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JpiPQUESTiON 20Howmany of the following species are Is amphoteric? HPO4 HzoHSO4-HCO;HJPOHHCHH;O2SO32QUESTION 21Which of the following #olutions %s good buffer syste...

Question

JpiPQUESTiON 20Howmany of the following species are Is amphoteric? HPO4 HzoHSO4-HCO;HJPOHHCHH;O2SO32QUESTION 21Which of the following #olutions %s good buffer system? Asclution that i5 130 M HBr and 0.90 M KBr solution that H| 1090 MHl and 90 MNHT Fsolution thal [90 MHI ad 0.050 MNH + Eolution that = 1280 MNaOH and 980 MKOH Ajolution that 650 M HF and 0.6S0MLiF solution that E 730 M HBr and 5 -730 MKBr solution thar E OOSO MHF and OOS0MLiF

JpiP QUESTiON 20 Howmany of the following species are Is amphoteric? HPO4 Hzo HSO4- HCO; HJPOH HCHH;O2 SO32 QUESTION 21 Which of the following #olutions %s good buffer system? Asclution that i5 130 M HBr and 0.90 M KBr solution that H| 1090 MHl and 90 MNHT Fsolution thal [90 MHI ad 0.050 MNH + Eolution that = 1280 MNaOH and 980 MKOH Ajolution that 650 M HF and 0.6S0MLiF solution that E 730 M HBr and 5 -730 MKBr solution thar E OOSO MHF and OOS0MLiF



Answers

Indicate which of the following aqueous solutions are buffer solutions, and explain your reasoning. [Hint: Consider any reactions that might occur between solution components.] (a) $0.100 \mathrm{M} \mathrm{NaCl}$ (b) $0.100 \mathrm{M} \mathrm{NaCl}-0.100 \mathrm{M} \mathrm{NH}_{4} \mathrm{Cl}$ (c) $0.100 \mathrm{M} \mathrm{CH}_{3} \mathrm{NH}_{2}-0.150 \mathrm{M} \mathrm{CH}_{3} \mathrm{NH}_{3}^{+} \mathrm{Cl}^{-}$ (d) $0.100 \mathrm{M} \mathrm{HCl}-0.050 \mathrm{M} \mathrm{NaNO}_{2}$ (e) $0.100 \mathrm{M} \mathrm{HCl}-0.200 \mathrm{M} \mathrm{NaCH}_{3} \mathrm{COO}$ (f) $0.100 \mathrm{M} \mathrm{CH}_{3} \mathrm{COOH}-0.125 \mathrm{M} \mathrm{NaCH}_{3} \mathrm{CH}_{2} \mathrm{COO}$

For it to be a buffer solution. We need to have a weak acid with its conjugate base. So for the first one, we have a strong asset HBR and another week asset. H o B r. So this is not a buffer solution for B. We have a strong acid hcl 04 and a strong base rubidium hydroxide. So this is not a buffer solution for see, we have a weak acid. H o C l and we have It's conjugal base. Oh, C l minus. So this is a buffer. Then we have potassium hydroxide, a strong base, and we have a weak acid. H o N two. So this is not a buffer. And for the last one, we have a weak base. H two n n O h two and we have its conjugate acid h two and O H three plus. So this is a buffer. We can have a weak acid with its conjugate base, or we can have a weak base with its conjugate acid

So here we are calculating the pH of several different strong acids. So if we have a strong acid, the concentration of the strong acid is equal to the concentration of the H plus. So in the first example eight plus, it's equal to 1.21 times. Turn to the minus three, but pH is equal to negative log 1.2 long times 10 to the minus three. PH is equal to 2.918 so we can take a look at the next example here in part B. So the H Plus is equal to 1.99 times 10 to the minus four Moloch. The pH is equal to the negative log of 1.99 times 10 to the minus four Moloch pH is equal to 3.702 So in part C, here we have eight plus concentration. That's equal to 5.1 times 10 the minus five mola. So the pH is equal to negative log of 5.1 times 10 to the minus five mola, so the pH is equal to 4.301 In the final example in party. Each plus is equal to 1.4 times 10 to the minus three molar. So the pH is equal to the negative log of 1.4 times 10 to the minus three mola, so the pH is equal to 2.983

To prepare a buffer solution with A With a ph of nine, we need a weak acid that has a PKK close to nine and its conjugate base. The week at Acid, with a PK close to nine is H B R O, and its conjugate base would be n a O B r.

This question asks us to identify some buffer solutions. So we have to know that a buffer solution is a mixture of either a weak acid with its conjugate base or a weak base with its conjugate acid. And so that's what we're going to be looking for in each of the choices below. So the first choice here gives us a strong acid. Hydrochloric acid is a strong acid and we can basically stop right there because again it has to be a weak acid to be part of a buffer solution. So this is not a buffer. The answer is no. And in addition to that um even if this were a weak acid, noticed that the um conjugate base if it is that we're here is actually another acid, it's hippopotamus acid. Um we would need to have the bromide ion present as the conjugate base here. So that's not even the right conjugate base and in fact it's another acid for so for a couple of reasons this is not a buffer solution. The next answer choice uses per caloric acid. This again is a strong acid and um it's a mixture of that. Again it would have to be the conjugate base, the per chlorate ion that would be mixed in even if this were a weak acid and it's not it's a strong base here, rabb idiom hydroxide. So neither of the components involved here is correct and this too is not a buffer solution. Now answer choice B this is hypochlorite assassin. So yes this is a weak acid And its conjugate base is going to be the O. c. -1 which is the hypochlorite ion. And look here it is right. It's furnished here as an anti on with potassium. So yes we have relatively equal concentrations of a weak acid with its conjugate base. This then would be above her solution. Answer choice D. This is a strong base. Okay? And in addition the acid the week um are conjugate acid from this would have to be water. Remember conjugate acids and bases only ever differ by a proton. So this is an amino compound which isn't even you know related to um the strong base hydroxide. And for both of those reasons again we need to have a weak base and its conjugate acid. We don't have either of those things here. So the answer tries. D. Is also not a buffer. The final answer choice here has hydrazine. This is a weak base. Okay so we need its conjugate acid to be present. So the conjugate acid would have one more proton. Then the hydrazine has here it is right here, right. The formula is the same except it has an extra proton. She'll give it a positive charge. The nitrate ion is here to help place it in solution as an ionic compound. When this dissociates from nitrate ions. Indeed we will have the conjugate acid of hydrazine being present along with its weak base. This then is a buffer solution


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