+ + OH-

NaOH---------------------------> Na+    + OH-

due to common ion OH- the degree of dissociation of ammonia solution decreases. so OH- ion concentration decrease . pOH value increases so pH decreases

POH = -log[OH-]

[OH-] decreases pOH increases

pH + pOH = 14

pH = 14- pOH

pOH increases pH decreases

NH3 is weak base . on addition of strong base NaOH , the pH of resulting solution will be decreased. because strong base NaOH .

Kb of NH3 = 1.8 x 10^-5. the ammonia Kb value doesn't effect by strong base or strong acid . it is equilibrium constant.equilibrium constant value only depends on temperature . so Kb value depends on temperature.

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
What is the change in pH after addition of 10.0 mL of 1.0 M sodium hydroxide...
What is the change in pH after addition of 10.0 mL of 1.0 M sodium hydroxide to 90.0 mL of a 1.0 M NH3/1.0 M NH4+ buffer? [Kb for ammonia is 1.8 x 10-5]
A precipitate forms when a small amount of sodium hydroxide is added to a solution of...
A precipitate forms when a small amount of sodium hydroxide is added to a solution of aluminum sulfate. This precipitate dissolves when more sodium hydroxide is added. Explain what is happening.
The molarity of an aqueous solution of sodium hydroxide ( NaOH ) is determined by titration...
The molarity of an aqueous solution of sodium hydroxide ( NaOH ) is determined by titration against a 0.132 M nitric acid ( HNO3 ) solution. If 31.9 mL of the base are required to neutralize 29.2 mL of nitric acid , what is the molarity of the sodium hydroxide solution? Give your answer to three significant figures.
A 0.500M solution of Hcl is titrated with a 0.250M aqueous solution of sodium hydroxide. The...
A 0.500M solution of Hcl is titrated with a 0.250M aqueous solution of sodium hydroxide. The neutralization of hydrochloride acid with sodium hydroxide produces an aqueous solution of sodium chloride at the equivalence point. What is the concentration of sodium chloride at the equivalence point? Options a 0.500M b 0.250 M c. 0.375M d. 0.750M e 1.000M
   The addition of 0.010 moles of sodium hydroxide to a 1.0 L solution of a...
   The addition of 0.010 moles of sodium hydroxide to a 1.0 L solution of a buffer which is 1.0 M in acetic acid and 1.0 M in sodium acetate would shift the pH from 4.74 to _________.                 A buffer ceases to function in pH regulation once one of the components is ___________.                 The addition of a strong acid/base to a buffer system produces a situation where [H3O+] has changed, and so ___________.                 The amount of strong...
When an excess of sodium hydroxide is added to an aqueous solution of ammonium chloride, gaseous...
When an excess of sodium hydroxide is added to an aqueous solution of ammonium chloride, gaseous ammonia is produced: NaOH(aq) + NH4Cl(aq) → NaCl(aq) + NH3(g) + H2O(ℓ) Suppose 3.68 g ammonium chloride reacts in this way at 30°C and a total pressure of 0.9884 atm. At this temperature, the vapor pressure of water is 0.0419 atm. Calculate the volume of ammonia saturated with water vapor that will be produced under these conditions, assuming no leaks or other losses of...
An aqueous solution containing 0.2M of sodium hydroxide is allowed to equilibrate with the atmosphere in...
An aqueous solution containing 0.2M of sodium hydroxide is allowed to equilibrate with the atmosphere in an analytical laboratory where the temperature is kept at 25°C. The partial pressure of carbon dioxide in the atmosphere, PCO2, is10-3.5 atm, and the Henry’s Law constant for carbon dioxide KH = 10-1.5 mol.L/atm. Determine the pH and the total acid concentration, CT,CO3, of the solution when equilibrium with the atmosphere is reached. How do you expect the concentration CT,CO3 to vary with the...
Calculate the pH of a solution of   0.51 M aqueous ammonia and 0.48M ammonium nitrate before...
Calculate the pH of a solution of   0.51 M aqueous ammonia and 0.48M ammonium nitrate before and after 0.090 M NaOH is added to the solution.        Kb of ammonia = 1.7 x 10 -5 Please Use ICE Method
A.) A 1 liter solution contains 0.343 M acetic acid and 0.457 M sodium acetate. Addition...
A.) A 1 liter solution contains 0.343 M acetic acid and 0.457 M sodium acetate. Addition of 0.377 moles of calcium hydroxide will: (Assume that the volume does not change upon the addition of calcium hydroxide.) Raise the pH slightly Lower the pH slightly Raise the pH by several units Lower the pH by several units Not change the pH Exceed the buffer capacity B.) A 1 liter solution contains 0.340 M hydrocyanic acid and 0.453 M sodium cyanide. Addition...
1. An aqueous solution of barium hydroxide is standardized by titration with a 0.197 M solution...
1. An aqueous solution of barium hydroxide is standardized by titration with a 0.197 M solution of hydrobromic acid. If 10.4 mL of base are required to neutralize 22.7 mL of the acid, what is the molarity of the barium hydroxide solution? M barium hydroxide b.An aqueous solution of hydrochloric acid is standardized by titration with a 0.176 M solution of barium hydroxide. If 13.7 mL of base are required to neutralize 14.1 mL of the acid, what is the...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT