A 1.7483-g sample containing Al(NO3)3, AlCl3, and inert material was dissolved in acid and divided into two equal portions. One portion was treated with 5.00 mmol of AgNO3. The excess Ag+ required 28.89 mL of 0.l002 M KSCN for titration. The other portion required 26.02 mL of 0.1193 M NaOH for titration: Al3+ + 3 OH- → Al(OH)3(s) Calculate the percentage composition of Al(NO3)3 and AlCl3 in the sample.

Q: A 20.00 mL solution of 0.1200 M TI³+ is titrated with 0.2000 M Fe²+. TI³+ + 2e- TI* Eº = +1.280 V…

A: Given: Volume of Tl3+ = 20.00 mL Concentration of Tl3+ = 0.1200 M Concentration of Fe2+ = 0.200 M To…

Q: Titration of a 0.485 g sample by Mohr method required 36.80 mL of the standard 0.1060 M AgNO3…

A: The complete balanced reaction ;     Cl- + Ag+  →  AgCl(s) Given in the question, Mass of sample =…

Q: A 0.3311 -g sample of pure iron (55.847 g/mol) wire was dissolved in acid, reduced to the +2 state,…

A: We need to find molar concentration of cerium ion.

Q: Calculate the equilibrium constant for the following reaction at 25°C: Fe2 (aq) + 2Ag(s) Fe(s) 2Ag…

A:

Q: 9. What volume of a silver nitrate solution that contains 10.98 g of primary standard AgNO; in 1.00…

A: Mass of AgNO3 = 10.98 g Volume of primary standard AgNO3 = 1.0 L Mass of Na2CrO4 =  0.259 g

Q: A sample of bleach has a content of about 2.13% (w/v) in “active chlorine”. For perform its analysis…

A: Given that, Molecular weight of NaClO = 74.45 g/mol Molecular weight of Cl2 = 70.90 g/mol

Q: Calculate the molar concentration of cadmium(II) ion in equilibrium with solid Cd(OH)2 at pH =…

A:

Q: A 110.0-mL sample of spring water was treated to convert any iron present to Fe2+. Addition of…

A: Answer is 172.4 ppm

Q: A pure oxide of iron weighing 1.000 g is fused with K2S2O7 and the fused material dissolved in acid.…

A:

Q: 0.00247

A: Molarity of KMnO4 = 0.0010 M Volume of KMnO4 = 4.94 mL At equivalent point,  Geq. of KMnO4 = Geq. of…

Q: A 1.000-g sample containing KHC204, H2C204, and impurities required 38.22 mL of 0.1000 M NaOH for…

A: 1.582 m moles of KHC2O4 is present

Q: A 1.000-g sample containing KHC204, H2C204, and impurities required 38.22 mL of 0.1000 M NaOH for…

A: The answer is 1.582 m moles of KHC2O4

Q: As part of a geological team that studied a local cave, you brought with you a bunch of 1.00 g rock…

A: Cacite is also called as Calcium carbonate (CaCO3). Its abundance is very high and is referred as…

Q: The sulfur content of an iron pyrite ore sample is determined by converting it to H2S gas, absorbing…

A:

Q: A Chemist collected a 0.4891-g sample of an ore for Fe determination by a redox titration with…

A:

Q: deposition

A: Given: CuSO4 Solution: 0.01M H2SO4 pH = 4

Q: A 0.2000-g illegal firework was tested for its KClO3 content. The sample was treated with 50.00 mL…

A: Given that -  Mass of KClO3 illegal fireworks = 0.2000 g  Molarity of Fe2+ Solution = 0.01750 M…

Q: 1. A 1.000 g sample.containing Na,C,0, (MM=134 mg/mmol) is titrated with 40.00 mL of 0.0200 M KMNO,…

A: Given,

Q: The volume of 0.0125 mol/L sodium thiosulfate used for titration is 98.7 mL. What is the amount of…

A:

Q: As part of a geological team that studied a local cave, you brought with you a bunch of 1.00 g rock…

A: The reaction taking place will be, MgOH2+EDTA4-  → MgOH2EDTA4- Calculate number of moles of EDTA: 1…

Q: A 0.8040 g sample of an iron ore is dissolved in acid. The iron is then reduced to Fe²+ and titrated…

A:

Q: A0.600 g sample containing arsenic (As) was converted to H,AsO, by suitable treatment. 40.00 mL of…

A:

Q: A 0.600 g sample containing arsenic (As) was converted to H3AS0, by suitable treatment. 40.00 mL of…

A:

