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Weak diprotic acid H2A is titrated with 0.2000 M NaOH. The initial concentration of H2A is 0.1000 M and the initial volume is 50.00 mL. Ka1 = 1.0 x 10?5 Ka2 = 1.0 x 10?9 a) Identify the predominate species at the first equivalence point, by chemical formula: b) Calculate the pH of the solution before any base is added. c) Calculate the pH at the first equivalence point. d) How many mL base, total, must be added to achieve the 2nd equivalence point? e) Calculate the pH at the second equivalence point. f) ) From the attached table of acid/base indicator transition ranges (bottom half of p.7), identify an appropriate indicator for: i) the 1st equivalence point ii) the 2nd equivalence point:
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calculating the pH of the final solution at equivalance point. Please show a step-by-step process
By definition, which of the following can be broken down into simpler substances?
A company produces vinegar products and discharges between 50,000 and 200,000 gallons per day (131 to 525 L / min) of a liquid waste stream that contains only acetic acid at a concentration of 80 mg/L.
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pH = log[H3O+] , pH + pOH = 14, [H3O+] * [OH-] = 1.0 X 10^-14, pH = -log(0.001) = 3 Could you show me a few of the steps between line one and two in both of these conclusions?
all possible structural formulas for all different conjugated dienes that can be completely hydrogenated
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Develop an argument based on bond enthalpies for the importance of SiO bonds in substances common in the Earth's crust in preference to SiSi or SiH bonds
When methanol, CH3OH, is dissolved in water, a nonconducting solution results. When acetic acid, CH3COOH, dissolves in water, the solution is weakly conductiong and acidic in nature. Describe what happens upon solution dissolution in the two cases..
Titration of sodium carbonate with HCl to the methyl orange end point involves the reaction of 1 mole of Na2CO3 with 2 moles of HCl. Write the balanced chemical equation in a.
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