To calculate the alkalinity of a water sample, especially when it is stated that there are no carbonate or other dissolved proton donors or acceptors, we must understand the basic concept of alkalinity and pH.

Alkalinity measures a water sample's ability to neutralize acids, primarily determined by the presence of bicarbonate, carbonate, and hydroxide ions. In this scenario, however, we are informed that there are no significant carbonate or other proton acceptors/donors.

The pH value provided is 9, which indicates that the solution is slightly basic. We will employ the following logic and steps:

1. Understanding pH 9: A pH of 9 suggests a concentration of hydroxide ions, as pH > 7 indicates a basic solution. Therefore, the hydroxide ion (\( \text{OH}^- \)) concentration is: \([\text{OH}^-] = 10^{-(14 - pH)} = 10^{-(14 - 9)} = 10^{-5}\, \text{mol L}^{-1}\).
2. Alkalinity in the context of pH and absence of carbonate:
   • Since we have no carbonates or bicarbonates, the alkalinity in this case will solely be from the hydroxide ions present.
   • The actual measurement of alkalinity is expressed in terms of calcium carbonate (CaCO₃) equivalent, but given the absence of significant contributors, it simplifies the situation.
3. Considerations: 
   • The problem specifies no other dissolved proton donors or acceptors, hinting at very pure, deionized conditions apart from the basic nature (pH 9).
   • Even with the hydroxide presence, the calculation may yield minimal measurable alkalinity.
4. Conclusion: Given the absence of typical alkalinity-contributing species, the alkalinity of the water sample should be very close to zero, given that significant contributors (bicarbonates/carbonates) and effects have been removed.

Therefore, the solution confirms that the alkalinity is approximately \(\sim 0 \, \mu \text{mol L}^{-1}\).