Quiz — rappel acide-base1.pdf

Question 1 sur 10 20:00

[{"id":33160,"question":"Selon la théorie de Brønsted-Lowry, un acide est une espèce chimique capable de :","option_a":"Donner un proton H⁺","option_b":"Capter un proton H⁺","option_c":"Donner un électron","option_d":"Capter un électron","option_e":"","option_f":"","bonne_reponse":"a","explication":"Un acide, selon Brønsted-Lowry, est une espèce chimique capable de donner un proton H⁺ (ou ion hydrogène).","points":1,"type":"qcm","actif":1,"section_id":null,"ordre":0,"_debug_answer_data_type":"string","_debug_answer_data_preview":"{\"correct\": \"a\", \"options\": {\"a\": \"Donner un proton H⁺\", \"b\": \"Capter un proton H⁺\", \"c\": \"Donne","_debug_options_count":4},{"id":33161,"question":"Le pH d'une solution de concentration en ions H₃O⁺ égale à 10⁻³ mol\/L est :","option_a":"3","option_b":"11","option_c":"1","option_d":"7","option_e":"","option_f":"","bonne_reponse":"a","explication":"Le pH se calcule avec la formule pH = -log[H₃O⁺]. Ici, pH = -log(10⁻³) = 3.","points":1,"type":"qcm","actif":1,"section_id":null,"ordre":0,"_debug_answer_data_type":"string","_debug_answer_data_preview":"{\"correct\": \"a\", \"options\": {\"a\": \"3\", \"b\": \"11\", \"c\": \"1\", \"d\": \"7\"}}","_debug_options_count":4},{"id":33162,"question":"Un acide faible a une constante d'acidité Ka très grande.","option_a":"Vrai","option_b":"Faux","option_c":"","option_d":"","option_e":"","option_f":"","bonne_reponse":"b","explication":"Un acide faible a une constante d'acidité Ka faible, car il ne se dissocie que partiellement en solution.","points":1,"type":"qcm","actif":1,"section_id":null,"ordre":0,"_debug_answer_data_type":"string","_debug_answer_data_preview":"{\"correct\": \"b\", \"options\": {\"a\": \"Vrai\", \"b\": \"Faux\", \"c\": \"\", \"d\": \"\"}}","_debug_options_count":4},{"id":33163,"question":"Lors d'une réaction acido-basique, l'espèce qui capte un proton est :","option_a":"Un acide","option_b":"Une base","option_c":"Un solvant","option_d":"Un sel","option_e":"","option_f":"","bonne_reponse":"b","explication":"Une base est une espèce chimique capable de capter un proton H⁺.","points":1,"type":"qcm","actif":1,"section_id":null,"ordre":0,"_debug_answer_data_type":"string","_debug_answer_data_preview":"{\"correct\": \"b\", \"options\": {\"a\": \"Un acide\", \"b\": \"Une base\", \"c\": \"Un solvant\", \"d\": \"Un sel\"}}","_debug_options_count":4},{"id":33164,"question":"Le pH d'une solution neutre à 25°C est égal à :","option_a":"0","option_b":"7","option_c":"14","option_d":"10⁻⁷","option_e":"","option_f":"","bonne_reponse":"b","explication":"À 25°C, une solution neutre a un pH de 7, car [H₃O⁺] = [OH⁻] = 10⁻⁷ mol\/L.","points":1,"type":"qcm","actif":1,"section_id":null,"ordre":0,"_debug_answer_data_type":"string","_debug_answer_data_preview":"{\"correct\": \"b\", \"options\": {\"a\": \"0\", \"b\": \"7\", \"c\": \"14\", \"d\": \"10⁻⁷\"}}","_debug_options_count":4},{"id":33165,"question":"La constante d'acidité Ka d'un acide fort est généralement :","option_a":"Très petite (Ka \u003C\u003C 1)","option_b":"Très grande (Ka \u003E\u003E 1)","option_c":"Égale à 1","option_d":"Nulle","option_e":"","option_f":"","bonne_reponse":"b","explication":"Un acide fort se dissocie totalement, donc sa constante d'acidité Ka est très grande (Ka \u003E\u003E 1).","points":1,"type":"qcm","actif":1,"section_id":null,"ordre":0,"_debug_answer_data_type":"string","_debug_answer_data_preview":"{\"correct\": \"b\", \"options\": {\"a\": \"Très petite (Ka \u003C\u003C 1)\", \"b\": \"Très grande (Ka \u003E\u003E 1)\", \"c\": \"Ég","_debug_options_count":4},{"id":33166,"question":"Un indicateur coloré comme le bleu de bromothymol (BBT) est jaune en milieu acide et bleu en milieu basique.","option_a":"Vrai","option_b":"Faux","option_c":"","option_d":"","option_e":"","option_f":"","bonne_reponse":"a","explication":"Le BBT est jaune en milieu acide (pH \u003C 6) et bleu en milieu basique (pH \u003E 7,6).","points":1,"type":"qcm","actif":1,"section_id":null,"ordre":0,"_debug_answer_data_type":"string","_debug_answer_data_preview":"{\"correct\": \"a\", \"options\": {\"a\": \"Vrai\", \"b\": \"Faux\", \"c\": \"\", \"d\": \"\"}}","_debug_options_count":4},{"id":33167,"question":"Lors de la neutralisation d'un acide par une base, les produits formés sont :","option_a":"De l'eau et un sel","option_b":"Un gaz et un sel","option_c":"Un oxyde et de l'eau","option_d":"Un acide et une base","option_e":"","option_f":"","bonne_reponse":"a","explication":"La neutralisation d'un acide par une base produit de l'eau et un sel (réaction acido-basique).","points":1,"type":"qcm","actif":1,"section_id":null,"ordre":0,"_debug_answer_data_type":"string","_debug_answer_data_preview":"{\"correct\": \"a\", \"options\": {\"a\": \"De l'eau et un sel\", \"b\": \"Un gaz et un sel\", \"c\": \"Un oxyde et d","_debug_options_count":4},{"id":33168,"question":"Le pKa d'un couple acido-basique est défini comme :","option_a":"pKa = -log(Ka)","option_b":"pKa = log(Ka)","option_c":"pKa = Ka","option_d":"pKa = 1\/Ka","option_e":"","option_f":"","bonne_reponse":"a","explication":"Le pKa est défini comme le logarithme négatif de la constante d'acidité Ka : pKa = -log(Ka).","points":1,"type":"qcm","actif":1,"section_id":null,"ordre":0,"_debug_answer_data_type":"string","_debug_answer_data_preview":"{\"correct\": \"a\", \"options\": {\"a\": \"pKa = -log(Ka)\", \"b\": \"pKa = log(Ka)\", \"c\": \"pKa = Ka\", \"d\": \"pKa","_debug_options_count":4},{"id":33169,"question":"Une solution tampon est une solution qui :","option_a":"Résiste aux variations de pH","option_b":"A un pH très acide","option_c":"Précipite en milieu basique","option_d":"Ne contient pas d'ions","option_e":"","option_f":"","bonne_reponse":"a","explication":"Une solution tampon est une solution qui résiste aux variations de pH lors de l'ajout modéré d'acide ou de base.","points":1,"type":"qcm","actif":1,"section_id":null,"ordre":0,"_debug_answer_data_type":"string","_debug_answer_data_preview":"{\"correct\": \"a\", \"options\": {\"a\": \"Résiste aux variations de pH\", \"b\": \"A un pH très acide\", \"c\": ","_debug_options_count":4}]