Tusaale Su'aalaha Doodda Aashitada ee Brønsted-Lowry
Asiidhyada iyo saldhigyadu waa fikrado muhiim ah oo ku saabsan kiimikada oo ay soo saareen saynisyahano badan sannado badan. Mid ka mid ah aragtiyaha ugu caansan waa aragtida Brønsted-Lowry, oo ay soo jeediyeen Johannes Nicolaus Brønsted iyo Thomas Martin Lowry sannadkii 1923. Aragtidani waxay bixisaa aragti ballaaran oo ku saabsan sida asiidhyada iyo saldhigyadu u falgalaan falgallada kiimikada. Maqaalkan, waxaan ka wada hadli doonnaa dhowr tusaale oo dhibaatooyin ah oo la xiriira fikradda Brønsted-Lowry ee asiidhyada iyo saldhigyada iyo sida loo xalliyo.
Fikradaha Aasaasiga ah ee Asiidhyada iyo Salka Brønsted-Lowry
Sida laga soo xigtay aragtida Brønsted-Lowry, aashitadu waa walax ku deeqi karta proton (H+), halka saldhigu yahay walax aqbali karta proton. Falgallada kiimikada, aashitadu iyo saldhigyadu waxay is dhexgalaan iyada oo loo marayo habka wareejinta proton, halkaas oo hal isku-dhafan uu u dhaqmo sidii aashito isagoo sii deynaya proton, kan kalena uu u dhaqmo sidii saldhig isagoo aqbalaya proton.
Tusaalooyinka Falcelinta Aashitada-Saldhigga
Tusaale ahaan falgal fudud oo u dhexeeya aashito iyo saldhig sida waafaqsan aragtida Brønsted-Lowry waa falgalka u dhexeeya copper(II) sulfate (H2SO4) iyo sodium hydroxide (NaOH):
\[ \text{H}_2\text{SO}_4 + \text{NaOH} \rightarrow \text{NaHSO}_4 + \text{H}_2\text{O} \]
Falgalkan, asiidhka sulfuric (H2SO4) wuxuu u dhaqmaa sidii asiidh Brønsted-Lowry ah sababtoo ah wuxuu ku deeqaa proton (H+) saldhigga NaOH, kaas oo aqbala proton-ka.
Su'aalo iyo Doodo Tusaale ah
Su'aal 1aad: Aqoonsashada Asiidhyada iyo Salka
Su'aal:
Soo ogow asiidhyada iyo saldhigyada Brønsted-Lowry ee falcelinta soo socota:
\[ \text{NH}_3 + \text{H}_2\text{O} \rightarrow \text{NH}_4^+ + \text{OH}^- \]
Dood:
Falgalkan, ammonia (NH3) iyo biyaha (H2O) ayaa ah falgalayaasha, halka ammonium ions (NH4+) iyo hydroxide ions (OH-) ay yihiin waxyaabaha la soo saaray. Aan aragno midka u shaqeeya sidii aashito iyo kan u shaqeeya sidii saldhig.
– NH3 waxay u dhaqantaa sidii saldhig sababtoo ah waxay aqbashaa protons (H+) laga bilaabo H2O si ay u sameeyaan NH4+.
– H2O wuxuu u dhaqmaa sidii asiidh sababtoo ah wuxuu ku deeqaa proton (H+) NH3 si uu u sameeyo OH-.
Markaa, falcelintan:
– NH3 waa saldhig Brønsted-Lowry ah.
– H2O waa aashitada Brønsted-Lowry.
Su'aal 2: Qorista Falcelinta Isku-xidhka
Su'aal:
Qor lammaanayaasha aashitada isku xiran ee falcelinta soo socota:
\[ \text{HCl} + \text{H}_2\text{O} \rightarrow \text{H}_3\text{O}^+ + \text{Cl}^- \]
Dood:
Falcelintan, HCl wuxuu u dhaqmaa sidii aashitada Brønsted-Lowry isagoo ku deeqaya proton (H+) H2O. Biyuhu (H2O) waxay aqbalaan proton-ka waxayna u dhaqmaan sidii saldhig Brønsted-Lowry ah. Ka dib markay lumiyaan proton, HCl wuxuu isu beddelaa Cl-, H2O, ka dib markay helaan proton, wuxuu isu beddelaa H3O+.
