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A 30.00mL sample of 0.1234M hypobromous acid (HBrO) is titrated with a 0.2555M potassium hydroxide solution. (Ka for hypobromous acid = 2.5x10^-9) How many milliliters of potassium hydroxide solution would be required to reach the midpoint of the titration?
The only materials on hand are 300 mL of white vinegar (5.00% by mass acetic acid, density = 1.006g/mL) and potassium acetate. How should the student proceed?
converted completely to FeNCS 2+ when the calibration curve was prepared, would this raise or lower the value of Keq? explain?
Is the reaction exothermic or endothermic. Does the reaction lead to an increase or decrease in the disorder of the system
If we inject 120.0 mL of liquid helium and allow the entire system to warm to room temperature (25°C), what is the pressure inside the bottle
Tabulate the viscosity and density of water between the temperatures of 10 degrees and 80 degrees, in one degree increments in the 20 to 35 degrees interval and in 5 degrees increments outside this interval
What is the molarity of ZnCl2 that forms when 30.0 of zinc completely reacts with CuCl2 according to the following reaction? Assume a final volume of 285 mL . Zn+ CuCl2=ZnCl2+Cu.
The material was used for thermal insulation in the 2003 Mars Exploration Rover. If the maximum space for insulation in the spacecraft's hull was 2294 cm3, what mass (in grams) did the aerogel insulation add to the spacecraft?
What is the theoretical yield of ammonia in grams that can be prepared from 41.0 g of nitrogen and excess hydrogen
An evaluation of R was performed, following the procedure described in this module. The barometric pressure was 736 torr, the temperature was 295k and volume of hydrogen gas collected was 35.6 mL. The calculated value of R was 82.1 mL atm K^-1 mol..
what is the freezing point of solution made up of 54.9 g of NaCl dissolved in 800 g of water
Calculate the percent (by volume) of air that would be displaced when all of theN2 (l) get evaporated. it is given that Liquid nitrogen has a density of 0.807 g/mL
The iron (55.847 g/mol) in a 700.0 mL sample of a natural water was determined by precipitation of the cation as hydrated Fe2O3. The precipitate was filtered
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