Consider a 300mL sample of 0.250M HCN (Ka=4.9x10^-10). To find the pH, do you need an...

Consider a 300mL sample of 0.250M HCN (Ka=4.9x10^-10). To find the pH, do you need an ice table, can you use the Henderson-Hasselbalch equation, or something else? If an ice table, will it be a Ka or Kb equilibrium? Can you use the small x assumption? Is this a buffer? If something else, then how?

(Need Help Please!!! If possible could you work it out so i can know how to do it)

Expert Solution

[HCN] = 0.250 M

ICE table

HCN + H2O <==> H3O+ + CN-

Initial 0.250 - -

change -x +x +x

Eq (0.250-x) x x

Ka = [H3O+][CN-]/[HCN]

4.9 x 10^-10 = x^2/0.250

Since Ka is very small, extent of dissociation x would be small and can be ignored in the denominator,

4.9 x 10^-10 = x^2/0.250

x = [H3O+] = 1.107 x 10^-5 M

pH = -log[H3O+] = 4.956

queen_honey_blossom answered 2 days ago

Find the pH of 0.190M NaCN solution. For HCN, Ka=4.9?10?10.

Determine the pH of 0.35M HCN. The Ka of HCN is 6.2e-10 M.

consider the titration of a 20ml sample of .105M HCN with .125M NaOH(ka=4.9*10^-10 of HCN) Draw...

consider the titration of a 20ml sample of .105M HCN with .125M NaOH(ka=4.9*10^-10 of HCN) Draw a scheme of how the titration curve should look like Find: initial pH, pH when 10ml of NaOH were added, pH at the equivalence point, pH when 16.8ml of NaOH were added

Consider a solution made by mixing HCN (Ka = 6.2 × 10–10) with HC2H3O2 (Ka =...

Consider a solution made by mixing HCN (Ka = 6.2 × 10–10) with HC2H3O2 (Ka = 1.8 × 10–5) in aqueous solution. What are the major species in solution? H+, CN–, H+, C2H3O2–, OH–, H2O H+, CN–, HC2H3O2, H2O HCN, HC2H3O2, H2O H+, CN–, H+, C2H3O2–, H2O HCN, H+, C2H3O2–, H2O Please explain with your answer.

What is the Ka reaction of HCN? The Ka of HCN is 6.2 × 10-10. What...

What is the Ka reaction of HCN? The Ka of HCN is 6.2 × 10-10. What is Kb value for CN– at 25°C?

The pH of 0.30 M solution of HCN is 5.20. Calculate the Ka value for HCN.

what is the ph of a 0.10m solution of nacn at 25°c (ka=4.9×10^-10 for hcn). I've...

what is the ph of a 0.10m solution of nacn at 25°c (ka=4.9×10^-10 for hcn). I've gotten 5.15 as a pH but the correct answer is 11.15. I don't see how it's 11.15...

A 50.0mL solution contains 0.120M HCN (Ka=6.2x10^-10) and 0.240M NaCN Calculate the final pH of the...

A 50.0mL solution contains 0.120M HCN (Ka=6.2x10^-10) and 0.240M NaCN Calculate the final pH of the solution after adding 20.0 mL of 0.0800 M HCl

Please explain these: 34. Which solution has the highest pH? Ka: HCN 5.8×10–10 CH3COOH 1.8×10–5 (A)...

Please explain these: 34. Which solution has the highest pH? Ka: HCN 5.8×10–10 CH3COOH 1.8×10–5 (A) 0.10 M CH3COOH (B) 0.10 M HCN (C) 0.10 M CH3COOK (D) 0.10 M NaBr 7. A dilute solution of which acid is most likely to produce a reduction product other than H2 when it reacts with a metal? (A) HF (B) HCl (C) HNO3 (D) H2SO4 35. A 75 mL solution that is 0.10 M in HC2H3O2 and 0.10 M in NaC2H3O2 has...

Find the pH of a 0.14M CH3COOH solution. Ka= 1.8x 10^-5

Question