Question

1. An aqueous solution is made by dissolving 18.0 grams of aluminum iodide in 389 grams of water.
The molality of aluminum iodide in the solution is

2. In the laboratory you are asked to make a 0.406 m barium hydroxide solution using 425 grams of water.
How many grams of barium hydroxide should you add?

3. An aqueous solution is 5.50% by mass ammonia, NH₃, and has a density of 0.975 g/mL.
The molality of ammonia in the solution is

4. An aqueous solution is 36.0% by mass potassium bromide, KBr, and has a density of 1.33 g/mL.
The molality of potassium bromide in the solution is

Answer 1

1 moles of aluminum iodide a mais - log, 0.044 mol - molamals 407-7 g/mol molality = moles of solute 0.044 -0.113m 0.354 kg of solvent molality of aluminum iodide = 0.113 m 7 moles of barium hy dovide a molality & kg of solvent = 0.406x 0.425 - 0.17255 mol mass of barium hydronide moles & molal mass = 0.125TX 171 g/mol - 29.5 gram mass of barium hydwride added = (3) mass of ammonia = 5.5g to mais & Weath = 94.5g moles gammonta a mesta song - 0.323 smo molemass 72g/mol molality a moles 8 solute 013285 --3-42 m. is a solrent - 0.0945 - 2 molality & Whs in the solutions 3.42 m

, mass AK BY 5 36 gii mass of watel a 100-16 2 64g moles of kar mals 1 molal mais 36 g C20-30 mol ligg/mol SENESTE molality = 0.30 -=4.72m moles of solute Kg q solrent 10064 molality 9 BOY a 4-72m