Fe in ore can be analyzed by oxidizing Fe to Fe2+ then titrating  Fe2+with K2Cr2O7  .  See equation below.   K2Cr2O7(aq)  +  6Fe2+(aq)  +  14H+(aq)  → 2Cr3+(aq)  +   2K+(aq)   +  6Fe3+(aq)  +   7H2O(l)  What is the stoichiometry  of the analyte and titrant ?

Q: In a titration experiment, H2O2(aq) reacts with aqueous MnO4^1- (aq) as represented by the equation…

A: In  a titration experiment , H2O2(aq) reacts with aqueous MnO4- as represented by the equation- 5…

Q: Write the net ionic equation, including phases, that corresponds to the reaction…

A:

Q: A 1.6394-g sample of limestone taken from Sinuhutan Cave in Brgy. Onop, Miagao was analyzed for Fe,…

A: ib

Q: Predict the products and balance the following reaction: Ag,SO,(aq) + NaCI(aq) - A) Ag,SO,(aq) +…

A: C)   Ag2SO4 (aq) + 2 NaCl (aq) → 2 AgCl (s) + Na2SO4 (aq)

Q: For the analysis of trace metals it is necessary to prepare solutions of very low concentrations…

A: To solve this question we use the total volume strength formula.

Q: a. Ag*, Pb2+ b. Mn2+, Fe+ С. c. Ni2+, Al3+

A: a. Ag+, Pb2+ Here the basic medium --> OH- excess will precipitate Pb(OH)2 and leave Ag+ in…

Q: The average human body contains 6.40 L of blood with a Fe2+ concentration of 1.40×10−5 M. If a…

A: Calculation of no. of mol of Fe2+: No.of mol=Molarity×Volume=1.40×10-5mol/L×6.40 L=8.96×10-5mol…

Q: Which of the following ions form distinctive colors (i.e. not white or colorless) upon addition of…

A: Aluminum  upon addition of aqueous NH3 gives white precipitate of Al(OH)3. Calcium usually does not…

Q: A 0.5000 g sample of a pesticide (DDT, C14H9Cl5, MM 354.49 g/mol) was decomposed with metallic…

A: Number of moles of Cl in AgCl will be same as in DDT. This is due to the fact that mass is…

Q: 3. Sulfuric acid and strontium chloride a. М: b. TI: c. NI: 4. Sulfuric acid and magnesium nitrate…

A: 3. Molecular reaction of sulphuric acid with Strontium nitrate ;. H2SO4 (aq) + Sr(NO3)2 (aq) --->…

Q: Uranium can be isolated from its ores by dissolving it as UO2(NO3)2, then separating it as solid…

A: The balanced chemical equation is as follows,

Q: A 0.750 g sample of finely ground limestone was placed in an Erlenmeyer flask, and 25.00 mL of 1.00…

A: Mass of sample = 0.750 grams Volume of HCl added = 25.0 mL Concentration of HCl added = 1M Volume of…

Q: 3. A sample of KHP, KHCaH.O., weighing 2.035 g is titrated with NaOH and backtitrated with HCI. NaOH…

A:

Q: A solution of hydrogen peroxide,H2O2, is titrated with a solution of potassium permanganate, KMnO4.…

A: Number of moles of KMnO4​=MV/1000 ​=0.145×51.7/1000=7.4×10−3

Q: 2. An iron ore was analyzed by dissolving a 1.1324 g sample in concentrated HC. The resulting…

A: Percentage of Fe and Fe3O4 can be calculated from the total moles of iron present in the sample.

Q: A 0.7785 g sample containing hydrazine (N2H4, rocket fuel) was dissolved and diluted to 250.0 mL in…

A: Answer: This question is based on stoichiometric calculation where we have to convert the moles of…

Q: A sample of pearl ash (impure K2CO3) is titrated with 0.2500 N HCl. If the sample weighs 1.1000 g…

A: Normality is defined as the amount of solute expressed in the number of gram equivalents present per…

Q: What is the net ionic equation of the reaction of MgSO 4  MgSO4 with Pb(NO 3 ) 2  Pb(NO3)2 ?

A: The net ionic equation is given in step 2.

Q: Pb(NO3)2 + Ni(en)1(H20)4SO4 ------> Pb(SO4)(s) + 2NO31- + Ni2+ + 4H2O + 1 en b. How many grams of…

A: Number of atoms, ions and molecules present on a given amount can be determined by “Mole Concept”.…

Q: In an acid-base titration experiment, 36.44 mL of NaOH was placed in the Erlenmeyer flask and…

A: The number of moles of a substance is determined as the mass of a substance upon its molar mass. The…

Q: (ii) A student was given 400 cm of aqueous ammonia solution, NH, (aq). The student was asked to…

A: The balanced reaction given is: 2NH3(aq)+H2SO4(aq)→(NH4)2SO4 Conversion unit: 1 L=1 dm31 L=1000 cm3…

Q: A chemist dissolves a 1.497-g sample of a type of metal (an alloy of Sn, Pb, Sb, and Cu) in nitric…

A: Yield is defined as the amount produced during a reaction. It means that yteld is nothing but the…

Q: 1. H2SO4. The resulting solution contained excess acid and required 15.85 mL of 0.09850 M NaOH for…

A: The balanced equations are   CaCO3 + H2SO4 ----------> CaSO4 + CO2 + H2O    H2SO4 + 2 NaOH…

Q: 0.6465 grams of bleach, Ca(OCI)2, is dissolved in acid and treated with excess KI. Calculate the…

A: Redox titrations are used here to determine mass percentage of Ca(OCl)2 in the bleach sample .…

Q: A sample of soda ash (impure Na2CO3) is titrated with 0.5000 N H2SO4. If the sample weighs 1.1000 g…

