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Current Question (ID: 8524)

Question:

$\text{The ionization constant of chloroacetic acid is } 1.35 \times 10^{-3}. \text{ The pH of a } 0.1 \text{ M acid solution will be:}$

Options:

1. $1.94$
2. $6.14$
3. $3.23$
4. $5.64$

Solution:

\text{Hint: Chloroacetic acid is a weak acid.} \text{Explanation:} \text{Step 1: Write down the given data:} \text{Ionisation constant: } K_a = 1.35 \times 10^{-3} \text{Concentration: } c = 0.1 \text{ M} \text{Step 2: Calculate degree of ionization} K_a = c\alpha^2 \Rightarrow 1.35 \times 10^{-3} = 0.1 \times \alpha^2 \alpha = \sqrt{\frac{1.35 \times 10^{-3}}{0.1}} = 0.116 \text{Step 3: Calculate pH of the solution} [\text{H}^+] = c\alpha \Rightarrow [\text{H}^+] = 0.1 \times 0.116 = 0.0116 \text{ M} \text{pH} = -\log[\text{H}^+] \Rightarrow \text{pH} = -\log(0.0116) = 1.94

Import JSON File

Upload a JSON file containing LaTeX/MathJax formatted question, options, and solution.

Expected JSON Format:

{
  "question": "The mass of carbon present in 0.5 mole of $\\mathrm{K}_4[\\mathrm{Fe(CN)}_6]$ is:",
  "options": [
    {
      "id": 1,
      "text": "1.8 g"
    },
    {
      "id": 2,
      "text": "18 g"
    },
    {
      "id": 3,
      "text": "3.6 g"
    },
    {
      "id": 4,
      "text": "36 g"
    }
  ],
  "solution": "\\begin{align}\n&\\text{Hint: Mole concept}\\\\\n&1 \\text{ mole of } \\mathrm{K}_4[\\mathrm{Fe(CN)}_6] = 6 \\text{ moles of carbon atom}\\\\\n&0.5 \\text{ mole of } \\mathrm{K}_4[\\mathrm{Fe(CN)}_6] = 6 \\times 0.5 \\text{ mol} = 3 \\text{ mol}\\\\\n&1 \\text{ mol of carbon} = 12 \\text{ g}\\\\\n&3 \\text{ mol carbon} = 12 \\times 3 = 36 \\text{ g}\\\\\n&\\text{Hence, 36 g mass of carbon present in 0.5 mole of } \\mathrm{K}_4[\\mathrm{Fe(CN)}_6].\n\\end{align}",
  "correct_answer": 4
}