Wednesday
April 16, 2014

Homework Help: Chemistry

Posted by Chris on Friday, November 30, 2012 at 10:04pm.

consider 1.0 L of a solution which is 0.55 M HF and 0.2 M NaF (Ka for HF = 7.2 x 10-4). Calculate the pH after 0.10 mol of HCl has been added to the original solution. Assume no volume change on addition of HCl.
Goes along with the last one i posted, i know i have to realize that the acid will go to completion and subtract it from the base but im a little lost on how to go on

Answer this Question

First Name:
School Subject:
Answer:

Related Questions

Chemistry - consider 1.0 L of a solution which is 0.55 M HF and 0.2 M NaF (Ka ...
chemistry - how many moles of solute are contained in each solution? 250 mL of a...
Chemistry - A teacher prepares a saturated NaCli solution at 55 Degree C. What ...
chemistry - A solution is prepared by adding 30.00 g of lactose (milk sugar) to ...
Chemistry - what is the hydronium ion concentration in a 0.55 M HNO3 solution...
Chemistry - what is the hydronium ion concentration in a 0.55 M HNO3 solution...
Chemistry - Consider a 0.80M solution of HCN. The Ka of HCN is 6.2x10-10. What ...
math - A pharmacist mixes 14 ounces of 68% saline solution with 55% saline ...
Chemistry - 24.5 ml of water are added to a 1.20 molar solution of nitric acid. ...
Chemistry - Consider a 9.5e-10 M solution of HClO4 at 283 K. What is the pH of ...

Search
Members