Calculate the volume

Calculate the molarity of a solution prepared by dissolving: 0.17 mol sulfuric acid in 85 mL of solution.   7.5 x 10–3 mol of sodium nitrate in a total volume of 13.5 mL of solution.

A student determines the calcium content of a solution by first precipitating it as calcium hydroxide, and then decomposing the hydroxide to calcium oxide by heating. How many grams of calcium oxide should the student obtain if his solution contains 53.0 mL of 0.461 M calcium nitrate?

As shown in the following Figure, an aqueous solution of Nal is poured into an aqueous solution of Pb(NO3)2 which results in the formation of a yellow precipitate. Assuming stoichiometric amounts of Nal and Pb(NO3)2 are reacted, give the chemical formula of the yellow precipitate and the chemical formula of all molecules and/or ions that are present in the solution (You may use the solubility matrix to answer this question). (b)

A solution is prepared by mixing 703 mL of ethanol with 697 mL of water. The molarity of ethanol in the resulting solution is 8.96 M. The density of ethanol at this temperature is 0.7893 g/mL. Calculate the difference in volume between the total volume of water and ethanol that were mixed to prepare the solution and the actual volume of the solution.

12.8 mL of 0.0354 M potassium permanganate solution is used to titrate 0.188 g of an unknown sample containing iron (II).  Calculate the percent by mass of an iron (II) in the unknown sample.

To analyze the alcohol content of a certain wine, a chemist needs 1.02 L of an aqueous 0.328 M K 2Cr 2O 7 (potassium dichromate) solution.  How much solid K 2Cr 2O 7 must be weighed to make this solution?

1.45-g sample of oxalic acid, H2C2O4, is dissolved in distilled water to make 50.00 mL of aqueous solution. This solution is called “Solution A”. The 5.00 mL of Solution A is added to 20.00 mL of distilled water to make “Solution B”.H2C2O4(aq) reacts with MnO4–(aq) to produce CO2(g) and Mn2+(aq).When 19.41 mL of H2C2O4(aq) (Solution B) is mixed with 21.59 mL of 0.0400 M MnO4–(aq), the mass of CO2(g) obtained is 0.0990 g.(a) In this chemical reaction, which substance is the oxidizing agent? Why?(b) Calculate the percentage yield of CO2(g).(c) Determine the molarity of the excess reactant at the end of the chemical reaction.

In the laboratory, a student dilutes 25.3 mL of a 8.46 M hydrobromic acid solution to a total volume of 100.0 mL. What is the concentration of the diluted solution?

The town of Andover obtains drinking water from three sources that together produce up to 6.81 × 107 L per day. If effective flocculation requires 9.248 × 10-5 M iron (III) chloride, how many grams of calcium hydroxide are required for treating one day’s worth of water?