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Sodium bicarbonate is reacted with concentrated hydrochloric acid at 37.0°C and 1.00 atm. The reaction of 6.00 kg of bicarbonate with excess hydrochloric acid under these conditions will produce __________ L of CO2.
you wish to prepare a buffer solution containing nan3 and hn3 hydrazoic acid. you have to prepare the solutions first.
Assign an oxidation state to each element in each compound. Express all answers as a signed integer. 1. Na3PO4 2. Hg2S 3. Fe(CN)3 4. NH4Cl
In the lab using conc. HCL and heat, if the solubities of reactant and product were reversed , how would the isomerization be followed. How would one knows when it is complete
When the reaction that occurs finally ceases, what will be the mass of unreacted copper in the bar? What will be the mass of silver metal that "plates out" of solution (that is, what mass of silver metal is produced by the reaction)
Balance each of the following neutralization reactions. Express your answer as a chemical equation. Identify all of the phases in answer.
A 50.0-mL volume of 0.15 M HBr is titrated with 0.25 M KOH . Calculate the pH after the addition of 20.0 mL of KOH.
What will the pH of the equivalence point be when 10.00 mL of .0200M Carbonic acid is fully titrated to the 2nd end point using .05 M NaOH?
Say your a facility manager at a powerplant and your preparing for an interview with a news media reporter concerning environmental hazards at your facility
nathen and su-liu have new jobs at the fun house. they have been given the job of counting the balls in the kiddie
Using Gas Chromatography results and mass of your product mixture, calculate the percent yields of both 1-Hexanol and 2-Hexanol.
25 cubic centimetres of potassium hydroxide solution were neutralized by 24.0 cubic cenimtre of 1M per decimetre hydrochloric acid. what is the concentration in molar per decimetre of alkali?
The endpoint corresponds to the equivalence point. D. At the equivalence point the amount of reagent added does not yet equal to the amount of analyte present
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