Import Question JSON

Current Question (ID: 10669)

Question:

$\text{Which of the following statements about acid strength is false?}$

Options:

1. $\text{HI} > \text{HBr} > \text{HCl}$
2. $\text{HIO}_4 > \text{HBrO}_4 > \text{HClO}_4$ (Correct)
3. $\text{HClO}_4 > \text{HClO}_3 > \text{HClO}_2$
4. $\text{HF} > \text{H}_2\text{O} > \text{NH}_3$

Solution:

$\text{Hint: Acidic strength in oxyacids the larger the oxidation state of the central atom the stronger the acid.}$ $\text{a. The bond strength H-X decreases from HF to HI. Thus, HF is most stable while HI is least stable and because of it down the group acidity increases.}$ $\text{HI} > \text{HBr} > \text{HCl is correct order}$ $\text{b. As electronegativity of the central atom increases the acidity of the compound also increases.}$ $\text{HF} > \text{H}_2\text{O} > \text{NH}_3 \text{ is the correct order.}$ $\text{c. As oxidation of the central atom increases the acidity of the compound also increases.}$ $\text{HClO}_4^{+7} > \text{HClO}_3^{+5} > \text{HClO}_2^{+3}$ $\text{d. Acidic strength has been decided on the basis of electronegativity or charge density on the central atom.}$ $\text{The Hydrogen atom in HClO}_4 \text{ will experience less attraction to Oxygen than in HIO}_4\text{. That's why HClO}_4 \text{ is stronger than HIO}_4\text{.}$ $\text{On comparing acidic strength in oxyacids the larger the oxidation state of the central atom the stronger the acid and if the oxidation is the same as the electronegative the central atom is stronger the acidic strength.}$ $\text{Hence, the correct order is -}$ $\text{HIO}_4 < \text{HBrO}_4 < \text{HClO}_4$

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
}