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Question Which one 0f / the 9 following 'buffer ! statements Is an 'True? aqucous = The solutlon , common composed C 'Ion In a '0( (o = bull...

Question

Question Which one 0f / the 9 following 'buffer ! statements Is an 'True? aqucous = The solutlon , common composed C 'Ion In a '0( (o = buller 'weak acids; soluuon buller E does = Tesists [ not / pH have change any eliea ( on lhe t nculrali/ana - Ulssechuon d Ud *e bufler {edded acida und batcs Oetnt docs nol change ! pH when ' lurge ' AnUnls 0/ 0 Wiong buffer can absorb = ecuor 4to1t unlimilcd bas Drdukd amount of ncid or base .QUESTION 5Which of the

Question Which one 0f / the 9 following 'buffer ! statements Is an 'True? aqucous = The solutlon , common composed C 'Ion In a '0( (o = buller 'weak acids; soluuon buller E does = Tesists [ not / pH have change any eliea ( on lhe t nculrali/ana - Ulssechuon d Ud *e bufler {edded acida und batcs Oetnt docs nol change ! pH when ' lurge ' AnUnls 0/ 0 Wiong buffer can absorb = ecuor 4to1t unlimilcd bas Drdukd amount of ncid or base . QUESTION 5 Which of the following is the cOnect cqualion relating Q to Kip lor w cquilibnam [cacpon Q < Ksp Q > Ksp Q = Ksp



Answers

Consider a buffered solution containing $\mathrm{CH}_{3} \mathrm{NH}_{3} \mathrm{Cl}$ and $\mathrm{CH}_{3} \mathrm{NH}_{2}$ . Which of the following statements concerning this
solution is(are) true? $\left(K_{\mathrm{a}} \text { for } \mathrm{CH}_{3} \mathrm{NH}_{3}+=2.3 \times 10^{-11}\right)$
a. A solution consisting of 0.10$M \mathrm{CH}_{3} \mathrm{NH}_{3} \mathrm{Cl}$ and 0.10 $\mathrm{M}$ $\mathrm{CH}_{3} \mathrm{NH}_{2}$ would have a greater buffering capacity than one
containing 1.0 $\mathrm{M} \mathrm{CH}_{3} \mathrm{NH}_{3} \mathrm{Cl}$ and 1.0 $\mathrm{M} \mathrm{CH}_{3} \mathrm{NH}_{2}$
b. If $\left[\mathrm{CH}_{3} \mathrm{NH}_{2}\right]>\left[\mathrm{CH}_{3} \mathrm{NH}_{3}^{+}\right],$ then the $\mathrm{pH}$ is larger than the $\mathrm{p} K_{\mathrm{a}}$ value.
c. Adding more $\left[\mathrm{CH}_{3} \mathrm{NH}_{3} \mathrm{Cl}\right]$ to the initial buffer solution
will decrease the pH.
d. If $\left[\mathrm{CH}_{3} \mathrm{NH}_{2}\right]<\left[\mathrm{CH}_{3} \mathrm{NH}_{3}^{+}\right],$ then $\mathrm{pH}<3.36$
e. If $\left[\mathrm{CH}_{3} \mathrm{NH}_{2}\right]=\left[\mathrm{CH}_{3} \mathrm{NH}_{3}^{+}\right],$ then $\mathrm{pH}=10.64$

The first statement, a solution consisting of 0.1 Moeller of the A weak acid and 0.1 Moeller of the week base is gonna have a higher buffer capacity than a one Moeller and a one Moeller. Concentration of the weak acid in its conjugate base is false because higher concentrations of the buffering species always results in higher buffer capacity, not lower concentrations. The next statement, if the base concentration is greater than the acid concentration than the pH, is larger than Piquet. This is true when those two concentrations are equal. PH equals P K. And then if we, ADM or base PH always increases with more base. So true for the next one. Adding mawr of the acid to the initial buffer will decrease the pH. This is true. Adding more acid always decreases the pH for the next one. It asks if we have concentration of the base less than the concentration of the acid than pH is less than 3.36 Well, peek A is the negative log of 2.3 times 10 to the negative 11 which is 10.64 So if we have Mawr base, I'm sorry for Part D. If we have more acid, then we can comfortably state that the pH is going to be less than Piquet at 10.64 But it's unlikely that we're gonna have so much more acid that the pH is going to be less than 3.36 So this is false, but we could say that it's less than 10.64 and then the last one. If the two concentrations are equal, pH equals the PK PK being 10.64 is true.

Okay. So for part A If I have a form eight ion concentration and I want to compare it as coming from sodium for mate And if this is .1 moller Then the concentration of the Form eight ion Is going to be .1 moller what if it's coming from formic acid, Right was .1 Moller This concentration is going to be much much less than .1 Mueller because weak acids only ionized a little bit. So this statement is false and you could fix it simply by saying that the concentration is much less than rather than equal to. Okay, so I would say less than rather than equal to in that statement. So we've got a buffer and we're going to take our buffer and we're going to add a whole bunch of strong acid. So a buffer is made of a weak acid and a weak base. So what happens if you add too much strong acid then it completely removes all of the week base and all you're left with is weak acid. So you no longer have a buffer, you just have a weak acid. So this statement is true. Okay, when we want to make a buffer, Okay, so buffers or approximately equal amounts of a weak acid and specifically its conjugate weak base. So that statement needs a little bit of help. So as written it was false. Mhm. This last statement is also true. Okay, so let's rewrite it. So because the K. A. Or bicarbonate, is this? That means that the KB not for bicarbonate but for carbonate Is one time Santa -14 over that value. So that's where this 2.1 time send a negative four goes okay so the K and K B have to be a weak acid and conjugate base pair.

Okay. So for part A If I have a form eight ion concentration and I want to compare it as coming from sodium for mate And if this is .1 moller Then the concentration of the Form eight ion Is going to be .1 moller what if it's coming from formic acid, Right was .1 Moller This concentration is going to be much much less than .1 Mueller because weak acids only ionized a little bit. So this statement is false and you could fix it simply by saying that the concentration is much less than rather than equal to. Okay, so I would say less than rather than equal to in that statement. So we've got a buffer and we're going to take our buffer and we're going to add a whole bunch of strong acid. So a buffer is made of a weak acid and a weak base. So what happens if you add too much strong acid then it completely removes all of the week base and all you're left with is weak acid. So you no longer have a buffer, you just have a weak acid. So this statement is true. Okay, when we want to make a buffer, Okay, so buffers or approximately equal amounts of a weak acid and specifically its conjugate weak base. So that statement needs a little bit of help. So as written it was false. Mhm. This last statement is also true. Okay, so let's rewrite it. So because the K. A. Or bicarbonate, is this? That means that the KB not for bicarbonate but for carbonate Is one time Santa -14 over that value. So that's where this 2.1 time send a negative four goes okay so the K and K B have to be a weak acid and conjugate base pair.


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