Question:
Calculate the van't Hoff factor of a centimolar solution of potassium ferrocyanide if it is \(60\%\) dissociated at \(300\) K.
Calculate the van't Hoff factor of a centimolar solution of potassium ferrocyanide if it is \(60\%\) dissociated at \(300\) K.
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K4[Fe(CN)6] gives 5 ions. Use i = 1 + 4 alpha.
Updated On: Oct 1, 2026
- \(3.4\)
- \(3.9\)
- \(3.1\)
- \(3.7\)
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The Correct Option is A
Solution and Explanation
Step 1: Understanding the Concept:
Potassium ferrocyanide \(K_4[Fe(CN)_6]\) is an electrolyte. The van't Hoff factor \(i\) relates the real number of particles to the number expected without dissociation.
Step 2: Key Formula:
If one formula unit gives \(n\) ions and the degree of dissociation is \(\alpha\), then
\[ i = 1 + (n-1)\alpha \]
Step 3: Find n:
\(K_4[Fe(CN)_6] \rightarrow 4K^+ + [Fe(CN)_6]^{4-}\). So \(n = 5\).
Step 4: Calculate:
\[ i = 1 + (5-1)(0.60) = 1 + 2.4 = 3.4 \]
The concentration (0.01 M) and temperature do not enter the formula. The answer is option (A).
Final Answer:
The van't Hoff factor is 3.4. \[ \boxed{3.4} \]
Potassium ferrocyanide \(K_4[Fe(CN)_6]\) is an electrolyte. The van't Hoff factor \(i\) relates the real number of particles to the number expected without dissociation.
Step 2: Key Formula:
If one formula unit gives \(n\) ions and the degree of dissociation is \(\alpha\), then
\[ i = 1 + (n-1)\alpha \]
Step 3: Find n:
\(K_4[Fe(CN)_6] \rightarrow 4K^+ + [Fe(CN)_6]^{4-}\). So \(n = 5\).
Step 4: Calculate:
\[ i = 1 + (5-1)(0.60) = 1 + 2.4 = 3.4 \]
The concentration (0.01 M) and temperature do not enter the formula. The answer is option (A).
Final Answer:
The van't Hoff factor is 3.4. \[ \boxed{3.4} \]
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