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Assume you are given 39.5 ml of a 0.129 M Ca(OH)2 solution that you will titrate with a 0.253 M HNO3 solution. If you used methyl orange as an endpoint indicator in your titration, how much would you be in error in your endpoint determination? (Report your error in ml of HNO3). The pKa of methyl orange is 4.10
How much heat would be given off per mole of NaOH if 4.6g of NaOH dissolves to give off 755J of heat? b)How many grams of NaOH are needed to produce 88 kJ of heat
The enthalpy of combustion of acetylene C2H2 is C2H2(g) + 5/2O2(g) ->2CO2(g) + H2O(l) H°rxn= -1299 kJ Calculate the enthalpy of formation of acetylene, given the following enthalpies of formation H°f[CO2(g)] = -393.5 kJ/mol ,H°f[H2O(l)] = -285.8 k..
A certain pesticide is fatal to fish fingerlings at a level of 0.50 parts per million in water. A leaking metal can containing 5.00 kg of the pesticide was dumped into a stream with flow of 10.0 L/sec moving at 1 km/hr.
question if 61.5 l of oxygen at 18c and an absolute pressure of 2.45 atm are compressed to 48.8l and at the same time
A reaction that is second-order in one reactant has a rate constant of 2.2 × 10-2 L/(mol · s). If the initial concentration of the reactant is 0.360 mol/L, how long will it take for the concentration to become 0.180 mol/L?
How many mL of 1.183 M H2SO4 must be added to 18.22 mL of 0.531 M NaOH to just completely react all of the NaOH according to the equation
When 2.45 g of an unknown weak acid HA with a molar mass of 85.0g /mol is dissolved in 250.0g of water, the freezing point of the resulting solution is -0.256 C.
A 1.70-g sample of a large biomolecule was dissolved in 14.0 g of carbon tetrachloride. The boiling point of this solution was determined to be 77.85°C.
How Well Do You Protect Your Safety - Are You an Environmentalist?
Two students prepare two cyclohexane solutions having the same freezing point. Student 1 uses 26.6 g of cyclohexane solvent, and student 2 uses 24.1 g of cyclohexane solvent. Which student has the greater number of moles of solute Show calculation..
although aspirin solutions do not absorb visible light, we are still able to use visible light in an experiment to analyze the purity of aspirin. Why?
Compute the final temperature of solution when 12 g of oxalic acid (COOH)2(s), is dissolved in 113.0mL of water that is initially at 16 C. Explain the enthalpies of formation of oxalic acid in the solid as well as aqueous phases are -826.8 and -81..
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