Answer:
The pH of the buffer solution = 8.05
Explanation:
Using the Henderson - Hasselbalch equation;
pH = pKa₂ + log ( [HPO₄²-]/[H₂PO4⁻]
where pKa₂ = -log (Ka₂) = -log ( 6.1 * 10⁻⁸) = 7.21
Concentration of OH⁻ added = 0.069 M (i.e. 0.069 mol/L)
[H₂PO4⁻] after addition of OH⁻ = 0.165 - 0.069 = 0.096 M
[HPO₄²-] after addition of OH⁻ = 0.594 + 0.069 = 0.663 M
Therefore,
pH = 7.21 + log (0.663 / 0.096)
pH = 7.21 + 0.84
pH = 8.05
Answer:
63.5 w isvthebanswerok is th answer
Answer:
[H⁺] = 3.98×10⁻⁷ M
Explanation:
Given data:
pH of blood = 6.40
Hydrogen ion concentration = ?
Solution:
Formula:
pH = - log[H⁺]
by rearranging this formula,
[H⁺] = 10⁻(pH)
By putting values,
[H⁺] = 10 ⁻⁶°⁴⁰
[H⁺] = 3.98×10⁻⁷ M
106.4 is going to be your answer
