Question

In: Chemistry

A solution is prepared by dissolving 12.36 g of CaCl2 ( an electrolyte, molar mass= 111g)...

A solution is prepared by dissolving 12.36 g of CaCl2 ( an electrolyte, molar mass= 111g) in 135g of H2O ( molar mass =18.0g). The resulting solution has a density of 1.10 g/ml. Calculate the molarity of CaCl2 in the solution.

Solutions

Expert Solution

Total mass = 12.36 g + 135 g = 147.36 g

density = mass / volume
1.10 g/ml = 147.36 / volume
volume = 134 mL
                 = 0.134 L


mass of CaCl2 = 12.36 g
Molar mass of CaCl2 = 111 g
number of moles of CaCl2 = mass / molar mass
                                                      = 12.36/111
                                                      = 0.114 mol

V = 0.134 L

M = number of moles / volume
     = 0.114 / 0.134
     = 0.83 M

Answer: 0.83 M

queen_honey_blossom answered 1 year ago
Next > < Previous

Related Solutions

A solution is prepared by dissolving 23.7 g of CaCl2 in 375 g of water. The...
A solution is prepared by dissolving 23.7 g of CaCl2 in 375 g of water. The density of the resulting solution is The mole fraction of Cl- in this solution is __________ M.
A solution is prepared by dissolving 23.7 g of CaCl2 in 375 g of water. The...
A solution is prepared by dissolving 23.7 g of CaCl2 in 375 g of water. The density of the resulting solution is 1.05 g/mL. The concentration of CaCl2 in this solution is M
A standard FAS solution is prepared by dissolving 0.1221 g of FAS (uncorrected mass) in water...
A standard FAS solution is prepared by dissolving 0.1221 g of FAS (uncorrected mass) in water in an amber bottle. The dry weight of the capped bottle is 256.77 g; the total weight of the bottle plus standard FAS solution is 750.13 g. Calculate the concentration of this solution in mg Fe/g soln. (Note that FAS has a density of 1.86 g/mL and contains 14.24087% Fe.) Then, a calibration standard test solution is made by dispensing 3.8514 g of the...
A. Calculate the mass percent (m/m) of a solution prepared by dissolving 51.22 g of NaCl...
A. Calculate the mass percent (m/m) of a solution prepared by dissolving 51.22 g of NaCl in 151.9 g of H2O. B. Vinegar is a solution of acetic acid in water. If a 265 mL bottle of distilled vinegar contains 19.2 mL of acetic acid, what is the volume percent (v/v) of the solution? C. Calculate the mass/volume percent (m/v) of 20.5 g NaCl in 75.0 mL of solution. D. Calculate the molarity (M) of 155.2 g of H2SO4 in...
A standard iodate solution is prepared at 22.0 °C by dissolving 0.9123 g (uncorrected mass) of...
A standard iodate solution is prepared at 22.0 °C by dissolving 0.9123 g (uncorrected mass) of KIO3 with deionized water in a 499.92 mL volumetric flask. To standardize the Na2S2O3 solution, a 10.005 mL aliquot of the KIO3 solution is acidified, treated with excess KI, and titrated with Na2S2O3, requiring 22.05 mL to reach the end point. Finally, a 10.005 mL aliquot of unknown Cu solution is reduced with excess KI. The liberated iodine requires 31.46 mL of Na2S2O3 solution...
A standard iodate solution is prepared at 22.0 °C by dissolving 0.9123 g (uncorrected mass) of...
A standard iodate solution is prepared at 22.0 °C by dissolving 0.9123 g (uncorrected mass) of KIO3 with deionized water in a 499.92 mL volumetric flask. To standardize the Na2S2O3 solution, a 10.005 mL aliquot of the KIO3 solution is acidified, treated with excess KI, and titrated with Na2S2O3, requiring 22.05 mL to reach the end point. Finally, a 10.005 mL aliquot of unknown Cu solution is reduced with excess KI. The liberated iodine requires 31.46 mL of Na2S2O3 solution...
You form a solution by dissolving 15.39 grams of sodium chloride (molar mass = 58.44 g/mol)...
You form a solution by dissolving 15.39 grams of sodium chloride (molar mass = 58.44 g/mol) into 163.7 grams of water (molar mass = 18.02 g/mol). The total volume of the solution is 180.1 mL. Part #1: What is the molarity of sodium chloride in this solution? Part #2: What is the mass percent of sodium chloride in this solution? Part #3: What is the mole fraction of sodium chloride in this solution? Part #4: What is the molality of...
Calculate the concentration in osmolarity of a solution prepared by adding 5.00 g NaCl (molar mass...
Calculate the concentration in osmolarity of a solution prepared by adding 5.00 g NaCl (molar mass = 58.44) to a 100 mL volumetric flask, filling the flask to the mark with distilled water, and mixing.
a) What is the molarity of the solution that was prepared by dissolving 3.25 g of...
a) What is the molarity of the solution that was prepared by dissolving 3.25 g of sulfuric acid in water to a total volume of 500.0 mL? b)What is the molarity of the hydrogen ion in part a if you assume the sulfuric acid ionizes completely? Write a balanced chemical equation.
A 0.100-L solution is made by dissolving 0.441 g of CaCl2(s) in water. (a) Calculate the...
A 0.100-L solution is made by dissolving 0.441 g of CaCl2(s) in water. (a) Calculate the osmotic pressure of this solution at 27 °C, assuming that it is completely dissociated into its component ions. (b) The measured osmotic pressure of this solution is 2.56 atm at 27 °C. Explain why it is less than the value calculated in (a), and calculate the van’t Hoff factor, i, for the solute in this solution. (c) The enthalpy of solution for CaCl2 is...
ADVERTISEMENT
Subjects
ADVERTISEMENT
Latest Questions
ADVERTISEMENT