NTA fraction, given pH and HCO3 concentr

What is the fraction of NTA present after HT2- has been brought to equilibrium with solid PbCO3 at pH 7.00, in a medium in which [HCO3-] = 1.00E-3 M? Hint: Use the equilibrium constant expression to solve this problem. I used a couple of study guides but could not get the right answers..please help, thanx!

CH20 waste given mg/L, processed through sewage treatment, calculate volume for conversion

Assume that a waste contains 395.0 mg/L of biodegradable CH2O and is processed through a 190000.0 L/day sewage treatment plant which converts 40% of the waste to CO2 and H2O. Calculate the volume(L) of air (at 25 degrees, 1 atm) required for this conversion. Assume that the O2 is transferred to the water with 20% efficiency. Hint: Calculate mass of carbohydrate processed, use chemical equations to calculate mol oxygen needed to oxidize the carbohydrate, and the volume of air needed. I downloaded a couple of study guides but I kept getting the wrong answer. I don't know where I went wrong but I think the study guides may be wrong.

metric tons needed to yield H2SO4 required to produce specific rainfall amt?

How many metric tons of 5%-S coal would be needed to yield the H2SO4 required to produce a 4.0-cm rainfall of pH 2.00 over an area of 100 square kilometers? Hint: Calculate vol rain, mol H+, mass of S, mass of coal

photosynthesis

photosynthesis produces plant matter(need carbon "fixed" amt), total moles of glucose produced?, %solar energy converted to chemical energy? a) Photosynthesis is estimated to produce 330.0 g (dry weight) of plant matter per square meter, 50% of which is carbon. Calculate the total number of grams of carbon "fixed" each year by 1000 square meters. b) The photosynthetic reaction can be represented as: 6CO2 + 6H2O -> C6H12O6 + 6O2 Of the glucose produced, 20.0% is used by the plant to fuel respiration; the rest is converted to plant matter. Calculate the total moles of glucose produced annually in our reference 1000 square meter area. c) Each mole of glucose produced represents the a... click for more

rate of rxn given concentrations and rate constant

For the concentration of hydroxyl radical of 7.5E06 molecules/cm3 and a carbon monoxide concentration of 18 ppm, calculate the rate of its reaction with atmospheric carbon monoxide at 11 degrees C, given that the rate constant for the process is 5E-13 E-300/T molecule-1 cm3 sec-1. Hint: Convert the rate constant to a numerical value. Calculate the CO concentration to molecules/cm3, calculate the rate. I had an OTA help me but I am still getting the wrong ANSWER. I am supposed to multiply k*[CO][hydoxyl radical] and convert CO to molecules/cm3.