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
28 gram. = 2 * 56 * 250 / 1000
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
28 gram. = 2 * 56 * 250 / 1000
4314.9 grams
8.9g
400 mls would require 40g of glucose for a 10% solution and thus 20g for a 5% solution.