A sample of 0.7960 g of an unknown compound containing barium ions (Ba2+) is dissolved in water and treated with an excess of Na,SO4. If the mass of the BaSO4 precipitate formed is 0.8077 g, what is the percent by mass of Ba in the original unknown compound? %

Q: A solution of sodium hydroxide is standardized against potassium hydrogen phthalate (molecular mass…

A: We’ll answer the first question since the exact one wasn’t specified. Please submit a new question…

Q: A sample of 0.3220 g of an ionic compound containing the bromide ion (Br-) is dissolved in water and…

A: Given mass of sample=0.3220 gMass of AgBr precipitated=0.694 g% by mass of Br in sample=?

Q: A sample of 0.3207 g of an ionic compound containing the bromide ion (Br) is dissolved in water and…

A: Number of moles is calculated by dividing given mass with molecular mass.

Q: The calcium in a 300.0 mL sample of natural water was determined by precipitating the cation as…

A: Ca2+(aq) + C2O42-(aq) →CaC2O4(s) CaC2O4(s) →CaO + CO2 +CO Weighing form =Obtained precipitate is…

Q: If 49.2 g of NaI (MM = 149.89 g/mol) are added to a 500.0 mL volumetric flask, and water is added to…

A:

Q: If you start with a solid acid that can be dissolved in water, you can determine the molar mass of…

A: Given that : Mass of acid = 0.447  Volume of water = 10 mL = 0.01 L Volume of base (NaOH) = 18.57 mL…

Q: A sample of 0.3233 g of an ionic compound containing the bromide ion (Br¯) is dissolved in water and…

A: Given information: Mass of sample = 0.3233 g Mass of AgBr = 0.7017 g

Q: A sample of 0.7960 g of an unknown compound containing barium ions (Ba5 is dissolved in water and…

A: The given compound is BaSO4. The molar mass of BaSO4 = Molar mass of Barium + Molar mass of Sulphur…

Q: A sample of 0.8360 g of an unknown compound containing barium ions (Ba2+) is dissolved in water and…

A: The species mass is expressed as the multiplication between the species moles and species molar…

Q: Sulfate samples are to be analyzed by BaSO4 (233.38 g/mol) precipitation. It was known that the SO4…

A:

Q: Write the balanced NET ionic equation for the reaction when aqueous BaCl and aqueous (NHa)2SOa are…

A: Balanced molecular equation for aqueous BaCl2 and aqueous (NH4)2SO4 to give aqueous NH4Cl and solid…

Q: A 0.6247g sample of an ionic compound containing the bromide ion (Br-) is dissolved in water and…

A: Bromide ion reacts with silver nitrate and silver bromide is precipitated during this reaction.  The…

Q: A 0.5620-g sample of an ionic compound containing the bromide ion (Br−) is dissolved in water and…

A:

Q: A solution is prepared by dissolving 27.03 grams of FeCl3* 6H2O, and diluting to give a final volume…

A: Molarity is a concentration term for a solution. The molarity of a given solution is defined as the…

Q: 3. A 0.8838-g sample of an ionic compound containing bromide ions and an unknown metal cation is…

A:

Q: If 50.0 g of CH₃OH (MM = 32.04 g/mol) are added to a 500.0 mL volumetric flask, and water is added…

A: Number of moles =50.0 g/32.04 g/mol                                      =1.56 mol

Q: What mass of iron(III) hydroxide precipitate can be produced by reacting 75.0 mL of 0.105 M…

A: Number of moles of a substance can be calculated by using Molarity ( M ) and volume of solution ( V…

Q: A sample of 0.3220 g of an ionic compound containing the bromide ion (Br−) is dissolved in water and…

A: Calculate the number of moles of AgBr formed. Number of moles = Given massMolar massNumber of moles…

Q: What mass of precipitate (in g) is formed when 20.5 mL of 0.500 M Cu(NO₃)₂ reacts with 24.0 mL of…

A: Cu(NO₃)₂ + 2 NaOH = Cu(OH)2 + 2 NaNO3. From the above chemical equation we can see that , 1 mol…

Q: Enter your answer in the provided box. A sample of 0.8360 g of an unknown compound containing barium…

