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1. You titrate 125 mL of a solution of ammonia (NH3) with 1.0 M HClO4. The equivalence point is reached after adding 25 mL of the titrant.
a.) What kind of titration was this (WA/SB; WB/SA; SA/SB; polyprotic A (or B) /SB (or SA); WA/WB)?
b.) Write a balanced reaction for the titration.
c.) What is the concentration of the NH3?
d.) Would the resulting solution be acidic, basic, or neutral?
4. Write the Keq expression for the following equilibria:
a.) H3PO4 (aq) + H2O (l) ? H3O + (aq) + H2PO4 - (aq)
b.) HCO3 - (aq) + H+ (aq) ? H2O (l) + H2CO3 (aq)
c.) PbSO4 (s) ? Pb+2 (aq) + SO4 -2 (aq)
Three 10.00mL samples of the ascorbic acid solution necessary an average of 25.7mL of titrant for the complete reaction. Compute the mean molarities of the DCP solution
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Liquid nitrogen trichloride is heated in a 2.50-L closed reaction vessel until it decomposes completely to gaseous elements. The resulting mixture exerts a pressure of 754 mmHg at 95 0C. What is the mass of the original sample.
molar absorbtivity data for the cobalt and nickel complexes with 23-quinoxalinedithiol are epsilonco 36400 and
Problem- A 100.0-mL sample of 0.2 M (CH3)3N (Kb = 5.33 x 10^-5) is titrated with 0.2 M HCl. What is the pH at the equivalence point
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At high temperatures phosgene (COCl2) decomposes to give carbon monoxide CO and Cl2. In a typical experiment, 0.631 g of COCl2 is injected into a flask of volume 472 cc. When equilibrium is established, it is found that the total pressure is 2.175..
If 5.20 g of HCL is added to enough distilled water to form 3.00 L of solution, explain what is the molarity of the solution. Use molecular weight: HCL, 36.46 amu
A particular reactant decomposes with a half-life of 127 s when its initial concentration is .364M. The same reactant decomposes with a half-life 245 s when its initial concentration is .189 M.
A chemist dissolves 0.151g of pure perchloric acid in enough water to make up 0.370L of solution. Calculate the pH of the solution. Be sure your answer has the correct number of significant digits.
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