Mene ne lalata ruwa?

Musamman mawuyacin rashin daidaituwa (tsari na lalacewar ƙananan ƙwayoyin kwayoyin halitta - kwayoyin ions ko radicals - cikin ƙananan ƙwayoyin cuta) ƙaddarar ƙwayoyin electrolytic, wanda kwayoyin tsaka-tsaki daga wani abu da ake kira "electrolyte" ya rushe a cikin kwayoyin da aka caji (sakamakon sakamakon kwayoyin na ƙwayoyin polar): cations Kuma anions. Wannan ya bayyana da ikon na electrolyte mafita da za su gudanar da wutar lantarki.

Ana karɓa don raba dukkan masu jefa lantarki cikin ƙungiyoyi biyu: rauni da karfi. Ruwa yana nufin masu raunin zafin jiki, raguwa da ruwa yana ɗauke da ƙananan ƙwayoyin ƙwayar cuta, tun da yake suna da tsayin daka kuma kusan bazasu shiga cikin ions ba. Tsari (ba tare da tsabta) ruwa yana haifar da raunin wutar lantarki. Wannan shi ne saboda yanayin sunadarai na kwayoyin kanta kanta, lokacin da aka samar da nau'in hydrogen a fili a harsashin wutar lantarki wanda ke da ƙananan oxygen atom, wadda aka lalata da kyau.

A karfi da rauni da electrolyte ne halin da wani mataki na dissociation (nuna α, wannan yawa ne sau da yawa bayyana a matsayin% na 0 zuwa 100, ko a kasarun adadi na wani yanki daga 0 to 1) - ikon rarrabu cikin ions, Ina nufin rabo na yawan karye barbashi daga cikin barbashi don durkushe. Abubuwa irin acid da kuma tushe salts da mataki na iyakacin duniya ruwa kwayoyin dissociate cikin ions gaba daya. Tsarin ruwa yana tare da bazuwar H2O kwayoyin cikin proton H + da kuma hydroxyl kungiyar OH-. Idan muka wakilci raguwa da zazzaɓin ga electrolyte a cikin nau'i: M = K ++ A-, to, zubar da ruwa za a iya bayyana ta hanyar daidaituwa: H2O + H ++ OH-, da kuma daidaitakar da aka ƙididdige ƙimar da aka ƙera a ruwa zai iya wakilta a cikin siffofin biyu Gudanar da kafa protons ko maida hankali akan kafa kungiyoyin hydroxyl): α = [H +] / [H2O] ko α = [OH -] / [H2O]. Tun da darajar α ba ta shafi ba kawai ta hanyar yanayin sinadarin abu ba, amma ta hanyar mayar da hankali akan maganin ko zafin jiki, yana da kyau a yi magana game da digiri na (disney).

Halin yanayin kwayoyin masu raunin ƙarfi, ciki har da ruwa, zuwa lalata cikin ions yana nunawa sosai ta hanyar rikicewar rikicewa (wani nau'i na ma'auni na ma'auni), wanda ake kira Kd. Don ƙididdige wannan darajar, ana amfani da dokar yin amfani da mutane, wanda ke tabbatar da ragowar tsakanin yawancin abubuwan da aka samu da abubuwan da suka fara. An electrolytic dissociation na ruwa - wani bazuwar fara ruwa kwayoyin cikin hydrogen protons da hydroxyl kungiyar, duk da haka da dissociation m da aka bayyana ta da lissafi: KD = [H +] • [OH -] / [H2O]. Wannan darajar ruwa yana da ƙarfi kuma ya dogara ne kawai akan zafin jiki, a zafin jiki daidai da 25 ° C, Kd = 1.86 • 10-16.

Sanin yawan ruwa na ruwa (18 g / mol), da kuma watsi da ƙaddamar da kwayoyin da ba a raba su da kuma daukar nauyin 1 dm3 na ruwa da 1000 g, yana yiwuwa a lissafta ƙaddamar da kwayoyin da ba a raba su cikin 1 dm3 na ruwa: [H2O] = 1000 / 18.0153 = 55.51 Mol / dm3. Bayan haka, daga daidaituwa na wanzuwa, wanda zai iya samun samfurin samfurin protons da ƙungiyoyin hydroxyl: [H +] • [OH -] = 1.86 • 10-16 • 55.51 = 1 • 10-14. Lokacin da aka samo asalin tushen daga samfurin da aka samo, an samu yawancin protons (hydrogen ions), wanda ke ƙayyade acidity na maganin kuma yayi daidai da maida hankali akan kungiyoyin hydroxyl: [H +] = [OH -] = 1 • 10-7.

Amma a cikin yanayin ruwa na irin wannan tsabta ba ya wanzu saboda kasancewar gasadarar ciki a ciki ko gurbataccen ruwa ta wasu abubuwa (hakikanin gaskiya, ruwa shine maganin masu yawan lantarki), sabili da haka a 25oC maida hankali akan hawan hydrogen protons ko ƙaddamar da kamfanonin hydroxyl ya bambanta da 1.10-7. Watau, acidity na ruwa ne saboda ƙaddamarwa ba wai kawai wani tsari ba ne kamar lalata ruwa. A hydrogen index ne korau logarithm na hydrogen ion maida hankali (PH), shi ne ya gabatar ga kimantawa da acidity ko alkalinity na ruwa da kuma mai ruwa-ruwa mafita, kamar yadda lambobin da korau ikon amfani da wuya. Domin ruwa mai tsabta, pH = 7, amma tun da babu ruwa mai tsabta a yanayi, da kuma ɓatar da ruwa ya zo tare da rushe wasu sunadarai masu rarraba, haɗin ginin hydrogen zai iya zama ƙasa ko fiye da 7, wato, don ruwa, a aikin, pH ≠ 7.