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What is the pH of a buffer that results when 0.50 mole of Na3PO4 is mixed with 0.75 mole of HCl and diluted with water to 1.00 L? (The acid dissociation constants for phosphoric acid are Ka1 = 7.5 * 10^-3, Ka2 = 6.2 *10^-8, and Ka3 = 3.6 * 10^-13)
4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g) In a certain experiment, 4.30 g of NH3 reacts with 7.48 g of O2. Which is the limiting reactant?
Separation of Amines and Carboxylic Acids Using Extraction, Initially have a sample of a water-insoluble, neutral organic compound dissolved in 50 mL methylene chloride that may be contaminated with
A 1.00 L balloon filled with nitrogen at 25 ° C and 765.3 torr is moved to a closed vessel with the pressure now at 659.3 torr and temperature 25 ° C.
In the first 12.0 of the reaction, 1.8×10-2 of is produced in a reaction vessel with a volume of 0.260 . What is the average rate of the reaction over this time interval.
A close chemical relative of the banned insecticide DDT is methoxychlor (C16H15Cl3O2). Methoxychlor is currently used as a home insecticide. Calculate the mass percent of oxygen in methoxychlor.
If 6.06 L of O2 gas is collected over water at 250C (vapor pressure = 23.8 torr) and a barometric pressure of 702 torr, what is the mass of H2O2 (MM = 34.02 g/mole) decomposed?
Consider the titration of 50.0 mL of 0.217 M hydrazoic acid (HN3, ka=2.6x10^-5) with 0.183 M NaOH. Calculate the pH of the solution after the addition of 29.7 mL of NaOH solution
Calculate the number of grams of H2 formed If the wet Hydrogen gas formed occupies a volume of 9.67 Litres
What mass of sodium chloride, NaCl, is needed to make 389. g of a 3.89%(m/m) NaCl solution? (atomic masses: Na = 22.99, Cl = 35.45)
Consider the following reactions and select the false statement below. CO2(g) + OH?(aq) ? HCO3?(aq) Cr3+(aq) + 6H2O(l) ? Cr(H2O)63+(aq) A. a lone pair of electrons on the OH?
Calculate the enthalpy of the reaction: 2NO(g) + O2(g) --> 2NO2(g) given the following reactions and enthalpies of formation: 1/2 N2(g) + O2(g) --> NO2(g), delta H *A = 33.2 kJ 1/2 N2(g) + 1/2O2(g) --> NO(g), delta H *B= 90.2 kJ
2 FeS + 3 N2 → 2 FeN + 2 SN2 This reaction has a 65.0% yield. How much N2 is consumed if 13.6 g of FeN are produced?
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