Consider a buffered solution containing CH_3NH_3CI and CH_3NH_2. Which of the fo

Question

Consider a buffered solution containing CH_3NH_3CI and CH_3NH_2. Which of the following statements are line concerning this solution? (K_a for CH_3NH_3^+ = 2.2 times 10^-11). (Select all that apply.) If [CH_3NH_2] - [CH_3NH_3^+], then pH = 10.64 If NaOH were added to the initial buffered solution, then the (CH_3NH_2) would increase. A solution consisting of 0 10. M CH_3NH_3C1 and 0.10 MCH_3NH_2 would have a higher capacity than one containing 1.0 MCH_3NH3_CI and 1.0 MCH_3 NH_2. Adding more [CH_3NH_3CI] lo the initial bullet solution will decrease the pH. If [CH_3NH_2]

Explanation / Answer

pKa = - logKa = - Log (2.2*10-11) = 10.66

pH = pKa + Log[Salt]/[Base]

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* If [CH3NH2] = [CH3NH3Cl], pH = 10.64   TRUE

* If NaOH wer added to initial buffer [CH3NH2] would incease. TRUE

Becasue it reacts with salt to form base. CH3NH3Cl + NaOH ----> CH3NH2 + NaCl + H2O

* FALSE. Because same is concentration of salt and base, the capacity of buffer is same.

* FALSE because Adding salt increase the pH.      

* FALSE

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