A:

Q: Write the net ionic equation for Fe(C2H3O2)3 + Ca(OH)2

A: When Ferric acetate is reacted with calcium hydroxide double decomposition takes place. The products…

Q: 0.6465 grams of bleach, Ca(OCl)2, is dissolved in acid and treated with excess KI. Calculate the…

A: Weight percent of Ca(OCl)2 quantitatively determined by titration.  First excess kI is added with…

Q: Balance the following equation by filling the gaps with appropriate numbers. Co + HCI → CoCl2 +…

A: For balancing an equation, easiest way is to 1st balance that group of elements (compund) which has…

Q: A student is given 1.4571 g of pure CuO. To recover the Cu present in the compound, the dark powdery…

A: In this question, we have given : Mass of pure CuO = 1.4571 gVolume of HCl       = 15.0 mLMolarity…

Q: Complete the following decomposition reaction: (a) Na,CO3(s) + H,Ou) (b) PBSO4(s) +H2O¶ (c)…

A: A decomposition reaction is the one in which a species gets dissociated into more than one. A simple…

Q: 0.5 g sample of an alloy containing 30% (m/m) iron (MM 55.84 g/mol) is dissolved in acid and diluted…

A: Mass of iron in alloy can be calculated using the formula:Mass % = (Mass of element / Mass of…

Q: A 0,4500 g sample of a pesticide (DDT, C14H9Cl5, MM 354,49 g mol^-1) was decomposed with metallic…

A: Given that : Mass of sample of pesticide (DDT, C14H9Cl5) = 0.4500 g Molar mass of pesticide…

Q: An iron ore sample weighing 0.9174 g is dissolved in HCl(aq), and the iron is obtained as Fe2+(aq).…

A: Mass percent provides the information about the solute concentration that is available in any…

Q: 0.5 g of the sample containing KHC204.H2C204 and inert impurities is dissolved in water and…

A: The required reactions are: KHC2O4 . H2C2O4    →Ca(OH)2  2 CaC2O42 CaC2O4 →∆ 2 CaO + 2 CO2 +  2CO

Q: Which of these weighing forms provides the greatest mass of precipitate from a given quantity of…

A: A)      Na2U2O7 ( Molar Mass = 634.0 g/mol)                         % Uranium = 476 g/mol/ 634 g/mol…

Q: Sn2+ can be analysed by reaction with excess Fe3+ and the Fe2+ produced is oxidised back to Fe3+…

A: Here we are required to find the moles of Sn2+ present which was analysed  by redox titration using…

Q: An iron containing sample of mass 0.53 g is first treated with HCI(aq) to convert all iron to Fe*…

A: The ratio of mass of particular atom to the total mass multiply by 100 is known as percent by mass.

Q: K2C204 • H2Olag) + CaCl2 • 2H2O(ag) → CaC2O4 • H2O(s) + 2KCI(ag) + 2H2O) Unspecified amounts of…

A: When CaCl2.2H2O is added to the supernatant, it reacted with the excess potassium oxalate…

Q: For the analysis of trace metals it is necessary to prepare solutions of very low concentrations…

A: Molarity of a solution is defined as the moles of solute present in one litre of solution. It is…

Q: What is the balanced net ionic equation of the following: Cu(NO3)2 + (NH4)3PO4 Li2CO3 + CaCl2…

A: To write the net ionic equation, we will:-  a)write the balanced molecular equation b)We will write…

Q: In the laboratory you are given the task of separating Ca2+ and Ag* ions in aqueous solution. For…

A: When  Ca2+ and Ag+ ions Present in the Solution, then using different type of reagents we can…

Q: A 0.8571 g sample of iron ore is dissolved in acid, the iron is oxidized to the +3 state and then…

A: The mass of the iron ore sample is = 0.8571 g The mass of iron(III) oxide is = 0.1132 g The molar…

Q: 0.5166 grams of iron mineral is dissolved with acid and Fe2+ is titrated with 42.96 mL of 0.0213 M…

A: Solution -  According to the question - Given values are - Molarity of Na2Cr2O7 is 0.0213 M Volume…

Q: Calculate the percentage of Fe in pure iron(II) ammonium hexahydrate: (NH4)2[Fe(SO4)2] x 6H2O

A: The solution is as follows :

Q: Dichromate reacts with aqueous iron (II) ion in acidic solution according to the balanced equation:…

A: During the titration, the moles of species K2Cr2O7 and FeSO4 is equivalent then this point will be…

Q: what mass of precipitate (in g) is formed when 45.5L of 0.300 M Na3PO4 reacts with 59.0 mL of 0.200…

A: Na3PO4 ; Volume = 45.5L  Molarity = 0.300 M = 0.300 mol/L * Moles of Na3PO4 = 45.5 L × 0.300 mol/L =…

Q: 0.6465 grams of bleach, Ca(OCl)2 , is dissolved in acid and treated with excess KI. Calculate the…

A: Given data contains, Mass of bleach is 0.6465 g. The volume of Na2S2O3 is 36.92 mL=0.03692 L.…

Q: 1. A sample containing magnetite, Fe;O4, was analyzed by dissolving a 1.5419-g sample in…

A: A numerical problem based on isolation of metals, which is to be accomplished.

Q: g. Aluminium in 1.200 g sample of impure ammonium aluminium sulphate was precipitated with aqueous…

A: Given: Mass of the sample=1.200g Mass of anhydrous Al2O3=0.1798g Atomic weight of Al=26.98 g mol-1…

Stoichiometry

Stoichiometry is a chemical division that evaluates the quantitative content of the chemical process with the help of the reacting molecules or products taking part in the reaction. The term “stoicheion” in “Stoichiometry”, is an old Greek term for "element" whereas “metron” means "measure".