Misalan tambayoyi game da Ƙarfin Electrolytes, Rauni Electrolytes, da Ba electrolytes ba
Electrolytes muhimmin ra'ayi ne a fannin ilmin sunadarai wanda yake da matuƙar muhimmanci, musamman a nazarin halayen da suka shafi mafita. Electrolytes sune mahaɗan da, idan aka narkar da su a cikin ruwa, suke samar da ions waɗanda ke ba da damar maganin ya gudanar da wutar lantarki. Dangane da ikonsu na rabuwa zuwa ions, an raba electrolytes zuwa rukuni uku: ƙarfi electrolytes, rauni electrolytes, da kuma waɗanda ba electrolytes ba. Wannan labarin zai tattauna misalai daban-daban na matsaloli da suka shafi waɗannan nau'ikan electrolytes guda uku, tare da bayani mai sauƙin fahimta.
Ƙarfin Electrolyte
Kwayoyin lantarki masu ƙarfi sune mahadi waɗanda ke narkewa gaba ɗaya a cikin ruwa. Wannan yana nufin cewa idan aka narkar da wani sinadarin lantarki mai ƙarfi a cikin ruwa, kusan dukkanin ƙwayoyin halittarsa suna rabuwa zuwa ions. Misalan da aka saba gani na ƙwayoyin lantarki masu ƙarfi sun haɗa da gishiri kamar sodium chloride (NaCl), acid masu ƙarfi kamar hydrochloric acid (HCl), da tushe masu ƙarfi kamar sodium hydroxide (NaOH).
Tambaya ta 1:
Yadda ake ƙididdige molarity na ions a cikin maganin HCl na 0,1 M?
Tattaunawa:
HCl wani sinadari ne mai ƙarfi wanda ke rabuwa gaba ɗaya cikin ruwa bisa ga lissafin:
\[ \text{HCl} \rightarrow \text{H}^+ + \text{Cl}^- \]
Tunda HCl mai ƙarfi ne na electrolyte, za mu iya ɗaukar farkon yawan HCl (0,1 M) a matsayin yawan H+ da Cl- ions da aka samar. Don haka, a cikin maganin HCl na 0,1 M:
[\(\text{H}^+\)] = 0,1 M
[\(\text{Cl}^-\)] = 0,1 M
Rauni Electrolyte
Rashin ƙarfin lantarki (eletryl) yana yin ion ne kawai a cikin ruwan da aka narkar. Wannan yana nufin cewa ƙaramin ɓangare ne kawai na ƙwayoyin electrolyte masu rauni ke samar da ions idan aka narkar da su a cikin ruwa. Misalan raunin lantarki sun haɗa da acid masu rauni kamar acetic acid (CH3COOH) da tushe masu rauni kamar ammonia (NH3).
Tambaya ta 2:
A tantance matakin ionization da yawan ion a cikin 0,1 M CH3COOH. Matsakaicin rabuwar acid (\(K_a\)) na CH3COOH shine 1,8 × 10^-5.
Tattaunawa:
Za a iya rubuta martanin rabuwar CH3COOH a cikin ruwa kamar haka:
\[ \text{CH}_3\text{COOH} \rightleftharpoons \text{CH}_3\text{COO}^- + \text{H}^+ \]
An bayyana matakin rabuwar (\(\alpha\)) a matsayin ɓangaren acid ɗin da ke rabuwa zuwa ions. Ta amfani da ƙimar \(K_a\), za mu iya rubuta alaƙar da ke gaba don maganin 0,1 M CH3COOH:
\[ K_a = [\text{CH}_3\text{COO}^-][\text{H}^+] / [\text{CH}_3\text{COOH}] \]
Tunda ionization na CH3COOH wani ɓangare ne, yawan ions da aka samar shine cα, inda c shine farkon yawan CH3COOH (0,1 M). Sannan lissafin ya zama:
\[ sau 1,8 10^{-5} = \frac{(0,1\alpha)(0,1\alpha)}{0,1(1-\alpha)} \]
Sauƙaƙa zuwa:
\[ sau 1,8 10^{-5} = \frac{0,01\alpha^2}{0,1 – 0,1\alpha} \]
A ɗauka cewa α ƙarami ne har za mu iya yin watsi da α a cikin ma'aunin rabo:
\[ sau 1,8 sau 10^{-5} \ kusan 0,01\alpha^2 / 0,1 \]
\[ sau 1,8 sau 10^{-5} \kimanin \alpha^2 \]
\[ \alpha \approx \sqrt{1,8 \sau 10^{-5}} \]
\[ \alpha \kimanin 4,24 \sau 10^{-3} \]
Don haka, matakin ionization shine 4,24 × 10^-3 ko 0,424%.
Yawan H+ da CH3COO- ions a cikin maganin shine:
\[ [\text{H}^+] = 0,1 \sau 4,24 \sau 10^{-3} \sau 4,24 \sau 10^{-4} \]
\[ [\text{CH}_3\text{COO}^-] = 0,1 \times 4,24 \times 10^{-3} \approx 4,24 \times 10^{-4} \]
Ba electrolytes ba
Ba electrolytes ba mahadi ne da ba sa yin ion a cikin ruwan da ke cikinsa. Wannan yana nufin cewa mafita waɗanda ba electrolyte ba ba sa samar da ions, don haka ba za su iya gudanar da wutar lantarki ba. Misalan waɗanda ba electrolytes ba sun haɗa da sukari (sucrose), urea, da barasa.
Tambaya ta 3:
Me yasa maganin ethanol na 0,1 M (C2H5OH) baya gudanar da wutar lantarki?
Tattaunawa:
Maganin ethanol ba shi da sinadarin electrolyte. Ethanol, idan ya narke a cikin ruwa, ba ya rabuwa zuwa ions. Tsarin kwayoyin halittar ethanol yana nan a cikin ruwan. Saboda rashin ions a cikin ruwan, ethanol ba zai iya gudanar da wutar lantarki ba. Saboda haka, kodayake ethanol yana narkewa cikin ruwa cikin sauƙi, saboda babu ions da aka samar, ruwan ethanol ba zai iya gudanar da wutar lantarki ba ko da a kowane taro, gami da 0,1 M.
Kammalawa
Fahimtar halayen ƙarfi na electrolytes, raunin electrolytes, da waɗanda ba electrolytes ba muhimmin tushe ne a cikin sinadaran mafita. Ƙarfin electrolytes suna yin ion a cikin ruwa gaba ɗaya don haka suna gudanar da wutar lantarki da kyau, yayin da raunin electrolytes suna yin ionize kaɗan kawai, wanda ke nuna ƙarancin wutar lantarki. A gefe guda kuma, waɗanda ba electrolytes ba ba sa yin ionize kwata-kwata don haka ba za su iya gudanar da wutar lantarki ba. Fahimtar wannan ra'ayi yana taimaka wa ɗalibai gano mahaɗan dangane da halayensu a cikin mafita da amsa tambayoyin da suka shafi daidai.
