21.2. The pH Concept http://www.ck12.org
- How can the pOH of a solution be determined if its pH is known?
Problems
- Calculate the OH−ion concentration in solutions with the following H+concentrations. Assume a temperature
of 25°C. State whether the solution is acidic or basic.
a. [H+] = 2.3× 10 −^4 M
b. [H+] = 8.7× 10 −^10 M - Calculate the H+ion concentration in solutions with the following OH−concentrations. Assume a temperature
of 25°C. State whether the solution is acidic or basic.
a. [OH−] = 1.9× 10 −^9 M
b. [OH−] = 0.60 M - Calculate the pH of a solution with each of the following ion concentrations and indicate if the solution is
acidic or basic.
a. [H+] = 1.0× 10 −^5 M
b. [H+] = 2.8× 10 −^11 M
c. [OH−] = 1.0× 10 −^2 M
d. [OH−] = 4.4× 10 −^9 M - Calculate the pOH of the solutions listed in question 7.
- Determine [H+] and [OH−] in aqueous solutions with the following pH or pOH values.
a. pH = 1.87
b. pH = 11.15
c. pH =−0.95
d. pOH = 6.21
e. pOH = 14.42
f. pOH = 7.03 - A solution is prepared by dissolving 15.0 grams of NaOH into enough water to make 500.0 mL of solution.
Calculate the pH of the solution. - You have prepared 1.00 L of a solution with a pH of 5.00. What is the pH of the solution if 0.100 L of
additional water is added to it? (Hint: Calculate the moles of H+ions present in the solution.) - How much water would need to be added to the original solution in question 11 in order to bring the pH to
6.00?
Further Reading / Supplemental Links
- pH, http://www.kentchemistry.com/links/AcidsBases/pH.htm
- TheIonicProductforWater,Kw, http://www.chemguide.co.uk/physical/acidbaseeqia/kw.html
Points to Consider
Acids and bases can be characterized as either strong or weak, based on the extent to which they ionize in water.
- What are acid and base ionization constants?
- How is the pH of a solution containing a weak acid or a weak base calculated?