Depends on how you measure your 35% - 35% w/w or 35% w/v.
Also whether you are measuring US gal or Imperial Gal. And what form of calcium chloride you are starting with (fused anhydrous or dihydrate are the two common ones)
Easier to work in litres -
200 gal imperial is about 900 litres.
Density of 35%w/w is around 1.357 @ 25°C so 1 litre of finished 35% w/w CaCl2 solution weighs 1.357 kg.
900 lt of 35%w/w weighs 900 * 1.357 = 1221kg
amount of CaCl2 (anhydrous - 100%) required = 1221 * .35 kg
= 428 kg
Molarity = moles of solute/Liters of solution 0.320 M CaCl2 = moles CaCl2/4.5 Liters = 1.44 moles of CaCl2 1.44 moles CaCl2 (110.978 grams/ 1 mole CaCl2) = 159.81 grams needed so, considering the sigi figis, 160 grams needed.
Dissolve 111 g anhydrous CaCl2 in 1 L distilled water.
Molarity is probably the most commonly used unit of concentration. It is the number of moles of solute per liter of solution (not necessarily the same as the volume of solvent!). Example: What is the molarity of a solution made when water is added to 11 g CaCl2 to make 100 mL of solution? Solution: 11 g CaCl2 / (110 g CaCl2 / mol CaCl2) = 0.10 mol CaCl2 100 mL x 1 L / 1000 mL = 0.10 L molarity = 0.10 mol / 0.10 L molarity = 1.0 M http://chemistry.about.com/od/lecturenotesl3/a/concentration.htm http://www.tpub.com/content/MIL-SPEC/MIL-P/MIL-P-71158/MIL-P-7115800013.htm http://www.tpub.com/content/armymedical/md0837/md08370139.htm
(x L)((12%) = (100 L)(2%)x = 16.7 liters
About 80ml of water must be added to 40ml of a 25 percent by weight solution to make a 2 percent by weight solution.
Molarity = moles of solute/Liters of solution 0.320 M CaCl2 = moles CaCl2/4.5 Liters = 1.44 moles of CaCl2 1.44 moles CaCl2 (110.978 grams/ 1 mole CaCl2) = 159.81 grams needed so, considering the sigi figis, 160 grams needed.
4.84
144liters
50liters
256 liters
50 liters
50
50 Liters of the 60% solution.
Dissolve 111 g anhydrous CaCl2 in 1 L distilled water.
The volume is 0,3 mL.
A. 16 of 18 percent and 2 of 9 percent b. 14 of 18 percent and 4 of 9 percent c. 16 of 9 percent and 2 of 18 percent d. 14 of 9 percent and 4 of 18 percent
Molarity is probably the most commonly used unit of concentration. It is the number of moles of solute per liter of solution (not necessarily the same as the volume of solvent!). Example: What is the molarity of a solution made when water is added to 11 g CaCl2 to make 100 mL of solution? Solution: 11 g CaCl2 / (110 g CaCl2 / mol CaCl2) = 0.10 mol CaCl2 100 mL x 1 L / 1000 mL = 0.10 L molarity = 0.10 mol / 0.10 L molarity = 1.0 M http://chemistry.about.com/od/lecturenotesl3/a/concentration.htm http://www.tpub.com/content/MIL-SPEC/MIL-P/MIL-P-71158/MIL-P-7115800013.htm http://www.tpub.com/content/armymedical/md0837/md08370139.htm