10.23 g of sodium thiosulfate pentahydrate (ΔHsoln=+47.40 kJ/mol; MM = 158.108 g/mol) is dissolved in water. The mass of the water solution is 102.5 g. If the initial temperature of the water was 22.8°C, what will be the final temperature of the solution?
10.23 g of sodium thiosulfate pentahydrate (ΔHsoln=+47.40 kJ/mol; MM = 158.108 g/mol) is dissolved in water....
What is the final temperature of the solution when 4.806 g of sodium hydroxide is dissolved in 100.0 mL of water at an initial temperature of 24.5 C?. The density of water is 0.9969 g/cm3, and the heat capacity is 4.184 J/C. The enthalpy of dissolution for sodium hydroxide is -44.2 kJ/mol.
15.48 g of nickel sulfate (MM 154.75 g/mol) was dissolved in 100.00 mL of water. The initial temperature was 20.00 oC, and the final temperature was 25.06 oC, The specific heat capacity of the reaction mixture was 4.18J/g oC. What is the temperature change T? A.20.00 oC B.25.06 oC C.22.53 oC D. 278.06K E. 5.06 oC
1) The heat of solution (delta H) For sodium hydroxide is -44.5 kJ/mol calculate the amount of energy involved when 5.0 g sodium hydroxide is dissolved in water 2) calculate the change in temperature expected when 5.0 g sodium hydroxide is dissolved in 50.0 g water using the energy (Joules) calculated above. (Ccal= 4.5J/g°C, include 4.0g magnetic stir-bar in the total mass) Prelab Exercise: The Heat of solution (H) for sodium hydroxide is -44.5 kJ/mol. Calculate the amount of energy...
The salt sodium perchlorate is soluble in water. When 9.07 g of NaClO4 is dissolved in 103.00 g of water, the temperature of the solution decreases from 25.00 to 22.70 °C. Based on this observation, calculate the enthalpy of dissolution of NaClO4 (in kJ/mol). Assume that the specific heat of the solution is 4.184 J/g °C and that the heat absorbed by the calorimeter is negligible. ΔHdissolution kJ/mol =
Given 15.0 g of NaCl (MM of NaCl = 58.44 g/mol) is dissolved in 100.0 g of water: a. Determine the mass percent of this solution. b. Assume the density of the solution is 1.00 g/ml, calculate the molarity of the solution.
Part A When a 1.78 g sample of solid sodium hydroxide was dissolved in a calorimeter in 60.0 g of water, the temperature rose from 4.2 °C to 40.8 °C . Calculate AH (in kJ/mol NaOH) for the following solution process: NaOH(s)- Na (aq) +OH (aq) Assume that it's a perfect calorimeter and that the specific heat of the solution is the same as that of pure water. ΑΣφ ? kJ/mol
A 7.41 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 15.00 g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72 degrees celsius. After the salt has completely dissolved, the temperature of the solution is 28.54 degrees celsius. A) Was the dissolution process endothermic or exothermic? B) What is the heat for the dissolution reaction?
Heat of Solution The heat of solution of potassium acetate (KC2H3O2) in water is -15.30 kJ/mol. If 16.80 g of KC2H3O2(S) is dissolved in 525.0 mL of water that is initially at 22.70 °C, what will be the final temperature in degrees Celcius) of the resulting aqueous solution? (Assume no heat exchange with the surroundings.)_______ ℃
A sample of sodium iodate with a mass of .311g is dissolved in water and made up to 250 ml. 25.0 ml potions are added to KI that has been dissolved in sulfuric acid. The resultant iodine is titrated against sodium thiosulfate, the average volume being 12.5 ml. Calculate the molarity of the thiosulfate solution
(c) (Challenging). 1.3608 g of sodium acetate trihydrate solid C2H3NaO2●3H2O (NaAc●3H2O, MM = 136.08 g/mol) was fully dissolved in 100.0 mL of pure water. What was the pH of this solution?