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Здравствуйте! Прошу помощи в следующем вопросе: необходимо представить ионные и молекулярные уравнения следующих реакций - -CoCl2+KCNS[$8594$] -CoCl2+KCNS+H2O[$8594$] -CoCl2+KCNS+C2H5OH[$8594$] -K3Fe(CH)6+KCNS[$8594$] -FeCl3+KCNS[$8594$]
Это из лабораторной работы? какие при этом наблюдения? CoCl2+KCNS - образуется синий комплекс CoCl2+KCNS+H2O - разложение комплекса при разбавлении? CoC2+KCNS+C2H5OH - что именно делали и что происходит? K3[Fe(CN)6]+KCNS - не реагируют FeCl3+KCNS - образуется красный комплекс
Здравствуйте уважаемый Роман, при проведении лабораторных опытов установлено: по первой реакция образовался тетрароданокобальтат (II) калия раствор получил лиловую окраску далее раствор разделили на две части в одну добавили 10 капель воды раствор получил бледно розовую окраску в другую добавили этиловый спирт , цвет в пробирки разделился на 2 части, в верхней части пробирки он стал синим , снизу розовым, при перемешивании содержимого пробирки раствор постепенно стал синим. На основании опыта надо установить, где полнее происходит диссоциация комплексного иона в воде или спирте? Последняя реакция дала результат по изменению окраски раствора на красный. При проведении предпоследней реакции каких либо изменений не установлено.
Здравствуйте, samstep.stepanov! CoCl2+4KSCN=K2[Co(SCN)4]+2KCl Co2++4SCN-=[Co(SCN)4]2- Или точнее (учитывая, что количество лигандов может варьироваться) Co2++nSCN-=[Co(SCN)n]2-n При этом фиолетовый цвет вероятно свидетельствует о неполном протекании реакции (поскольку комплекс имеет синий цвет).
далее раствор разделили на две части в одну добавили 10 капель воды раствор получил бледно розовую окраску
Этот комплекс весьма малостабилен, поэтому при разбавлении раствора он легко диссоциирует - равновесие в предыдущей реакции смещается в обратную сторону из-за уменьшения концентраций. Розовый цвет раствора обусловлен гидратированными ионами кобальта (II)
в другую добавили этиловый спирт , цвет в пробирки разделился на 2 части, в верхней части пробирки он стал синим , снизу розовым, при перемешивании содержимого пробирки раствор постепенно стал синим
Роданидный комплекс кобальта лучше растворим в спиртах и поэтому экстрагируется в верхний слой. Помимо этого нужно отметить, что добавление органического растворителя стабилизирует комплекс не только сольватацией, но и уменьшением концентрации свободной воды (особенно если спирт сильно с ней координируется). Нужно учитывать, что на самом деле равновесие представляет из себя не образование-диссоциацию комплекса, а замещение в координационной сфере воды на роданид и обратно: [Co(H2O)4]2++4CNS-=[Co(CNS)4]2-+4H2O В водном растворе гидротационную воду обычно не рассматривают, поскольку концентрация свободной воды практически постоянна, но уже при добавлении органического растворителя (особенно, способного связывать воду), её количество уменьшается, что повышает стабильность комплексных ионов относительно аквакомплексов (то есть гидратированных ионов комплексообразователя)
K3[Fe(CN)6]+KSCN реакции не происходит, поскольку цианидный комплекс железа (III) гораздо стабильнее роданидного. Гексацианоферраты вообще настолько стабильны, что даже практически нетоксичны.
FeCl3+4KSCN=K[Fe(SCN)4]+3KCl Fe3++4SCN-=[Fe(SCN)4]- или в общем виде Fe3++nSCN-=[Fe(SCN)n]3-n Здесь число лигандов может варьироваться от 1 до 6. [Fe(SCN)4]- - наиболее стабильный из комплексных ионов и даёт тёмно красную окраску. Интересно отметить что цвет зависит от числа лигандов: Если добавить небольшое количество соли железа (III) к насыщенному раствору роданида калия, то можно увидеть, что [Fe(SCN)6]3- на самом деле обладает розово-фиолетовой окраской. Если же раствор [Fe(SCN)4]- разбавлять, то при частичной диссоциации комплекса становится видно, что [Fe(SCN)]2+ имеет жёлтую окраску, более выраженную, чем у Fe3+.
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