Final answer:
The pH of a solution formed with calcium oxide is approximately 13.3, assuming it forms a 0.2M solution of Ca(OH)2. A similar solution of strontium oxide would also be very basic; however, exact pH requires specific concentration data.
Step-by-step explanation:
To suggest the approximate pH of the solutions formed with calcium oxide and strontium oxide, we assume that both form strong bases in water (Ca(OH)2 and Sr(OH)2, respectively). Given that [OH-] = 2[Ca(OH)2] = 0.2M for calcium hydroxide, we can find the pOH using the formula pOH = -log[OH-]. Subsequently, we use pH = 14 - pOH to find the pH of the solution.
For calcium hydroxide:
pOH = -log(0.2 M) = 0.7
pH = 14 - pOH = 14 - 0.7 = 13.3
For strontium hydroxide, which is also a strong base and likely to have a similar concentration when dissolved in water, the pH calculation would be similar, suggesting a pH close to 13.3 as well. Without specific concentration data for strontium hydroxide, we can hypothesize that its pH will also be very basic, but precise numbers would require exact concentration values.