What would happen if small amounts of 1M Ba(OH)2 were added to a solution of 1M...

What would happen if small amounts of 1M Ba(OH)2 were added to a solution of 1M NH3?

a. The base ionization constant for NH3 will go down

b. The base ionization constant for NH3 will go up

c. The percent ionization of NH3 will go down

d. The percent ionization of NH3 will go up

e. The percent ionization for NH3 will remain unchanged

Solutions

Expert Solution

NH3 is weak base.
The equilibrium reaction is:
NH3 + H2O <-> NH4+ + OH-

Adding small amount of string base is like adding OH- which is product in above equilibriujm/

So, the above equilibrium will shift to reactant side.

That is percent ionisation of NH3 will decrease.

Ionisation constant do not change as this is constant and deepen only on temperature.

Answer: c

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

What would happen if small amounts of 1M HNO3 were added to a solution of 1M...

What would happen if small amounts of 1M HNO3 were added to a solution of 1M HC2H3O2? a) The acid ionization constant for HC2H3O2 will go down. b) The percent ionization of HC2H3O2 will go down. c) The percent ionization for HC2H3O2 will remain unchanged d) The acid ionization constant for HC2H3O2 will go up. e) The percent ionization of HC2H3O2 will go up.

What would happen if small amounts of 1M HNO3 were added to a solution of 1M...

What would happen if small amounts of 1M HNO3 were added to a solution of 1M HC2H3O2? A: The percent ionization of HC2H3O2 will go down. B: The acid ionization constant for HC2H3O2 will go up. C: The percent ionization for HC2H3O2 will remain unchanged D: The percent ionization of HC2H3O2 will go up. E: The acid ionization constant for HC2H3O2 will go down.

Solution of Ba(OH)2 has pH=12.10. How many grams of Ba(OH)2 contain 250.0mL of solution?

You added 20 mL of 0.20M solution of Ba(OH)2(aq) to 50 mL of 0.10M solution of...

You added 20 mL of 0.20M solution of Ba(OH)2(aq) to 50 mL of 0.10M solution of HCl(aq). The pH of the resulting solution is ________.

75.0 mL of 0.250 M hydrochloric acid is added to 225.0 mL of 0.0550 M Ba(OH)2 solution. What is the concentration of Ba2+ ion left in solution?

75.0 mL of 0.250 M hydrochloric acid is added to 225.0 mL of 0.0550 M Ba(OH)2 solution. What is the concentration of Ba2+ ion left in solution? 75.0 mL of 0.250 M hydrochloric acid is added to 225.0 mL of 0.0550 M Ba(OH)2 solution. What is the concentration of Cl- ion left in solution?

1) The solubility of Cu(OH)2 would _____ if one added NaCN to the solution. A. Increase...

1) The solubility of Cu(OH)2 would _____ if one added NaCN to the solution. A. Increase or B. Decrease 2) AS the temperature increases chemical reactions tend to become more ______ controlled. A. Entropy or B. There is no temperature effect. 3) A cell where electricity is used to make the reaction run in a nonspontaneous direction is a ______ cell. A. Avogadro B. Electrolytic or C. Galvanic 4) Alkaline Batteries use this mtal in the anode. A. Iron B....

If I collect 14 grams of Ba(OH)2 and add it to water, what kind of solution...

If I collect 14 grams of Ba(OH)2 and add it to water, what kind of solution do you expect to be formed (acidic or basic)? Suppose that I make up a solution that is 750 ml using this barium salt and add it to my buret. I collect 6 grams of a solid material and titrate it against the barium, and I do this a total of 3 times. The volumes of barium containing solution used were: 22.9 ml, 24...

What is the pH of 0.005 M Ba(OH)2 solution? a) 12 b) 2 c) 0.005 d)...

What is the pH of 0.005 M Ba(OH)2 solution? a) 12 b) 2 c) 0.005 d) -2

Assuming complete dissociation, what is the pH of a 4.21 mg/L Ba(OH)2 solution? pH=

In a constant-pressure calorimeter, 60.0 mL of 0.330 M Ba(OH)2 was added to 60.0 mL of...

In a constant-pressure calorimeter, 60.0 mL of 0.330 M Ba(OH)2 was added to 60.0 mL of 0.660 M HCl. The reaction caused the temperature of the solution to rise from 21.42 °C to 25.92 °C. If the solution has the same density and specific heat as water (1.00 g/mL and 4.184 J/g·°C, respectively), what is ΔH for this reaction (per mole of H2O produced)? Assume that the total volume is the sum of the individual volumes.

Subjects