0.125M x 0.50L= .0625 mol x 118g= 7.4g KBr
Molarity = moles of solute/liters of solution ( 300 ml = 0.300 liter ) 0.250 molar KOH = moles KOH/0.300 liters = 0.075 moles KOH
dissolve iodine crystals in a saturated KI(potassium iodide) solution
Dissolve 50 g of potassium carbonate in 100 mL of water at 20 0C.
Take 10 gm oF KI dissolve it in 100ml.
Crystallisation from solution, flotation, or electrostatic separation from suitable minerals.
105 g
Drabkin's Solution is a mixture of potassium cyanide and potassium ferricyanide. What this solution does is hemolysis red blood cells and then hemoglobin is released.
111.72
Molarity = moles of solute/liters of solution ( 300 ml = 0.300 liter ) 0.250 molar KOH = moles KOH/0.300 liters = 0.075 moles KOH
dissolve iodine crystals in a saturated KI(potassium iodide) solution
pottassium permangate
ask your teacher.
Molarity = moles of solute/liters of solution or, for our purposes moles of solute = liters of solution * Molarity moles of AgNO3 = 0,50 liters * 4.0 M = 2.0 moles of AgNO3 needed --------------------------------------
Dissolve 101.1 g of potassium nitrate in 1 litre of water
it is primary standard........ but before making solution dry it at 120. C
I think this is inappropriate for asking on the Internet.
Dissolve 50 g of potassium carbonate in 100 mL of water at 20 0C.