When 3.25 g of sodium hydroxide (NaOH) was dissolved in 100.00 g
of water a value of 10.50oC was obtained for ΔT.
Calculate the molarity of the sodium hydroxide solution.
Calculate the value (calories) for the heat of solution of 3.25 g of NaOH
Calculate the number of calories that would be produced if one
mole of sodium hydroxide was dissolved.
(ΔHsolnNaOH)
.
When 3.25 g of sodium hydroxide (NaOH) was dissolved in 100.00 g of water a value of 10.50oC was obtained for ΔT. Calcul...
When 3.25 g of sodium hydroxide (NaOH) was dissolved in 150.00 g of water a value of 9.50oC was obtained for ΔT. Calculate the value (calories) for the heat of solution of 3.25 g of NaOH. Calculate the number of calories that would be produced if one mole of sodium hydroxide was dissolved. (ΔHsolnNaOH)
A. ΔHsolution of NaOH(s) Phase Change: Mass of NaOH: 2.02 g ΔT for reaction A : 9 °C updated: 50mL of water was added 1. Calculate the number of moles of NaOH in the Solution: (I solved this: 0.0505 moles) 2. Calculate the value (calories) for the heat of solution. 3. Calculate the ΔHsolution for sodium hydroxide.
A. ΔHsolution of NaOH(s) Phase Change: Mass of NaOH: 2.1 g ΔT for reaction A : 10 °C number of moles of NaOH in the Solution : 0.0525 moles Calculate the value (calories) for the heat of solution. Calculate the ΔHsolution for sodium hydroxide.
1, 3.50 g of sodium hydroxide (NaOH) are dissolved in water and the solution made up to 150.0 mL. What is the molarity, M, of the solution
When a 3.11 g sample of solid sodium hydroxide was dissolved in a calorimeter in 130.0 g of water, the temperature rose from 18.9 oC to 31.3 o C . Calculate Δ H (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.
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
25. When 5.35 g of slid sodium hydroxide was dissolved in a calorimeter containing 100 g of water, the temperature rose from 20.5 C to 28.6"C. calculate the ? H ( in KJ/mol NaOH) for the following solution process: NaOH (s)Na (aq) OH (aq) Assume that it is a perfect calorimeter and that the specific heat of the lution is the same as that of pure water (4.184 J/g °C).
C. ΔH for Reaction of HCl(aq) and NaOH(s): Volume of HCl: .05 L Volume of water: .05 L Volume total: .1 L Molarity of HCl: 2.08 M Mass of NaOH: 3.93 g ΔT for reaction C: 19°C 1. Calculate the number of moles of NaOH 2. Using NaOH as the limiting reagent, calculate the molarity of the resulting sodium chloride solution. 3. Calculate the value (calories) for the heat of reaction. 4. Calculate the ΔH for this reaction. 5. Is...
C. ΔH for Reaction of HCl(aq) and NaOH(s): Volume of HCl: 0.055 L Volume of water: 0.045 L Volume total: 0.1 L Molarity of HCl: 2.08 M Mass of NaOH: 4 g ΔT for reaction C: 23°C number of moles of NaOH : 0.100 moles molarity of the resulting sodium chloride solution : 1.00 M ΔT : 23.0 °C Calculate the value (calories) for the heat of reaction. Calculate the ΔH for this reaction.
0.45 g of sodium hydroxide (NaOH) pellets are dissolved in water to make 8.0 L of solution. What is the pH of this solution? Express the pH numerically to two decimal places.