Question

Equal volumes of 0.1 M NH3 (Kb= 1.8x10^-5) and 0.1 M HCN (Ka= 4.9x10^-10) are mixed...

Equal volumes of 0.1 M NH3 (Kb= 1.8x10^-5) and 0.1 M HCN (Ka= 4.9x10^-10) are mixed together. will the resulting solution be acidic, basic, or neutral? PLEASE SHOW WORK

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

NH4CN is the salt made up of weak acid(HCN) and weak base(NH3)

NH3 + HCN -- NH4CN

Salts of this kind can be neutral, acidic, or basic depending upon the

strength of the acid and base

strength of the acid and base

Expression for calculating the pH of salts of weak acids and weak bases

Expression for calculating the pH of salts of weak acids and weak bases

is as follows: pH = 7 + 1/2 — (pKa —pKb)

Ka of acid (HCN) = Kw/Kb = 49x10-10

pKa of acid = -log Ka

= -log (4.9 x 10-10)

= 9.31

Kb of base (NH3) -

pkb of base (NH3) -

- 10-5)

pH = 7+ 1/2

= 9.285

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
1) Kb for NH3 is 1.8x10^-5. What is the pOH of a .20M aqueous solution of...
1) Kb for NH3 is 1.8x10^-5. What is the pOH of a .20M aqueous solution of NH4Cl at 25 degrees Celsius? (Please show work) 2) Determine the pH of a 0.15 M aqueous solution of KF. For hydrofluoric acid, Ka=7.0x10^-4. (Please show work) 3) An aqueous solution of _____ will produce a neutral solution. A) NaNO2 B) LiNO3 C) KF D) Rb2CO3 E) NH4NO3
When equal volumes of 1.0 M solutions of barium hydroxide and hydrochloric acid are mixed, and...
When equal volumes of 1.0 M solutions of barium hydroxide and hydrochloric acid are mixed, and the reaction goes to completion, the resulting solution would be acidic, basic or neutral
#1 Given that at 25.0 ∘C Ka for HCN is 4.9×10−10 and Kb for NH3 is...
#1 Given that at 25.0 ∘C Ka for HCN is 4.9×10−10 and Kb for NH3 is 1.8×10−5, calculate Kb for CN− and Ka for NH4+. Enter the Kb value for CN− followed by the Ka value for NH4+, separated by a comma, using two significant figures. #2 Find the pH of a 0.250 M solution of NaC2H3O2. (The Ka value of HC2H3O2 is 1.80×10−5).
#1 Given that at 25.0 ∘C Ka for HCN is 4.9×10−10 and Kb for NH3 is...
#1 Given that at 25.0 ∘C Ka for HCN is 4.9×10−10 and Kb for NH3 is 1.8×10−5, calculate Kb for CN− and Ka for NH4+. Enter the Kb value for CN− followed by the Ka value for NH4+, separated by a comma, using two significant figures. #2 Find the pH of a 0.250 M solution of NaC2H3O2. (The Ka value of HC2H3O2 is 1.80×10−5).
Calculate the pH of a 0.1 M NaCN solution. Ka of HCN = 6.2 x10 -10....
Calculate the pH of a 0.1 M NaCN solution. Ka of HCN = 6.2 x10 -10. Please explain and/or show work.
Equal volumes of 0.190 M weak base (Kb = 2.0× 10–9) and 0.190 M HCl are...
Equal volumes of 0.190 M weak base (Kb = 2.0× 10–9) and 0.190 M HCl are mixed. Calculate the pH of the resulting solution.
Equal volumes of 0.120 M weak base (Kb = 5.0× 10–9) and 0.120 M HCl are...
Equal volumes of 0.120 M weak base (Kb = 5.0× 10–9) and 0.120 M HCl are mixed. Calculate the pH of the resulting solution.
calculate the pH of the following solution: 0.10 M NH3 with KB=1.8x10^-5
calculate the pH of the following solution: 0.10 M NH3 with KB=1.8x10^-5
Equal volumes of 0.030 M NH3 and 0.0150 M HCl are mixed together. What are the...
Equal volumes of 0.030 M NH3 and 0.0150 M HCl are mixed together. What are the concentrations of NH3 and NH4+ in the reaction? NH3 (aq) + H+ (aq) --> NH4+ (aq)
HNO2 ( Ka=4.5 x 10^-4) HCN (Ka= 4.9 x 10^-10) CH3NH2 (Kb=4.4 x 10^-4) HONH2 (Kb=1.1...
HNO2 ( Ka=4.5 x 10^-4) HCN (Ka= 4.9 x 10^-10) CH3NH2 (Kb=4.4 x 10^-4) HONH2 (Kb=1.1 x 10^-8) Use this data to rank the following solutions in order of increasing pH. In other words, select a '1' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on.. RANK THESE ONES: 0.1 M NaBr 0.1 M CH3NH3Cl 0.1 M KNO2 0.1 M HONH3Br
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT