Posted by Maddie on Friday, April 12, 2013 at 12:46pm.
The pH of an 0.0870 M solution of weak acid A is 2.20. The pH of an 0.0830 M solution of weak acid B is 4.07. The pH of an 0.0890 M solution of weak acid C is 5.13. Identify the three acids from among those listed below (the Ka values are listed in Appendix E of your textbook).
J None of the above
I'm not exactly sure what to do with the molarities... Any help please?
- Chemistry - DBob222, Friday, April 12, 2013 at 4:37pm
We will call weak acid A as HA.
pH = 2.20; therefore, H^+ = 6.31E-3
...........HA ==-> H^+ + A^-
You know x = 6.31E-3; therefore,
Ka = (H^+)(A^-)/(HA)
Ka = (6.31E-3)(6.31E-3)/(0.08069) = ?
Now look up the Ka values in Appendix E of your text and find the acid with the value you have above. That will identify the acid. Textbooks differ in what they print for the Ka/Kb values for weak acids and weak bases but I suspect acid A is HNO2.
Answer This Question
More Related Questions
- chemistry - 2- A 0.310 M solution of a weak acid, HX, has a pH of 2.53 a. Find ...
- chemistry - A 1.00M solution of a hypothetical weak acid (HB) has a pH of 2.85. ...
- chemistry - A. Strong Base 1.) What is the concentration of a solution of KOH ...
- chemistry help - A 15.00 mL sample of an unknown monoprotic weak acid solution ...
- Chemistry - 1 g of acid was mixed with 120 ml of distilled water and the ...
- chemistry - A 15.00 mL sample of an unknown monoprotic weak acid solution is ...
- Chemistry - A 0.108 M sample of a weak acid is 4.16% ionized in solution. what ...
- Chemistry-Dr Bob help!! - 0.100 M solution of a weak acid, HX, is known to be ...
- Chemistry - A 5.55g sample of a weak acid with Ka=1.3 x10^-4 was combined with 5...
- chemistry - A 0.27 sample of a weak acid with an unknown was combined with 12.0 ...