The pH of the buffer prepared by adding 275 mL of .676M of HCl to 500 mL of .525M sodium acetate is 6.45.
<h3>How to calculate pH?</h3>
The pH of a buffer solution can be calculated by initially calculating the millimoles of both the conjugate base and acid.
- Millimoles of hydrochloric acid = 275mL × 0.676M = 185.9millimoles
- Millimoles of sodium acetate = 500mL × 0.525M = 262.5millimoles
From, Henderson Hasselbalch equation,
pH = pKa + log conjugate base/acid
pka of HCl = -6.3
-6.3 + log 262.5/185.9
6.3 + 0.15
pH = 6.45
Therefore, the pH of the buffer prepared by adding 275 mL of .676M of HCl to 500 mL of .525M sodium acetate is 6.45.
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Answer:
Check Explanation.
Explanation:
Formation reactions are chemical reactions where one mole of a compound is produced from its constituent elements in their standard states.
NaBr (s)
The Standard formation reaction is
Na (s) + (1/2)Br₂ (g) → NaBr (s)
Using appendix C, the standard heat of formation of NaBr(s) is
ΔH∘f = -359.8 kJ/mol.
SO₃ (g)
The Standard formation reaction is
S (s) + (3/2) O₂ (g) → SO₃ (g)
Using appendix C, the standard heat of formation of SO₃(g) is
ΔH∘f = -395.2 kJ/mol.
Pb(NO₃)₂ (s)
The Standard formation reaction is
Pb (s) + N₂ (g) + 3O₂ (g) → Pb(NO₃)₂ (s)
Using appendix C, the standard heat of formation of Pb(NO₃)₂(s) is
ΔH∘f = -451.9 kJ/mol.
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