http://www.ck12.org Chapter 21. Acids and Bases
d. CsI
e. NH 4 Br
f. NaNO 2- Explain why an anion derived from the neutralization of a weak acid produces a basic solution when dissolved
in water. - Explain why a solution containing both HCN and NaCN is a buffer, but a solution containing both HBr and
NaBr is not a buffer.
Problems
- Write balanced net ionic equations showing the hydrolysis of the following salts.
a. NaNO 2
b. NH 4 NO 3
c. K 2 SO 3 - The Kbof the carbonate ion (CO 32 −) is 2.1× 10 −^4. Calculate the pH of a 0.400 M solution of sodium
carbonate (Na 2 CO 3 ). - The Kaof the methyl ammonium ion (CH 3 NH 3 +) is 2.3× 10 −^11. Calculate the pH of a 1.50 M solution of
methyl ammonium chloride (CH 3 NH 3 Cl). - The pH of a 1.00 M solution of a certain salt is measured to be 9.81. Calculate the Kbof the anion of the salt.
- Use the buffer between carbonic acid and the hydrogen carbonate ion (H 2 CO 3 / HCO 3 −) to show how a buffer
system works. Show with two separate equations how this buffer would respond to small additions of acid or
base. - Many household bleaches are a 6.0% by mass solution of sodium hypochlorite (NaClO). The Kbof ClO−is
2.9× 10 −^7. Assuming that the density of the bleach is 1.0 g/mL, calculate the pH of household bleach.
Further Reading / Supplemental Links
- HydrolysisofSalts, (http://www.kentchemistry.com/links/AcidsBases/Hydrolysis.htm
- BufferSolutions, (http://www.chemguide.co.uk/physical/acidbaseeqia/buffers.html
Points to Consider
Acid-base reactions involve the transfer of a hydrogen ion from one substance to another. An oxidation-reduction
reaction is another common type of reaction that involves the transfer of one or more electrons from one substance
to another.
- How can an oxidation-reduction reaction be recognized?
- What is corrosion, and how does it relate to a transfer of electrons?