Consider a 0.1 M aqueous solution of the following salts. Which solution(s) woul

Question

Consider a 0.1 M aqueous solution of the following salts. Which solution(s) would be considered "basic" AlCl_3 NaHSO_4 pK_a = 1.9 NaHCO_3 (H_2CO_3 pK_a1 = 3.6 pK_a2 10.2) NH4Cl pK_a = 9.24 2 and 3 3 2, 3 and 4 all of the above compounds will form a basic solution none of the above compounds will form a basic solution Which of the following statements is true? All Lewis bases are hydroxide donors Group 13 halides are Lewis acids (examples: BF_3, InBr_3) Lewis acids are electron pair donors Lewis bases are single electron acceptors All of these are true

Explanation / Answer

1) option (b) only correct, as it is prepared from strong base NaOH and weak acid H2CO3 ,hence it has basic nature

AlCl3 is prepared from weak base Al(OH)3and strong acid HCl

NaHSO4 prepared from strong acid and strong base hence it is almost neutral

NH4Cl is prepared from weak base NH4OH and strong acid HCl hence it has acidic nature

2)option (b) All 13 group halide are Lewis acids as they have vacant orbitals to accept a pair of electrons

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