Which would have the higher osmotic pressure: a 0.10 m solution of nacl or a 0.10 m solution of kbr?

Osmotic pressure is calculated by multiplying the molarity, temperature and the universal gas constant. It is expressed as:

P = iMRT

Say the temperature for both solutions is 373.15 K.

P(NaCl) = 2 x 0.10 x 0.08206 x 373.15 = 3.06 atm
P(KBr) = 2 x 0.10 x 0.08206 x 373.15 = 3.06 atm

They will have the same osmotic pressure since they have the same concentration, dissociate into 2 ions and at the same temperature.

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