Thursday
October 23, 2014

Homework Help: chemistry

Posted by Abigail on Tuesday, April 15, 2008 at 5:01pm.

Please judge my answer, thank you

Question:
What is the pH of a 1.24 mol/L solution of HCN(aq) if its Ka = 6.2 x 10-10?

Answer:
It is imperative to initially set up ionization. THen, it becomes important to write the Ka expression, after which setting up an ICE table becomes nessecary. Substituting as well as solving for H^+ and converting this to pH becomes the next step. The ionization equation is HCN(aq) + H20==> H3O^+ CN^-. The Ka expression becomes Ka=[H3O^+][CN^-]/[HCN][H2O] After setting up the ice table the equilibrium concentration, in order, are x- 1.33 +x -x -x Solving for H^+ gives a value of 4,61. Converting H^+ concentraitons to pH requires the use of the formula pH=-log[H^+]. After substituting in the values, the answer becomes 0.7. Therefore the pH is 0.7

Answer this Question

First Name:
School Subject:
Answer:

Related Questions

chemistry - What is the pH of a 1.24 mol/L solution of HCN(aq) if its Ka = 6.2 x...
chemistry - Please judge my answer: Question: 24 mL of 0.39 mol/L acetic acid is...
chemistry - Please let me know if my answer to the following question is correct...
chemistry - Calculate the pH of a 1.33 mol/L solution of HCN is the Ka value of ...
Chemistry - Indicate which of the following has the highest entropy at 298 K. 0....
chem - Calculate the [h3o+] and [oh-], pH and the percent dissociation for both ...
Chemistry - Determine [Zn2 ], [CN–], and [HCN] in a saturated solution of Zn(CN)...
Chemistry - Can you check if this is correct please? a) How many moles of sodium...
Chemistry(Please check) - 1) The Ka for acetic acid is 1.8e-5. What is the pH of...
CHEMISTRY> HELP QUICK! pls - i have an exam friday and cant figure this ...

Search
Members