Question

In: Chemistry

1. A.write a chemical equation which goes with the statement: i) Kb= 4.3 X 10-10 for...

1.

A.write a chemical equation which goes with the statement:

i) Kb= 4.3 X 10-10 for aniline (C6H5NH2)

ii)Kb = 2.1 X 10-4 for carbonate ion

B. Kb =1.3 X 10-3 for C5H11N and kb= 6.3 x 10-5 for N(CH3)3

i) Which base is the stronger base in water

ii) For the same solute concentration, which base has the larger equilibrium OH- concentrations?How did you decide?

C. Reaction of amide ion (NH2-), ethoxide ion (OCH2CH3-), methoxide ion (OCH3-), hydride ion (H-), or oxide ion (O2-) with water gives hydroxide ion as one product , for each ion, the reaction goes to completion.

i) For each of these ions write a net ionic equation for the reaction of the ions with water.

ii) is a salt supplying one of these ions a strong base or a weak acid?Explain.

Solutions

Expert Solution

1.

A.)

i) Kb= 4.3 X 10-10 for aniline (C6H5NH2)

C6H5NH2 + H2O ------------------------> C6H5NH3+   + OH-

ii)Kb = 2.1 X 10-4 for carbonate ion

CO3-2 + H2O ----------------------> HCO3- + OH-

B. Kb =1.3 X 10-3 for C5H11N and kb= 6.3 x 10-5 for N(CH3)3

C5H11N + H2O -------------------> C5H11NH+ + OH-

(CH3)3N + H2O --------------------> (CH3)3NH+   + OH-

i) Which base is the stronger base in water

C5H11N stronger base in water because its Kb value is nore than (CH3)3N

ii) For the same solute concentration, which base has the larger equilibrium OH- concentrations?

C5H11N has larger equilibrium OH- concentration because it gives more OH- ions , since it has larger Kb value

C. Reaction of amide ion (NH2-), ethoxide ion (OCH2CH3-), methoxide ion (OCH3-), hydride ion (H-), or oxide ion (O2-) with water gives hydroxide ion as one product , for each ion, the reaction goes to completion.

i) For each of these ions write a net ionic equation for the reaction of the ions with water.

NH2- + H2O -------------------> NH3 + OH-

CH3CH2O- + H2O ------------------> CH3CH2OH + OH-

CH3O- + H2O ------------------------> CH3OH + OH-

H- + H2O -----------------> 2OH-

O-2 + H2O -------------> 2OH-

ii) is a salt supplying one of these ions a strong base or a weak acid?Explain.

these are supplied by weak acid. becuase these are all strong conjugate and these salts are storng base

note : all bolded are answers


Related Solutions

If the Kb of aniline is 4.3 x 10-10, calculate the pH when 10.5 g of...
If the Kb of aniline is 4.3 x 10-10, calculate the pH when 10.5 g of aniline is dissolved in 120 mL of water. Select one: a. 9.3 b. 12.8 c. 14.0 d. 2.9
a. Calculate the pH of a 0.538 M aqueous solution of ethylamine (C2H5NH2, Kb = 4.3×10-4)...
a. Calculate the pH of a 0.538 M aqueous solution of ethylamine (C2H5NH2, Kb = 4.3×10-4) b. Calculate the pH of a 0.0473 M aqueous solution of piperidine (C5H11N, Kb = 1.3×10-3).
Find the equation of the line goes through (1,0,-1) that is perpendicular to the lines x...
Find the equation of the line goes through (1,0,-1) that is perpendicular to the lines x = 3+2t,y = 3t,z = −4t and x = t,y = t,z = −t. Write it in parametric and the vector equation form.
1) BOH is a weak Base. Kb = 2 x 10^-5. The pH of a 0.1M...
1) BOH is a weak Base. Kb = 2 x 10^-5. The pH of a 0.1M solution is? 2) A 0.1M solution of BCl is prepared. Kb for BOH is 6 x 10-6 . What is the solution’s pH?
1. Calculate the pH of: A) 0.10 M ammonia (kb = 1.7 x 10 -5) ....
1. Calculate the pH of: A) 0.10 M ammonia (kb = 1.7 x 10 -5) . B) 0.15 M ammonium iodide (ka = 1.8 x 10 -5) . C) pure water D) 0.15 M hydrogen fluoride (ka = 4.2 x 10 -5) . E) 0.25 M hydrochloric acid. F) 0.15 M calcium hydroxide.
The decomposition of N2O5 occurs with a rate constant of 4.3 x 10–3 sec–1 at 65C...
The decomposition of N2O5 occurs with a rate constant of 4.3 x 10–3 sec–1 at 65C and 3.0 x 10–5 sec–1 at 25C. What is the activation energy of the process?
The Ka of HC3H3O2  is 5.6 x 10-5 and the Kb of (CH3)3N is 6.4 x 10-5...
The Ka of HC3H3O2  is 5.6 x 10-5 and the Kb of (CH3)3N is 6.4 x 10-5 With the titration of 20.0mL of 0.40M HC3H3O2, what is the pH of the solution after adding a total of 40.0mL of 0.20M NaOH to the acid? A) 8.69 B) 8.93 C)7.00 D) 12.90 E) None of these
1. Write the chemical equation for the formation of KCl (s) 2. Write the chemical equation...
1. Write the chemical equation for the formation of KCl (s) 2. Write the chemical equation describing the lattice energy for KCl (s)
1) Write a chemical equation describing the condensation process for N2 and a chemical equation describing...
1) Write a chemical equation describing the condensation process for N2 and a chemical equation describing the freezing process for N2. For each process discuss the change in enthalpy and entropy that occurs. For each process describe the conditions (in terms of temperature) that support a thermodynamically favorable change, and the conditions that do not support a thermodynamically favorable change.
Calculate the pH of a 0.50 M NH4Cl solution (for NH3, Kb = 1.8 x 10-5). Write the net ionic equation for the reaction.
General Chemistry Calculate the pH of a 0.50 M NH4Cl solution (for NH3, Kb = 1.8 x 10-5). Write the net ionic equation for the reaction.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT