A25.0 ml aliquot of 0.05300.0530 m edtaedta was added to a 38.038.0 ml solution containing an unknown concentration of v3 v3 . all of the v3 v3 present in the solution formed a complex with edtaedta , leaving an excess of edtaedta in solution. this solution was back-titrated with a 0.03100.0310 m ga3 ga3 solution until all of the edtaedta reacted, requiring 11.011.0 ml of the ga3 ga3 solution. what was the original concentration of the v3 v3 solution?

Since the gas in your graduated cylinder is a mixture of butane and water vapor, you must determine the partial pressure of the butane, pbutane, alone. to do this, consult a reference and record the partial pressure of the water vapor, pwater, at the temperature you recorded. use the following formula to compute the partial pressure of the butane. pbutane = atmosphere - pwater use the following combined gas law formula and compute the volume that the butane sample will occupy at stp. (hint: convert both temperatures to kelvin.) pbutane x voriginal = pstandard x vfinal troom tstandard use the following ratio and proportion formula to determine the mass of butane needed to occupy a volume of 22.4 l at stp. grams of butane you used “x” grams of butane ml of butane corrected to stp = 22,400 ml compute the theoretical molar mass of butane based on its formula and the atomic masses on the periodic table. compare your experimental results from #3 to the theoretical value of #4, computing a percent error of your findings using this formula: % error = measured value - accepted value x 100 accepted value use the following ratio and proportion formula to determine the mass of butane needed to occupy a volume of 22.4 l at stp. need asap

In a reaction equation, where are the products located? a.) above the arrow b.) to the right of the arrow c.) to the left of the arrow d.) below the arrow

Iwould appreciate if someone could me.