What would one have to do differently if they used NaMnO4 instead of KMnO4 for redox titrations? I am doing a chemistry report related to redox titrations (using $\ce{KMnO4}$ as the titrant), and one section of the report asks me to explain what would occur if I were to use sodium permanganate ($\ce{NaMnO4}$) instead of potassium permanganate ($\ce{KMnO4}$), and more importantly, what I would have to do differently in my experiment if I were to use this new chemical.

What I know as of now.


Sodium permanganate is not widely used because it is more expensive and is much more difficult to create than potassium permanganate. 
Molar mass is different when performing stoichiometric equations, which leads to different results when calculating certain values. 


I looked online and found that the chemical is "hygroscopic;" however, I don't know if this changes anything in the experiment.

Is there anything else I can "change" in my experiment if I were to use $\ce{NaMnO4}$ instead of $\ce{KMnO4}$?
You are right. Preparing sodium permanganate is more expensive. The second reason is, sodium permanganate is hygroscopic and occurs as a monohydrate. This means that sodium permanganate is more soluble than potassium permanganate. (Solubility of $\ce{KMnO_4}$ is $0.065$ g/ml and that of $\ce{NaMnO_4}$ is $0.9$ g/ml)

So if you require a larger concentration of $\ce{MnO_4^-}$ in the solution, you can go for $\ce{NaMnO_4}$.