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Write a balanced chemical equation showing the formation of the salt, Na3PO4, from the reaction of the appropriate strong acid and strong base, and name each compound in the equation.
The esterification reaction of acetic acid with ethanol to give ethyl acetate proceeds with the following stoichiometry: CH3COOH + C2H5OH ----> H20 + CH3COOC2H5.
Assume that a particular reaction evolves 243 kJ of heat and that 28 kJ of PV work is gained by the system....? 1) What are the values of delta E and delta H for the system? 2) What are the values of delta E and delta H for the surroundings?
What would be the best indicator for the titration of 0.20 M CH3COOH titrated with 0.2 M NaOH? (Ka for acetic acid = 1.8 X 10-5) The pH ranges for the color change of some common acid base indicators are given below
How many grams of NaCl is needed to prepare 100.0ml of 1.50 molar solution of NaCl in a volumetric flask.
Indicate what precipitates, if any, form when solutions of each of the following are added to a solution containing the Group I cations.
Why we add buffer 7 and 1:4 toluene and 2-propanol to crude oil ahead of titrate with Cdcl2 to dtermine H2S in crude oil.And can toluene and 2- propanol be replaced with other solvent in terms of cost and safety.
Imagine you want to determine the binding constant for a reaction. You know you will need to generate data to calculate the binding constant.
Draw out partial pathways to show which carbon(s) of glucose are lost in the first two cycles of the TCA cycle after entry as acetyl CoA fragments.
Determine the pressure change when a constant volume of gass at 1.00 atm is heated from 20.0 C to 30.0C.
Calculate the theoretical amount of 2.5 M NaOH (10%) solution needed to convert the benzoic acid to its water-soluble salt. Is the combined volume of NaOH used in the extractions sufficient for complete deprotonation of benzoic acid
The wavelength of light emitted if the electron drops from n=5 to n=4 will be shorter than the wavelength of light emitted when the electron falls from n=5 to n=3.
If .050 moles of HA were dissolved in 1L of water, calculate the concentration of [HA], [H30+], and [A-] in the solution at equilibrium. What is the pH? Ka=7.94 x 10^-7, equivalence point ~ 9 mL, pH at equivalence ~ 9]
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