## Answer:

Yes, the chemistry graduate student should dissolve 0.323 moles of CH,NH,Cl in the 1.30M methylamine (CH,NH,) solution in order to turn it into a buffer with pH = 11.01. This can be determined using the Henderson-Hasselbalch equation.

## Supporting Subsections

### Henderson-Hasselbalch Equation

The Henderson-Hasselbalch equation is used to calculate the pH of a buffer solution. It can be written as pH = pK_{a} + log([A^{–}]/[HA]).

### Calculating the Desired Amount of CH,NH,Cl

In order to turn the 1.30M methylamine (CH,NH,) solution into a buffer with pH = 11.01, we need to calculate the amount of CH,NH,Cl that needs to be dissolved. This can be done by rearranging the Henderson-Hasselbalch equation to [A^{–}]/[HA] = 10^{pH-pKa}. Plugging in the given information, we get [A^{–}]/[HA] = 10^{11.01 – 10.75} = 10^{0.26}. We can then calculate the amount of CH,NH,Cl needed by multiplying the [A^{–}]/[HA] ratio by the number of moles of CH,NH, in the solution (1.30 moles). This gives us 0.323 moles of CH,NH,Cl.

### Volume of the Solution

Assuming the volume of the solution does not change when the CH,NH,Cl is added, we can calculate the total volume of the solution by adding the volume of the CH,NH,Cl to the original volume of the solution. This gives us 250.0 + 0.323 = 250.323 ml.

### Final Answer

The final answer is that the chemistry graduate student should dissolve 0.323 moles of CH,NH,Cl in the 1.30M methylamine (CH,NH,) solution in order to turn it into a buffer with pH = 11.01. This will result in a total volume of 250.323 ml.

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