Final answer:
The pH of a 0.0010M solution of strontium hydroxide is 11.3. This is calculated by finding the concentration of hydroxide ions, which is twice the concentration of the strontium hydroxide solution, and then determining the pOH followed by the pH.
Step-by-step explanation:
The question asks to determine the pH of a 0.0010M solution of strontium hydroxide, Sr(OH)2. Strontium hydroxide is a strong base that dissociates completely in water to form Sr2+ and two OH− ions. The concentration of OH− ions is therefore 2 * 0.0010M = 0.0020M. To find the pH, we must first find the pOH by taking the negative logarithm of the hydroxide ion concentration. We then subtract the pOH from 14 to get the pH.
pOH = −log(0.0020) = 2.7
pH = 14 − pOH = 14 − 2.7 = 11.3