M = moles/liter
100 ml = 0.1 liter
so 0.01 mole NaOH / 0.1 liter = .1 M NaOH
you can find how many grams of NaOH in .01 moles by multiplying .01 by the atomic weight of a mole of NaOH, which you can find by adding up the atomic weight of Na, and O, and H.
0.1 M Ca(OH)2 = 0.1 mol/L = 0.01 mol/100mL = 0.01(mol/100mL) * 74.093(g/mol) = 0.74 g/100mL Ca(OH)2
Molarity = moles of solute/Liters of solution ( 300.0 ml = 0.300 liters ) ( Ca(OH)2 is correct formulation ) 0.115 M Ca(OH)2 = moles Ca(OH)2/0.300 Liters = 0.0345 moles Ca(OH)2 (74.096 grams/1 mole Ca(OH)2) = 2.56 grams of Ca(OH)2 needed
The needed mass is 35,549 g.
The answer is 6,71 g dried KCl.
30 grams
160 g (solution) - [5/100*160] g (solute) = 152 g (solvent) water
Molarity = moles of solute/Liters of solution ( 300.0 ml = 0.300 liters ) ( Ca(OH)2 is correct formulation ) 0.115 M Ca(OH)2 = moles Ca(OH)2/0.300 Liters = 0.0345 moles Ca(OH)2 (74.096 grams/1 mole Ca(OH)2) = 2.56 grams of Ca(OH)2 needed
1.17 grams :)
The needed mass is 35,549 g.
See the two Related Questions to the left for the answer.The first is how to prepare a solution starting with a solid substance (and dissolving it). The second question is how to prepare a solution by diluting another solution.
The answer is 6,71 g dried KCl.
600 mL of 0,9 % sodium chloride: 6 x 0,9 = 5,4 grams NaCl
Molarity = moles of solute/Liters of solution 0.75 M KCl = moles KCl/2.25 Liters = 1.6875 moles KCl (74.55 grams/1 mole KCl) = 126 grams of KCl needed
30 grams
160 g (solution) - [5/100*160] g (solute) = 152 g (solvent) water
4314.9 grams
28 gram. = 2 * 56 * 250 / 1000
8.9g