This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
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c) (i) Step 1: Identify reactants and products. Reactants are sodium chloride (NaCl) and concentrated sulphuric acid (H_2SO_4). Products are hydrogen chloride (HCl) and sodium hydrogen sulphate (NaHSO_4). Step 2: Write the balanced chemical equation. NaCl(s) + H_2SO_4(conc) → NaHSO_4(s) + HCl(g) (ii) Concentrated sulphuric acid is a strong oxidizing agent. Iodide ions (I^-) are strong reducing agents. When sodium iodide reacts with concentrated sulphuric acid, the sulphuric acid oxidizes the iodide ions to iodine (I_2), and itself gets reduced to sulphur dioxide (SO_2), sulphur (S), or hydrogen sulphide (H_2S). Therefore, hydrogen iodide (HI) is not formed or is immediately oxidized. d) The acid strength of hypohalous acids (HOX) depends on the electronegativity of the halogen (X). As the electronegativity of X increases, it pulls electron density away from the O-H bond, making the hydrogen more acidic. The order of electronegativity is Cl > Br > I. Therefore, the increasing order of acid strength is: HOI < HOBr < HOCl e) (i) Groups I and II elements are called s-block elements because their outermost electron (the differentiating electron) occupies an s-orbital. (ii) Diagonal relationship refers to the similarity in chemical properties between elements that are diagonally adjacent in the periodic table. This occurs between elements of Group 1 and Group 2, and Group 2 and Group 13, due to similar charge/radius ratios or polarizing power. (iii) Two s-block elements showing diagonal relationship are: • Lithium (Li) and Magnesium (Mg) • Beryllium (Be) and Aluminum (Al) (iv) Effect of heat on s-block nitrates: For LiNO_3: 4LiNO_3(s) heat 2Li_2O(s) + 4NO_2(g) + O_2(g) For NaNO_3: 2NaNO_3(s) heat 2NaNO_2(s) + O_2(g) (v) A: Group I carbonates are more stable to heat than Group II carbonates. The thermal stability of carbonates is inversely related to the polarizing power of the cation. Group I cations have a lower charge (+1) and generally larger ionic radii compared to Group II cations (+2). This results in Group I cations having lower polarizing power. A lower polarizing power means less distortion of the carbonate ion (CO_3^2-), making the C-O bonds stronger and thus requiring more energy to decompose the carbonate. B: The solubility of group II sulphates decreases down the group. The solubility of ionic compounds depends on the balance between lattice energy and hydration energy. For Group II sulphates, the anion (SO_4^2-) is large. As the cation size increases down Group II, both the lattice energy and the hydration energy decrease. However, the decrease in hydration energy is more significant than the decrease in lattice energy for larger cations when the anion is large. This leads to a net decrease in solubility down the group. Send me the next one 📸