A 0.5187-gram sample of calcium chloride (CaCl2;MW 110.98g/mol) was dissolved in 300. mL of water. What is the molality of the solution? (Assume the density of water is 1.00g/ml)
A 0.5187-gram sample of calcium chloride (CaCl2;MW 110.98g/mol) was dissolved in 300. mL of water. What...
When 23.6 g of calcium chloride, CaCl2, was dissolved in water in a constant-pressure calorimeter, the temperature rose from 25.0 C to 38.7 C. If the heat capacity of the solution and the calorimeter is 1258 J/C, what is the enthalpy change when 0.710 mol of calcium chloride dissolves in water? The solution process is CaCl2(s) --> Ca2+(aq) + 2Cl–(aq)
specific heat capacity 2. If 3.8 g of calcium chloride (CaCl2) is dissolved in 100.0 mL of water, the following data are collected: starting temperature is 25.8 °C, final temperature after dissolving is 29.9 °C. Calculate the enthalpy of solution in Joules. You may assume a density of 1.00 g/mL for the solution and you may assume that the specific heat is that of water (this is a dilute solution) and is 4.18 J/(gx°C). Is this an endothermic or exothermic...
Consider the dissolution of Calcium Chloride: CaCl2(s)---->Ca^+2(aq) + 2Cl−(aq) ΔHrxn= -81.5kJ An 12.0 g sample of calcium chloride is dissolved in 100.0 g of water, with both substance at 22.0 degree C. Molar Mass: CaCl2= 110.98g.mol Molar Mass H20= 18.02g/mol Density of H20= 1.00g/mol Cs(soln)= 4.20 J/(g K) Will the temperature of the solution go up or down? Explain. Calculate q(reaction)
Part 4. Molality of the calcium chloride solution Molality is defined as mol solute Calculate the molality of your assigned calcium chloride solution. Assume that the density of kg solvent water is 1g/mL. Questions (SHOW ALL WORK) 1. Calculate the molarity (M) of a solution when 12.80 g of glycerol (CHsOs) is added to 40.70 g of water. The density of the solution is 1,052g/ml Colligative properties like boiling point elevation depend on the number of solute particles in solution....
A 0.5 gram sample of calcium chloride dihydrate (CaCl2 • 2H2O) is heated driving off the water. The dehydrated calcium chloride (CaCl2) weighs 0.38 grams. What was the % H2O by mass? Hint: Just use grams, there is absolutely no need for moles this time. It is not a trick question.
A 5.0067 g sample of Na2CrO4 (MW = 161.97 g/mol) is dissolved in 250.0 mL of water. Assume the solution has a density of 1.00 g/mL. A 50.0 mL aliquot of the solution is then diluted to a final volume of 250.0 mL. What is the concentration of Na+ in the diluted solution in units of parts per million (ppm)?
A 5.9957 g sample of Na, CrO, (MW = 161.97 g/mol) is dissolved in 1000.0 mL of water. Assume the solution has a density of 1.00 g/mL What is the concentration of Na* (MW = 22.9898 g/mol) in the solution in units of molarity (M)? concentration: М What is the concentration of Na+ in the solution in units of parts per thousand (ppt)? concentration: ppt A 50.0 mL aliquot of the solution is then diluted to a final volume of...
A 5.6780 gram sample of the compound Na2XO3 was dissolved in water then reacted with excess calcium chloride: Na2XO3(aq) + CaCl2(aq) →CaXO3(s) + 2NaCl(aq) A total of 5.4842 grams of CaXO3 were collected. What is the identity of the element “X?”
A 30% solution of calcium chloride (CaCl2 - MW = 110.98 g/mol) has been prepared by a technician for direct intravenous injection to a patient. While reviewing the order and preparation, you recall that this concentration seems to be abnormal. As a result, you want to determine the osmolarity of the solution. What is the osmolarity of this solution? Note: Please provide your answer in units of mOsmol/L.
5.3307 g of Na2CrO4 (MW 161.97 g/mol) is dissolved in 1000.0 mL of water. Assuming the solution has a density of 1.00 g/mL, what is the concentration of Na (MW 22.9898 g/mol) in the solution in units of a) molarity (M)? Number b) parts per thousand (ppt)? Number ppt c) 25.0 mL of the solution is then diluted to a final volume of 500.0 mL. What is the concentration of Na* in the diluted solution in units of parts per...