– Aashitada (HCl) iyo saldhigeeda isku xiran (Cl-)
– Salka (H2O) iyo aashitada isku xiran (H3O+)
Sidaa darteed, lammaanaha aashitada isku dhafan ee falgalkan waa:
– HCl / Cl-
– H2O / H3O+
Su'aal 3: Xisaabinta pH-ga ee Xalka Aashitada Daciifka ah
Su'aal:
Xisaabi pH-ga xalka 0.1 M ee aashitada aashitada (CH3COOH) haddii la og yahay in joogtada kala-goynta aashitada (Ka) ay tahay \(1.8 \jeer 10^{-5}\).
Dood:
Asiidhka Acetic waa asiidh daciif ah, biyahana qayb ahaan ayuu u ionizes sida waafaqsan isla'egta soo socota:
\[ \text{CH}_3\text{COOH} \rightleftharpoons \text{CH}_3\text{COO}^- + \text{H}^+ \]
Tallaabooyinka lagu xisaabinayo pH waa sida soo socota:
1. Deji muujinta dheelitirka adoo isticmaalaya fiirsashada bilowga ah iyo isbeddelka fiirsashada:
\[ \text{Ka} = \frac{[\text{CH}_3\text{COO}^-][\text{H}^+]}{[\text{CH}_3\text{COOH}]} \]
2. Ku beddel qiimayaasha la yaqaan oo u xalli \([H^+]\):
\[ 1.8 \jeer 10^{-5} = \frac{x^2}{0.1 – x} \]
Maadaama \(x\) uu aad u yar yahay marka la barbar dhigo 0.1, waxaan qiyaasi karnaa \(0.1 - x \qiyaastii 0.1\):
\[ 1.8 \jeer 10^{-5} = \frac{x^2}{0.1} \]
\[ x^2 = 1.8 \jeer 10^{-6} \]
\[ x = \sqrt{1.8 \jeer 10^{-6}} \]
\[ x \qiyaastii 1.34 \jeer 10^{-3} \]
3. Xisaabi pH-ga:
\[ \text{pH} = -\log[\text{H}^+] \]
\[ \text{pH} = -\log(1.34 \times 10^{-3}) \]
\[ \text{pH} \qiyaastii 2.87 \]
Markaa, pH-ga xalka aashitada aashitada 0.1 M waa qiyaastii 2.87.
Su'aal 4: Aqoonsiga Xalalka Amphiprotic
Su'aal:
Soo hel xalka amphiprotic-ga falcelinta soo socota oo sharax sababta:
\[ \text{HCO}_3^- + \text{H}_2\text{O} \rightleftharpoons \text{H}_2\text{CO}_3 + \text{OH}^- \]
Dood:
Xalka amphiprotic waa xal u dhaqmi kara sidii asiidh ama saldhig, iyadoo ku xiran xaaladaha falgalka. Falcelinta tusaalaha kore:
– \(\text{HCO}_3^-\) wuxuu u dhaqmaa saldhig marka uu aqbalo proton ka yimid \(\text{H}_2\text{O}\), isagoo soo saaraya \(\text{H}_2\text{CO}_3\).
– \(\text{HCO}_3^-\) sidoo kale wuxuu u dhaqmi karaa sidii asiidh xaalado kale, isagoo sii deynaya proton oo soo saaraya \(\text{CO}_3^{2-}\).
Tani waxay muujinaysaa in ion-ka \(\text{HCO}_3^-\) uu yahay amphiprotic. Waxay u dhaqmi kartaa sidii aashito (deeq-bixiye proton) iyo saldhig (aqbale proton ah), iyadoo ku xiran walaxda kale ee ay la falgasho.
Dhibaatooyinkan tusaalaha ah awgood, waxaan si fiican u fahmi karnaa sida aragtida salka aashitada Brønsted-Lowry loogu isticmaalo falanqaynta iyo saadaalinta isdhexgalka kiimikada. Faham adag oo ku saabsan aragtidan ayaa ah aasaaska codsiyada badan ee kiimikada, bayoolajiga, iyo cilmiga kale.
