An iron ore was analyzed by dissolving a 1.957-g sample in concentrated HCl. The resulting solution was diluted with water, and the iron(III) was precipitated as the hydrous oxide Fe2O3·xH2O by the addition of NH3. After filtration and washing, the residue was ignited at a high temperature to give 0.6009 g of pure Fe2O3. Calculate (a) the % Fe and (b) the % Fe3O4 in the sample.

A 0.124 M NaOH(aq) solution was used to titrate 20.00 mL of an acetic acid (CH3COOH) solution that has an unknown concentration. The equivalence point is reached after adding 15.34 mL of NaOH(aq). a) Write out the complete balanced equation for the reaction that occurs in this titration. b) How man moles of NaOH were added to the acetic acid solution? c) How many moles of acetic acid were in the original 20.00 mL solution? d) What was the concentration of acetic acid in the orignial 20.00 mL solution?

A 0.2174 g sample of a pure carbonate, XnCO3(s), was dissolved in 50.0 mL of 0.1500 M HCl(aq). The excess HCl(aq) was back titrated with 23.90 mL of 0.0980 M NaOH(aq). How many moles of HCl react with the carbonate? moles of HCL = 5.16*10^(-3) What is the identity of the cation, X? cation = ?

When a solution of hydrochloric acid is added to silver nitrate dissolved in water, a white precipitate called silver chioride is produced along with nitric acid which is highly corrosive. This is best represented by which chemical equation? O HCI (aa) - AGNO3 (ax) -→ AgCi (1) - H3N (ag) O HCI (ag) • AGNO3 (a) --→ AgCi (1) - HON(aq) O HCI (an) - AgNO3 (aa) --→ AgCI (1) - HNO3 (aq) O HCI (aq) + AGNO3 (a9) --> AgCI (1) + HNO3

An iron ore sample weighing 0.9174 g is dissolved in HCl(aq), and the iron is obtained as Fe2+(aq). This solution is then titrated with 34.62 mL of 5.016×10−2 M K2Cr2O7(aq)6Fe2+ + 14H+ + Cr2O2−7  → 6Fe3+ + 2Cr3+ + 7H2O What is the mass percent Fe in the ore sample?

0.9545 g of calcium nitrate salt, Ca (NO3) 2, is weighed, dissolved in concentrated HCl solution and added to 500 ml with water. It is diluted, 100 ml sample taken here is precipitated as CaC2O4, burned in the ash furnace and It is converted to CaCO3 and then to CaO. Since it comes to 0.2500 g when weighed, the amount of Ca in the sample and calculate its% (Ca: 40 g / mol, O: 16 g / mol)

What concentration of Zn²+ is present in solution when 5.00 g of zinc metal is used to displace hydrogen from 150 mL of 0.500 M HCl(aq)?

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?

A 50.0 mL solution of Ca(OH)₂ with an unknown concentration was titrated with 0.340 M HNO₃. To reach the endpoint, a total of 16.8 mL of HNO₃ was required. Write the balanced chemical equation based on the following description: solid calcium hydroxide reacts with aqueous nitric acid to produce the aqueous calcium nitrate and liquid water.  Ca(OH)2(aq)+HNO3(aq)------

A permanganate solution is prepared by dissolving 20.0123 g KMNO4 in 500 mL of distilled water and boiled for 1 hour to remove any organic material. Following sintered-glass filtration, the solution is quantitatively transferred to a 1.0 L volumetric flask and diluted to volume with distilled water. The permanganate solution was titrated against 0.1023 M oxalic acid prepared in sulfuric acid solution. A 50.00 mL aliquot of oxalic acid solution required 16.68 mL of permanganate solution. A titration blank required 0.04 mL of permanganate. What is the permanganate molarity? 3. 5 H;C204 + 2 MnO¿ + 6H* s 10 CO2 + 2 Mn²* + 8 H2O