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A) What is the pH (to nearest 0.01 pH unit) of a solution prepared by mixing 67.0 mL of 0.0755 M HBrO and 89.0 mL of 0.130 M NaOH?
B) What is the pH (to nearest 0.01 pH unit) of a solution prepared by mixing 52.0 mL of 0.125 M HF and 78.0 mL of 0.0465 M NaOH?
For the following reaction, 5.02 grams of nitrogen gas are mixed with excess hydrogen gas. The reaction yields 4.74 grams of ammonia. nitrogen (g) + hydrogen (g) --> ammonia (g)
a sample of 1.0 mole of a perfect gas with cp= 20.8 JK -1 is initially at 3.25 atm and 310 k. It undergoes reversible adiabatic expansion until its pressure reaches 2.50 atm. calculate the final volume and temperature and the work done
When maleic acid is heated to about 100C it forms maleic anhydride, however fumaric acid requires a much higher temperature (250-300C) before it dehydrates
Write an equation of the dissolution reaction for each of the precipitates that was soluble in CH3COOH. Al2(SO4)3+NaOH
rank the following compounds in order of decreasing vapor pressure. rank from highest to lowest vapor pressure. to rank
The boiling point of pure ethanol is 78 degres celsius .At the first sign of condensing vapors(when maybe just one drop of distillate has been collected) do you think you have pure ethanol?why or why not
what volume in milliliters of a 0.141 solution is required to reach the endpoint in the complete titration of a 16.0
this solution was added 1.960 grams of KI and 50.00 mL of a 0.00923 M KIO3 solution. The excess I3- was titrated with 50.00 mL of a 0.02000 M Na2S2O3 solution. What was the mass percent of arsenic trichloride in the original sample?
write the balanced net ionic equation for the reaction that occurs when 0.1 m solutions of copperii sulfate and calcium
Suppose that 25g of each of the following substances is initially at 27.0 degrees C. What is the final temperature of each substance upon absorbing 2.30kJ of heat
Isobutane is the fuel used in disposable lighters. The lighters' operation is dependent upon the butane's ability to vaporize and be ignited, and this depends somewhat upon the large pressure difference between the inside of the lighter
How many moles of each of the following were in the original sample? What is the molecular formula?
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