Answer:
1.3 × 10⁻¹⁵
Explanation:
At a certain temperature, the pH of a neutral solution is 7.45. Then, we can calculate the concentration of H⁺.
pH = -log [H⁺]
[H⁺] = antilog -pH = antilog -7.45
[H⁺] = 3.55 × 10⁻⁸
By definition, in a neutral solution the concentration of H⁺ is equal to that of OH⁻.
Finally, we can calculate the ionic product of water (Kw).
Kw = [H⁺] × [OH⁻]
Kw = 3.55 × 10⁻⁸ × 3.55 × 10⁻⁸
Kw = 1.3 × 10⁻¹⁵
Answer:
The value of Kw is 1.26 * 10^-15
Explanation:
Step 1: Data given
The pH of the neutral solution = 7.45
pH = -log[H+]
Kw = [OH-][H+]
Step 2: Calculate [H+]
pH = 7.45
-log[H+] = 7.45
[H+] = 10^-7.45
[H+] = 3.55 * 10^-8 M
Step 3: Calculate [OH-]
Since pH and pOH are equal in our neutral solution so are [H+] = [OH-]
[OH-] = 3.55 * 10^-8 M
Step 4: Calculate Kw
Kw = [H]*[OH]
Kw = 3.55 * 10^-8 M * 3.55 * 10^-8 M
Kw = (3.55 * 10^-8)²
Kw = 1.26 * 10^-15
The value of Kw is 1.26 * 10^-15
