A 185.0 mL sample of 1.200 M Pb(NO₃)₂ is mixed with 119.50 mL of 1.500 M NaCl, and the PbCl₂ precipitate is filtered from the solution. Then 200.0 mL of 3.000 M NaBr is added to the remaining solution, and the PbBr₂ precipitate is also collected and dried. What is the mass (in grams) of the PbBr₂ precipitate, assuming the yield in each precipitation step is 100%?

4. In an experiment to determine the concentration of an HCI sample of unknown concentration, 0.1 M NaOH solution was prepared in the first step. Then, 50 mL of NaOH prepared as 0.1 M and 5 drops of methylorange indicator were added to a 250 mL flask and titrated with H2C204 prepared as 0.05 M. The turning point was observed when 26 mL of H2C204 was consumed in the titration process. In the second step, 50 mL of a non-concentrated HCI solution and 5 drops of phenolphthalein solution were added to a 250 mL flask and titrated with the adjusted NaOH solution. Calculate the concentration of an HCI sample with an unknown concentration, since it is determined that 16 mL of NaOH solution was consumed after titration.

A solution contains 1.47x102 M zinc nitrate and 1.37x102 M cobalt(II) acetate. Solid potassium carbonate is added slowly to this mixture. A. What is the formula of the substance that precipitates first? formula B. What is the concentration of carbonate ion when this precipitation first begins? [Co,?] = M

a.  An aqueous solution contains 0.20 M hydrocyanic acid.One Liter of this solution could be converted into a buffer by the addition of:(Assume that the volume remains constant as each substance is added.) 0.21 mol KCN 0.21 mol HI 0.20 mol KBr 0.050 mol Ba(OH)2 0.10 mol HI   b. An aqueous solution contains 0.18 M ammonium iodide. One liter of this solution could be converted into a buffer by the addition of:(Assume that the volume remains constant as each substance is added.) 0.18 mol HNO3 0.17 mol KI 0.08 mol HNO3 0.08 mol KOH 0.17 mol NH3 c.  An aqueous solution contains 0.33 M sodium fluoride.One liter of this solution could be converted into a buffer by the addition of:(Assume that the volume remains constant as each substance is added.) 0.16 mol KOH 0.33 mol HCl 0.32 mol NaCl 0.32 mol HF 0.16 mol HCl

I have 250.0 mL solution that is 0.100 CH3NH2. I add 50.0 of 0.250 M HNO3. What is the acid buffer capacity of the resulting solution? What is the base buffer capacity of the resulting solution?

Solution A is 5.35×10 ^-4M sodium iodide and Solution B is 5.35×10^-5  M in copper(I) acetate. If these two solutions combined, what compound would you expect to precipitate? When you combine and mix 35.0 mL of each solution in a large beaker, does the precipitate form?

A 0.4550-g solid mixture containing CaCl2 is dissolved in water and treated with an excess of Pb(NO3)2, resulting in the precipitation of 0.6168 g of PbCl2.          What percent of sample is CaCl2?

Solid sodium sulfide is slowly added to 125 mL of a 0.0536 M iron(II) acetate solution. The concentration of sulfide ion required to just initiate precipitation is  M.

10.00 mL of a solution of NaOH was titrated with with 0.09546 M KHP solution. At the equivalence point, 14.97 mL of KHP had been added. What was the concentration of the NaOH solution?

A 1.2516 gram sample of a mixture of CaCO3 and Na2SO4 was analyzed by dissolving the sample and completely precipitating the Ca2+ as CaC2O4. The CaC2O4 was dissolved in sulfuric acid and the resulting H2C2O4 was titrated with a standard KMnO4 solution. The titration required 35.62 mL of 0.1092 M KMnO4. Calculate the number of moles of H2C2O4 that reacted with the KMnO4. Calculate the number of moles of CaCO3 in the original sample. Calculate the percentage by weight of CaCO3 in the original sample.