Homework Help: Chemistry

Posted by Raj on Thursday, May 31, 2007 at 9:02pm.

Calculate the end point pH, when 25 mL of 0.01 mol/L HCl solution reacts exactly with 25 mL of 0.1 mol/L NH4OH solution.

NH3 Kb = 1.8 x 10^-5

This will be the pH of NH4Cl solution.
NH4+ + HOH ==> NH3 + H3O^+
Ka = Kw/Kb = (NH3)(H3O^+)/(NH4^+). Solve for H3O^+, then pH = - log(H3O^+). Post your work if you get stuck.

But we haven't learned how to get the pH of H3O+...we only get the pH of [H+].

Same thing. They are all H3O^+ but sometimes we get a little lazy and instead of writing H3O^+ or H*H2O^+ we just omit the water part and write H^+.

No one has answered this question yet.

Answer this Question

Related Questions

chemistry - Please let me know if my answer to the following question is correct...
Chemistry - (a) Calculate the molarity of a solution that contains 0.175 mol ...
Chemistry - What is the concentration of HCl when 25.0 mL of HCl completely ...
Environmental Chemistry - Calculate the pH when the following volumes of 0.20 M ...
Chemistry - a 25.0 mL sample of .050 M solution of aqueous trimethylamine is ...
Chemistry - A solution is prepared using 15.0 mL of 1.0 M HCl and 20.0 mL of 0.5...
chemistry - 25 mL of standardized 0.45 mol/L NaOH is titrated with 21 mL of 0.35...
Chemistry - A 10.0-mL solution of 0.30 M NH3 is titrated with a 0.100 M HCl ...
Chemistry - The titration of a 50.0 mL solution of the monoprotic bromoacetic ...
chem - Calculate the [h3o+] and [oh-], pH and the percent dissociation for both ...

For Further Reading

First Name:
School Subject:
Answer: