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Just number 3 pls. I need complete solutions for review. thank you
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- A chemist dissolves a 1.497-g sample of a type of metal (an alloy of Sn, Pb, Sb, and Cu) in nitric acid, and metastannic acid, H2SnO3, is precipitated. She heats the precipitate to drive off the water, which leaves 0.4909 g of tin(IV) oxide. What was the percentage of [in in the original sample?A. Upon addition of concentrated HNO3 to copper metal B. Addition of water to resulting solution in A The chemical equation of A is Cu(s) + 4HNO3 (aq) -> Cu(NO3)2 (aq) +2NO2 (g) + 2H2O (l). What will be the chemical equation for B.?What type of reaction is this? 2 AGNO3 + Cu --> Cu(NO3)2 + 2 Ag What type of reaction is this? Pb + FeSO, --> PBSO, +Fe What type of reaction is this? MgCl2 + LizCO3 --> M8CO3 + 2 LICI
- +1.14 V TI Pt Cr3+ (1 M) Cr2+ (1 M) T13+ (1 M) T13+ (aq) + 3e- TI (s) Cr2+ (aq) → Cr3+ (aq) + e- The species being oxidized is and the species being reduced is respectively. Note: "TI" is the symbol for thallium (element #81). O Pt / TI O TI3 / Cr2+ O C/TP O C+/ TI • TI/ Cr+ DELL Esc F1 F2 F3 F4 F5 F6 F7 F8 F9 %231. A sample containing magnetite, Fe;O4, was analyzed by dissolving a 1.5419-g sample in concentrated HCI, giving a mixture of Fe2+ and Fe³+. After adding HNO3 to oxidize any Fe2+ to Fet, the resulting solution was diluted with water and the Fe+ precipitated as Fe(OH)3 by adding NH3. After filtering and rinsing, the residue was ignited, resulting to 0.8525 g of pure Fe2O3. Calculate the: a) % (w/w) Fe b) % (w/w) Fe;O4 in the sample.1. A sample containing magnetite, Fe;O4, was analyzed by dissolving a 1.5419-g sample in concentrated HCl, giving a mixture of Fe²+ and Fe+. After adding HNO3 to oxidize any Fe2+ to Fe+, the resulting solution was diluted with water and the Fe precipitated as Fe(OH)3 by adding NH3. After filtering and rinsing, the residue was ignited, resulting to 0.8525 g of pure Fe2O3. Calculate the: a) % (w/w) Fe b) % (w/w) Fe;O4 in the sample.
- To determine the amount of magnetite, Fe3O4 in an impure ore, a 1.5419 g sample is dissolved in concentrated HCl to obtain a mixture of Fe2 + and Fe3 +. After HNO3 is added to oxidize Fe2 + to Fe3 + and diluted with water, Fe3 + is precipitated as Fe (OH) 3 by adding NH3. 0.8525 g of pure Fe2O3 is obtained by filtering, rinsing and burning the precipitate. Calculate the percentage of Fe3O4% in the sample. (Fe = 55,847g / mol, O = 15,999g / mol)93 Chemistry I Laboratory Manual, 2019 Revision Questions: gy muibor alo vialom od W (E 1) Samples containing iron(II) ion can be titrated with solutions containing dichromate ion under acidic conditions. OCHS Cr2072- + 6Fe2+ + 14H* → 2Cr+ + 6Fe3+ + 7H2O itio (a) Which ion is oxidized in this reaction? (b) Which ion is the reducing agent in this reaction? ry nistry ple. (c) If a 1.924 g sample containing iron(II) sulfate is dissolved and requires 36.1 mL of 0.0100 M K2Cr2O7 solution to titrate it, what is the percent iron(II) sulfate in the at sample? routine tiration de enin rntory skills on of sodiu de KH ph pu that theAnalyze how the nitrate ion oxidizes the copper metal to copper (II) while itself being transformed to NO2 gas in the process. Cu (s) + 4 H3O+ (aq) + 2 NO3- (aq) --> [Cu (H2O)6]2+ (aq) + 2 NO2 (g)
- 2) What is the equilibrium equation for the following reaction? 2) FeS(s) + 2 H3O* (aq) = Fe2*(aq) + H2S (aq) + 2 H2O (g) [Fe2+] [H2S] A) Kc = [FeS] [H3O+]2 [Fe2+] [H2S] C) Kc = [Fe2+] [H2S] [H¿O]² B) Kc = [FeS] [H3O+? [Fe2+] [H2S] [H;O]? D) Kc = [H3O*]2 [H3O*j2Cr(OH)3(s) + C?O-(aq) > Cr042-(aq) + Cl2(g) (basic solution) balanceGiven the balanced equation: 16H+ + 2MnO4- + 5C2O42- --> 2Mn+ + 10CO2 + 8H2O If .184 g of green K3[Fe(C2O4)3]*3H2O was titrated with 19.5 mL .0310 M KMnO4, what is the percent purity? (I do not understand because there are not even any potassium in the equation to begin with. I do not know what to use to calculate molar mass or mole rations)