Homework #5
- Page ID
- 42484
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Due on Feb 19 (Friday)
Q1
One example for NH3 as a conjugate acid:
Show by suitable net ionic equations that each of the following species can act as a Brønsted-Lowry acid:
- HCl
- NH3
- CH3CO2H
\(\ce{HPO4^{2-}}\) \(\ce{HSO_4^-}\)
Q2
Calculate the pH and the pOH of each of the following solutions at 25 °C for which the substances ionize completely:
- 0.014 M NaOH
- 0.0031 M Ca(OH)2
Q3
Calculate the pH of each of the following solutions at 25 °C. The values of Ka and Kb are found in lecture slides. Verify assumptions you make.
- 0.50 M C2H5NH2
- 0.0010 M HCOOH
Q4
The strongest base or strongest acid is the one with the larger Kb or Ka, respectively. The values of Ka and Kb are found in lecture slides.
- Which is the stronger acid,
\(\ce{NH4+}\) or HCN? - Which is the stronger base, C5H5N or \(\ce{C_6H_5COO^-}\)?