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A solution contains 1.20 g of CaCl2 and 240 mL of solution what is the percent w-v concentration of the solution?
Wiki User
∙ 13y ago
W-V percent concentration
g/mL = 1.20g/240mL = 0.005 g/mL percent
Wiki User
∙ 13y ago
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What is the final concentration of cl- ion when 250 ml of 0.20 M cacl2 solution is mixed with 250 ml of 0.40 M kcl solution?
.01 M
Which solution turns cloudy when it react with a gas?
i)NaOH + FeCl3 ii) Na2CO3 + CaCl2
How does CaCl2 exhibit deliquescence?
Calcium chloride can absorb very much water and become a solution.
How much CaCl2.6H2O and water must be weighed to prepare 100g of a solution that is 5 percent CaCl2?
do you mean 100 ml? most solutions are given in terms of volume not mass. But ...CaCl2 has a molar mass of 111 g The hydrated form also contains 108 g water. This gives a total mass of 219 g for the hydrated form.The solution must contain: 100 g x 5% = 100 x 5/100 = 5g anhydrous CaCl25 / x = 111 / 219solve for x: x = 5(219)/111 = 9.865 g of the hydrate
What is the molarity of a solution that has 6 mol of CaCl2 in 3 kg of water?
The molarity is 2 mol/L.
What is the concentration of a solution which contains 1 mole of CaCl2 dissolved in 2000 milliliters of solution?
1.00 m
What is the percent mv of a water solution that contains 60 g of calcium chloride CaCl2 and that has a volume of 400 mL?
The percent mv is 6.7%.
How many moles of solutes in 2.10 ml CaCl2?
This depends of the concentration of CaCl2 in this solution.
What concentration of aqueous CaCl2 solution freezes at -10.2ºC?
1.83m
A solution contains 1.20 g of CaCl2 and 240 mL of solution what is the percent w-w concentration of the solution if the solution has a density of 1.13 g-mL?
Volume of solution=V=240ml . Density of solution=d=1.13g/ml. Mass of solution=V*d=240*1.13=271.2g . Mass of solute=1.20g . PERCANTAGE W/W = 1.20/271.2*100=0.44%
How many moles of CaCl2 are in 250 ml of CaCl2 solution?
It depends on the concentration of the solution. If you know the concentration(molarity) then use the equation. moles = [conc] x vol(mL) / 1000 NB The '1000' isusedto convert the concentration units of moles per litre (molL^-1) to mL.
What is the concentration of chloride ion in a 2.0M solution of calcium chloride?
CaCL2 on its own cannot have a concentration. It would have to be dissolved in a solution first. Then, from the amount of CaCl2 which is dissolved in a certain amount of a solute (such as water), you would be able to figure out the concentration.
What is the concentration of nitric acid in moles per liter in a sample which has density 1.41gm per ml and the mass percent of nitric acid is 69 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
What concentration of aqueous CaCl2 solution freezes at -10.2ºC. The freezing point of pure water is 0.0ºC and Kf of pure water is -1.86ºCm?
1.83m No srsly, it is. CaCl2 dissociates to form three ions.
What is the final concentration of cl- ion when 250 ml of 0.20 M cacl2 solution is mixed with 250 ml of 0.40 M kcl solution?
.01 M
What is the molarity of a CaCl2 solution containing 330 grams of CaCl2 in 1 liter of solution?
The molarity is 2,973.
How many grams of CaCl2 are needed to prepare 2.00 l if 0.700 M CaCl2 solution?
The gram formula mass of CaCl2 is 110.99. By definition, each liter of 0.700 M CaCl2 contains 0.700 gram formula masses of the solute. Therefore, 2.00 liters of such solution contain 1.400 formula masses of the solute, or 155 grams, to the justified number of significant digits.
