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The ionization constant or dissolution constant (KA) for acetic acid (HAc) is 1.8×10-5. (1) Write down the dissociation reaction. (2) Estimate pH of a solution containing 0.6 g of acetic acid in 1 L of water. Molecular weight of acetic acid is 60 g/mol.
Calculate the final temperature of the water and ice together once they have reached thermal equilibrium. The specific heat capacity of water is 4.184 J/g°C. Assume no heat is lost to the surroundings during the process
What is the pH at the equivalence point? the Ka of hydrofluoric acid is 3.5x10^-4.
In coffee, how much would the boiling point (in C) of the water be raised by the addition of 0.2 g of caffeine (C8H10N4O2) to 5.0 L of water in making this so much coffee
Determine what volume of .1 M HBr is required to neutralize 50 ml of .140 M Barium hydroxide and determine the normality of a solution consisting of 10.51 mg of NaOH in 591 mL of solution
At 25 oC the solubility of copper(II) iodate is 3.27 x 10-3 mol/L. Calculate the value of Ksp
Cesium has the smallest ionization energy of all the elements (376 kJ/mol), and chlorine has the most negative electron affinity (-349 kJ/mol).
Ferrophosphorus reacts with pryite producing iron(II) sulfide and a compound that is 27.82% P and 72.13% S by mass and has a molar mass of 444.56 g/mol. a) determine the empirical and molecular formulas of this compound. b) Write a balanced chemic..
What is the half life of a first order reaction if it takes 4.4 x 10-2 seconds for the concentration to decrease from an initial concentration
Draw the tetrahedral representation of the S enantiomer of the amino acid alanine, CH3CH(NH2)CO2H.
If 250 ml of H2SO4 of unknown concentration with a methyl orange indicator present is titrated with [0.345 M] NaOH, the red solution turns yellow after 20.4 ml of the NaOH is added. What is the molarity of the H2SO4 solution
If 84 g of CO reacts to produce 63 g of CH3OH, What is the percent yield of CH3OH?Answer in units of % ?
If an air bubble was initially in the buret tip but was dispensed during the back titration of the unreacted HCl. As a result of this technique error
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