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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?
To find the final concentration of Cl- ions, first calculate the moles of Cl- ions from each solution. Then add the moles of Cl- ions from both solutions and divide by the total volume of the mixed solution (500 ml) to get the final concentration. Using the formula C1V1 = C2V2 where C represents concentration and V represents volume, you can determine the moles of Cl- ions from each 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
How does CaCl2 exhibit deliquescence?
CaCl2 is deliquescent because it absorbs water vapor from the air to form a solution, ultimately dissolving in the absorbed water. This process occurs because CaCl2 has a high affinity for water molecules, leading to its ability to attract and retain moisture from the surrounding environment.
What is the molarity of a solution that has 6 mol of CaCl2 in 3 kg of water?
The molarity is 2 mol/L.
How many moles of CaCl2 contains 1.26 times 10 24 formula units CaCI2?
The answer is 2,09 moles.
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?
To calculate the percent mass/volume (m/v) of the solution, you would divide the mass of the solute (CaCl2) by the volume of the solution and then multiply by 100. In this case, the mass of CaCl2 is 60 g and the volume of the solution is 400 mL. So, the percent m/v would be (60g/400mL) x 100 = 15% m/v.
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?
First, find the total mass of the solution by multiplying the density (1.13 g/mL) by the volume (240 mL). This gives 271.2 g. Now, calculate the percent concentration of CaCl2 in the solution by dividing the mass of CaCl2 (1.20 g) by the total mass of the solution (271.2 g) and multiplying by 100. The percent w/w concentration of the solution is approximately 0.44%.
How many moles of solutes in 2.10 ml CaCl2?
This depends of the concentration of CaCl2 in this solution.
What is the concentration of a solution which contains 1 mole of CaCl2 dissolved in 2000 milliliters of solution?
The concentration of the solution is 0.5 mol/L, which is equivalent to 0.5 M. This is calculated by dividing the number of moles of solute by the volume of solution in liters.
What concentration of aqueous CaCl2 solution freezes at -10.2ºC?
1.83m
How many moles of CaCl2 are in 250 ml of CaCl2 solution?
To determine the number of moles of CaCl2 in a solution, you need to know the concentration of the solution in mol/L. Without this information, it is not possible to calculate the number of moles of CaCl2 in the given volume of 250 ml.
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 concentration of chloride ion in a 2.0M solution of calcium chloride?
The concentration of chloride ion in a 2.0M solution of calcium chloride would be 4.0M. This is because calcium chloride dissociates into one calcium ion and two chloride ions in solution. Therefore, the concentration of chloride ions is double the concentration of the calcium chloride solution.
What mass of CaCL2 is needed to prepare 2.850 L of a 1.56 M solution?
To find the mass of CaCl2 needed, you need to use the formula: Mass = molarity × volume × molar mass. First, calculate the number of moles of CaCl2 using the molarity and volume. Then, multiply the moles by the molar mass of CaCl2 (110.98 g/mol) to find the mass needed. A 1.56 M solution means it contains 1.56 moles of CaCl2 in 1 liter of solution.
If 3.0 mol of CaCl2 are added to water to make 0.500L of solution what is the concentration in molarity?
The molarity of the CaCl2 solution is 6.0 M. This is calculated by dividing the number of moles of CaCl2 (3.0 mol) by the volume of the solution in liters (0.500 L).
Molarity of CL in 110 ml of a solution containing 5.55g of CaCl2?
To find the molarity of Cl in the solution, first calculate the number of moles of CaCl2 using its molar mass. Then, since each formula unit of CaCl2 contains 2 moles of Cl, multiply the moles of CaCl2 by 2 to get moles of Cl. Finally, divide moles of Cl by the volume of the solution in liters to find the molarity.
How many grams of CaCl2 are needed to prepare 2.00 l if 0.700 M CaCl2 solution?
To prepare a 0.700 M solution of CaCl2 in 2.00 L of solution, you would need 2.00 L * 0.700 mol/L = 1.40 moles of CaCl2. With the molar mass of CaCl2 being 110.98 g/mol, you would need 1.40 moles * 110.98 g/mol ≈ 155.37 grams of CaCl2.