Q: A pure oxide of iron weighing 1.000 g is fused with K2S2O7 and the fused material dissolved in acid.…

A: Solution -

Q: The Zn in a 0.6803-g sample of foot powder was titrated with 27.3 mL of 0.04246 M EDTA. Calculate…

A: To calculate the percentage of zinc in the foot powder sample, use the EDTA titration. First…

Q: A waste water containing Fe(HCO3) 2 is discharged to a surface pond. Assuming complete oxidation of…

A: Solution =

Q: 0.683 grams of iron mineral dissolves with acid. Fe2+ is titrated with Ce(SO4)2 solution. Calculate…

A:

Q: A sample of 1.55g of iron ore is dissolved in a acid solution in which the iron is converted into…

A: Given : The titration reaction involves oxidation of Fe2+ to Fe3+ using MnO4- ions which is reduced…

Q: An iron ore sample which weighs 1.097 g is dissolved, the iron reduced to Fe*2, and the resulting…

A:

Q: 1. When Pearl added (NH4)2CO3 solution to an unknown salt solution in basic conditions, the solution…

A: Here we have predict which cation will not precipitate as carbonate when ammonium carbonate is added…

Q: When Cr(III) is oxidized to Cr(VI), its solubility, mobility and toxicity are dramatically…

A: The solution of the question is given below:

Q: 1. A 1.000 g sample containing Na,C,O, (MM=134 mg/mmol) is titrated with 40.00 mL of 0.0200 M KMNO,…

A: It is an application of redox titration where a redox reaction occur between KMnO4 as titrant and…

Q: A Chemist collected a 0.4891-g sample of an ore for Fe determination by a redox titration with…

A:

Q: A 1.000-g sample containing KHC2O4, H2C2O4, and impurities required 38.22 mL of 0.1000 M NaOH for…

A:

Q: The solubility equilibrium for Mn(IO3)2 is:

A: Equilibrium solubility of salt AxBy                                                        AxBy (s)…

Q: A precipitate of AgCl + AgBr weighs 0.8132 gram. On heating in a current of chlorine, the AgBr is…

A: Atomic Mass of Br - 79.904 u Atomic Mass of Cl - 35.5 u Molar mass of AgCl - 143.32 g/mol Molar mass…

Q: A sample of iron ore weighing 0.6248 g is dissolved in acid, the iron reduced to Fe²⁺, and the…

A: Given data,Mass of iron sample=0.6248gVolume of K2Cr2O7=33.60mLNormality of K2Cr2O7=0.1502NFormula…

Q: A sample of magnetite (impure Fe3O4) weighing 0.5000 g is fused with oxidizing flux and the ferric…

A: Magnetite is an ore of Fe with the formula Fe3O4.

Q: Would the addition of K2SO4 to a saturated solution of CaSO4 cause the solubility to increase or…

A:

Q: What chemical could you add to effectively separate Ag+ from AL3+ if both ions are present in a…

A: BY using ion seperation

Q: A 0.7120-g specimen of iron ore was dissolved and passed through a Jones reductor. Titration of the…

A:

Q: If a sample of silver coin weighing 0.2500 g gives a ppt of AgCl weighing 0.2991 g. What wt. of Agl…

A: Since moles = mass / molar mass And molar mass of AgCl = Atomic mass of Ag + Atomic mass of Cl = 108…

Q: A 100.0-mL sample of spring water was treated to convert any iron present to Fe. Titration with…

A:

Q: What is the concentration of Co(OH)₂ (aq) in a solution in which the concentrations of Co²+ and OH…

A:

Q: A sample of unknown iron ore weighs 0.35 g. It is digested using dilute HCl. An SnCl2 solution is…

A: Given that,  Weight of iron ore = 0.35 g The neutralisation reaction take place between Fe2+ and…

Q: Calculate the percent iron in an ore if a 0.3500 g sample is dissolved and the Fe2+ formed requires…

A: In presence of KMnO4 the Fe2+ is oxidised to Fe3+ .

Q: 4. Potassium dichromate is often used to standardize reducing agents like Fe2+: Cr:0, + 6Fe +14 H*…

A: Given data,Volume of Fe2+=34.00mL=0.034LMass of K2Cr2O7=398.5mg=0.3985gMolar mass of…

Q: The acid ionization constant for Fe(H 2O) 62+(aq) is 3 ×10-6. Calculate the pH of a 0.10 M solution…

A: Acid ionization constant denoted by Ka is the equilibrium constant measure of tendency of an acid to…

Q: A 5.70 g iron ore was dissolved in concentrated HCl. After the dissolution, the resulting solution…

A: