A stock solution containing Mn2+ ions was prepaned by dissolving 1.584 g pure manganese metal in nitric acid and diluting to a final volume of 1.000 L. The following solutions were then prepared by dilution: For solution A, 50.00 mL of stock solution was diluted to 1000.0 mL. For solution B, 10.00 mL of solution A was diluted to 250.0 mL. For solution C, I 0.00 mL of solution Bwas diluted to 500.0 mL. Calculate the concentrations of the stock solution and solutions A,B, and C.

The antacid found in Tums™ has the active ingredient calcium carbonate, which undergoes a reaction when mixed with hydrochloric acid to produce water, calcium chloride and carbon dioxide. A tablet of this antacid had a mass of 1.774g and was dissolved completely in an excess of 30.0mL of 0.794M HCl. The resulting solution was then titrated with 0.995M NaOH. The initial buret reading was 11.05mL and the final buret reading was 28.52mL. The listed mass of active ingredient on the bottle is 325mg. a. What is the calculated mass of active ingredient in this tablet? b. What is the percent error from the listed mass? c. What percent of the tablet is inert (non-active) ingredients? explain in detail

A 25.00 mL aliquot is withdrawn from the liquid portion of saturated Manganese (II) hydroxide and transferred to an Erlenmeyer flask.  After the addition of methyl orange, a titration with 0.0045 M HCl was performed.  The endpoint was reached after 8.72 mL of the acid was added.   What is the balanced chemical equation? How many moles of hydroxide ions were neutralized in the reaction?  What is the molar concentration of hydroxide in the saturated solution?  What is the molar concentration of Magnesium ion in solution?

A 100.0 ml solution of NaCl was mixed with a 100.0 ml solution of 0.1 M Pb(NO3)2. If 1.24 g of PbCl2 was obtained, what was the Molarity of NaCl in the initial 100.0ml?               What was the final concentration of Pb2+?

The zinc content of a 1.55 g ore sample was determined by dissolving the ore in HCl, which reacts with the zinc. The excess HCl is then neutralized with with NaOH. The reaction of HClHCl with Zn is shown.   Zn(s)+2HCl(aq)⟶ZnCl2⁢(aq)+H2⁡(g)   The ore was dissolved in 150 mL of 0.600 M HCl  and the resulting solution was diluted to a total volume of 300 mL. A 20.0 mL aliquot of the final solution required 8.92 mL of 0.548 NaOH to neutralize the excess HCl. What is the mass percentage (%w/w) of Zn in the ore sample?

The zinc content of a 1.07 g ore sample was determined by dissolving the ore in HCl, which reacts with the zinc. The excess HC1 is then neutralized with with NaOH. The reaction of HC1 with Zn is shown. Zn(s) + 2 HCl(aq) → ZnCl₂ (aq) + H₂(g) The ore was dissolved in 150 mL of 0.600 M HCl, and the resulting solution was diluted to a total volume of 300 mL. A 20.0 mL aliquot of the final solution required 9.96 mL of 0.540 M NaOH to neutralize the excess HC1. What is the mass percentage (%w/w) of Zn in the ore sample? %W/W = % Zn

A 185 mL sample of 1.20 M Pb(NO₃)₂ is mixed with 99.5 mL of 1.50 M NaCl, and the PbCl₂ precipitate is filtered from the solution. Then 200 mL of 3.00 M NaBr is added to the remaining solution, and the PbBr₂ precipitate is also collected and dried. What is the mass of the PbBr₂ precipitate, assuming the yield in each precipitation step is 100%?