excess silver nitrate is added to 100.0 mL of a solution containing barium ions to produce 1.84 g of AgCl precipitate molar mass equals 143.32 g•mol^-1. What is the molar concentration of the silver iron in the original solution? 

14.00 mL of deionized water is added to 35.00 mL 0.250 M hydrochloric acid. Calculate the molarity of the resulting solution.

A 2.37 g sample of a mixture of FeCl2 and Fe(NO3)2 is treated with excess AgNO3(aq). The precipitate is filtered off, dried and weighed. The dried precipitate weighs 4.05 g. What is the percentage by mass of FeCl2 in the original mixture? Your answer must be accurate to two sig figs.

A solution of NaCl(aq) is added slowly to a solution of lead nitrate, Pb(NO3)2(aq), until no further precipitation occurs. The precipitate is collected by filtration, dried, and weighed. A total of 17.07 g PbCl2(s) is obtained from 200.0 mL of the original solution. Calculate the molarity of the Pb(NO3)2(aq) solution.

A student investigated the stoichiometry of the reaction of zinc (Zn) with HCI solution and reported the following data: When 0.2158 g of Zn reacted with 10.00 mL of 1.000M HCI, 82.062 g of water was displaced. A total of 36.00 mL of 9.501 x 10 M NaOH solution was required to titrate the HCl remaining in the reaction mixture at the end of the reaction. The room temperature was 27.0°C and the barometric pressure was 777 torr. The gram atomic mass of Zn is 65.38 g mol. The density of water at 27.0 °C is 0.9965 g mLand its vapor pressure is 27.0 torr. R = 8.21 X.10 2 L- atm K mol 1 Calculate the number of millimoles of HCI remaining in the flask at the end of the reaction

Normally, the amount of silver nitrate required to precipitate all of the chloride in the sample is found by a trial and error process. However, to speed up the experiment, assume a sample mass of 0.1431 g, and that sample contains approximately 55.0% chloride ion by mass. From these assumptions, calculate the volume of 0.100 M AgNO3(aq) that needs to be added to precipitate all of the chloride ion. Please answer in mL. (Note: You are calculating the exact amount required and not adding 5mL in excess. In the experiment, you'd be adding an additional 5mL in excess since the chloride value of the salt may exceed 55%. Pay attention to the sig. figs. in your calculation; keep three sig. figs. in the answer.)

Calculate the volume (mL) of 1.0 M metal nitrate solution required to prepare 5.0 g of the COBALT pigment. Again, using the balanced chemical equation you should be able to relate the moles of pigment to the moles of metal nitrate and from that calculate the volume of 1.0 M metal nitrate solution required. Please report your value as XX.X mL (one decimal point and no units).