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A solution is prepared by adding sodium hypochlorite to enough water to make 800 mL of solution. The pH of this solution was determinded to be 10.50. Given that the Ka for hypochlorous acid is 3.0x10^-8 determine the number of moles of sodium hypochlorite needed to prepare this solution.
Explain the difference in the answers to question 2 and question 5. Which is the "correct" value for the concentration of the standard NaOH solution? Why?
The heat of solution of ammonium nitrate is 26.2 kJ/mol. If a 5.368 g sample of NH4NO3 is added to 40.0 mL of water in a calorimeter at 23.5°C, what is the minimum temperature reached by the solution.
Consider the following reaction: 2H2O + 2SO2 2H2 + 3O2 A reaction mixture initially contains 2.8M H2O and 2.6 M SO2.
HFC's (hydrofluorocarbons) are replacing CFC's (chlorofluorocarbons) because the C-H and C-F bonds are stronger than C-Cl bonds. If the bond enthalpy of a C-F bond is 482 kJ/mol.
Draw the Fischer projection of the enantiomer of (4S, 5S)-5-sec-butyl-4-(1,1-difluoromethyl)nonane
The reaction of calcium hydride with water can be used to prepare small quantities of hydrogen gas, as is done to fill weather observation balloons.
In a hydrogen atom, from what energy level must an electron fall to the n = 3 level to give a line at 1.28 micrometers in the infrared region? a. 7 b. 5 c. 6 d. 4 e
You have a 4 L bottle of sulfuric acid solution. You take 50.0 mL of this H2SO4(aq) solution and titrate it to the endpoint with a 0.10 M NaOH solution. If the volume of NaOH solution needed is 60.0 mL, the concentration of the sulfuric acid (H2SO..
The reaction of fluorine of 7.6 grams with excess chlorine(Cl) produced 3.3 grams of ClF3. Determine the percent yield of ClF 3 was obtained??
Hardness in groundwater is due to the presence of metal ions, primarily Mg2 and Ca2 . Hardness is generally reported as ppm CaCO3 or mmol/L Ca2
1. Gasoline (assumed to be 100% octane) is combusted in your car according to the following chemical reaction: 2 C8H18 + 25 O2 -> 16 CO2 + 18 H2O
Sorbic acid, C5H7COOH, is a weak monoprotic acid with Ka = 1.7 x 10-5. Calculate the pH of a solution containing 11.25 g of potassium sorbate in 1.75 L of solution.
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