Determine the enthalpy of neutralization in Joules/mmol for a solution resulting from 20 mL of 0.9 M NAOH solution and 20 mL of a HCI with the same molarity. If separately, each had a temperature of 28.6 degrees Celsius, and upon addition, the highest temperature reached by the solution was graphically determined to be 38.3 degrees Celsius. Round to the nearest whole number.

Determine the enthalpy of neutralization in Joules/mmol for a solution resulting from 20 mL of 0.9 M NAOH solution and 20 mL of a HCI with the same molarity. If separately, each had a temperature of 28.6 degrees Celsius, and upon addition, the highest temperature reached by the solution was graphically determined to be 38.3 degrees Celsius. Round to the nearest whole number.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Assuming 100% ionized in solution, what would be the calculated freezing point of 0.10 m solutions in wqter of a NaCl solution and BaCl2 solution. If the actual freezing points are -0.348 °C for NaCl and -0.470 °C for BaCl2 , explain the difference between these values and the calculated freezing points.
The freezing point of a liquid will change when a solute is added. Explain how the addition of salt impacts the boiling point of water. Calculate the freezing point change for a given concentration. Given that water’s freezing point is 0.00ºC and the freezing point depression constant (Kf) is 1.86 ºC･kg/mol, calculate the freezing point depression for a 4.35 molal solution (moles/kg) of NaCl in water. Assume ideal behavior of the ions.
calculate the boiking point of a solution in 0.20 grams of eugenol, dissolved in 12.0 grams of benzene (Kb benze = 2.53°C/m; Tb(solvent)= 80.10°C)
Using the Kf value for water from your book, you prepare a solution at 25.0 °C from 9.17 molof some solid and 7.31 L of water (d = 0.997 g/mL), but you forgot the identity of the solid. Youknow it was either glucose, sodium acetate, sodium phosphate, or sodium sulfate. You decideto determine the mass indirectly by measuring the freezing point depression of the solution,and find that the solution has a freezing point of −7.02 °C. Which substance is it and how doyou know this?
If dissolving 1.5 g of a solute into 100 mL of water caused the temperature of the solution toincrease by 4.7 ⁰C, what would the change of temperature be if 3.0 g of the solute were dissolvedin the same volume of water? Explain.
An experiment was conducted to determine the effect of glucose on the freezing point of water. Experimental data showed thatthe freezing point depression of water in solution was –2.6°C when 1.0 g of glucose was dissolved in 10g of solvent. Calculatethe expected freezing point for such solution and compare the expected freezing point to the value found experimentally. Give aplausible explanation for any discrepancies. (M.W. of glucose= 180.16g/mol; i=1). Show all your work.
Arrange the following solutions from lowest to highest freezing point (Tf) 0.65 m ethylene glycol (aq) 0.15 m CaCl2 (aq) 0.40 m MGSO4 (aq) (Ethylene glycol is non-electrolyte. The salts are strong electrolytes.) CaCl2 < Ethylene glycol < MGSO4 A. Ethylene glycol < CaCl2 < MgSO4 В. MGSO4 < Ethylene glycol < CaCl2 OC. CaCl2 < MgSO4 < Ethylene glycol D. Ethylene glycol < MGSO4 < CaCl2 Е.
The freezing point depression constant for benzene is 5.06 °C/m and the freezing point of pure benzene is 5.51°C. If a solution containing 3.241 g of a solid dissolved into 50.0 g of benzene has a freezing point of 4.68°C, what is the molar mass of the solid? Make sure units are correct and sig figs.
Use 2 decimal.
The dissociation of a salt in water to from an aqueous solution is called enthalpy of solution, AHoln- The AH3oln for CaCl, is -120 kJ/mol. When CaCl, is added to water 25. the temperature of the water will increase. the temperature of the water will remain the same. the process is endothermic. nothing will occur, CaCl, is insoluble.
Calculate the percent by mass of solute (%w/w) in solution when 2.14 g of potassium chloride is dissolved in 25.0 g of water.
8.71ml of a 4.00M HIO3(aq) solution is added to an ice-water mixture, and the freezing points were collected before and after addition of HIO3(aq). Once the temperature was stable after addition, the ice was separated from the solution and the mass of the beaker with solution was measured. The data below was recorded. Calculate the van't Hoff factor for HIO3. The freezing point depression constant for water is 1.86°C/m. Mass of beaker (g)l|Mass of beaker + solution (g T°f (°C)||Tf (°C) 87.438 176.179 0.305 ||-0.796