A: Mass of baso4 ppt=0.7737g Total mass of compound= 0.8360g

Q: A 35 mL of a Na3PO4 aqueous solution and 35mL of a BaCl2 aqueous solution were combined to form…

A: Consider the given information is as follows; Mass of Ba3PO42 = 0.520 g Volume of BaCl2 = 35 mL =…

Q: If 100. mL of 0.400 mol L-1 Na2SO4(aq) is added to 200 mL of 0.600 mol L- NaCl(aq), what is the…

A:

Q: If 27.8 g of CH3OH (MM = 32.04 g/mol) are added to a 500.0 mL volumetric flask, and water is added…

A: Mass = 27.80 g V = 500.00 mL

Q: A 110.520 g sample of mineral water is analyzed for its magnesium content. The Mg+ in the sample is…

A: ppm refers to parts per million which is a unit to express the concentration. It can be expressed as…

Q: Enter your answer in the provided box. A sample of 0.7560 g of an unknown compound containing barium…

A: The balanced chemical equation,  Ba²⁺(aq) + Na2SO4(aq) --> BaSO₄(s) + 2Na+(aq) Molar mass of Ba²⁺…

Q: The concentration of SO42– ions in a 45.0 mL sample of seawater is determined by adding a solution…

A: Given information: Mass of barium sulfate = 0.315 g Volume of sample = 45.0 mL or 0.045 L

Q: What mass of Na2 CrO4 is required to precipitate all of the silver ions from 25.0 mL of a 0.200 M…

A: Molarity of AgNO3 = 0.200 M Volume of AgNO3 solution = 25.0 mL = (25.0 / 1000 ) L = 0.025 L We need…

Q: Question is attached

A: Given, Volume of sodium chromate ( Na2CrO4 ) = 15 mL = 0.015 LVolume of lead nitrate ( Pb(NO3)2 ) =…

Q: If 17.0 g of NaI (MM = 149.89 g/mol) are added to a 500.0 mL volumetric flask, and water is added to…

A: Given, the amount of NaI =17.0 grammolar mass of NaI =149.89 g/molvolume of solution =500.0 mL =0.5…

Q: If 25.5 mL of a 0.123 M solution of iodide was added to 22.3 mL of a 0.209 M solution of iodate ions…

A: The reactants given are iodide i.e I- and Iodate i.e IO3- and the product forming is I3-. Hence the…

Q: mixture contains Mg(NO₃)₂ and KBr. A 1.85 g sample of this mixture is dissolved in water and an…

A: Given: Weight of sample containing  Mg(NO₃)₂ and KBr =1.85 g The mass of the precipitate = 0.475 g…

Q: A 0.5662-g sample of an ionic compound containing chloride ions and an unknown metal is dissolved in…

A: To calculate percent mass of chlorine in sample we first calculate the mass percent of chlorine in…

Q: The calcium in a 300.0 ml sample of natural water was determined by precipitating the cation as…

A: Answer: This question is based on stoichiometric calculation where we have to find out the number of…

Q: Phosphate in wastewater samples can be precipitated out as Ca10(PO4)6(OH)2 (1,004.6 g/mol).…

A: Given that phosphate in wastewater samples can be precipitated out as Ca10PO46OH2.And municipal…

Q: A sample of 0.3291 g of an ionic compound containing the bromide ion (Br) is dissolved in water and…

A: Given Mass of sample = 0.3291 g Mass of AgBr = 0.6905 g Moles of AgBr = mass of AgBrmolar mass of…

Q: What mass of precipitate (in g) is formed when 20.5mL of 0.300M Ni(NO3)2 reacts with 24.5mL of…

A: Molarity = moles of solute/volume of solution (L)  So, moles = molarity × volume  Number of moles =…

Q: Q5: A sample of 0.676g of an unknown compound containing barium ions (Ba+) is dissolved in water and…

A: The required reaction is : Ba2++ Na2SO4→BaSO4+2 Na+ mass of BaSO4 precipitated =0.4105 g

Q: 2) ) A student who wants to make the determination of calcium, and he dissolved impure 0.1453 g…

A:

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: A 1.345 gram sample of a compound containing barium and oxygen was dissolved in hydrochloric acid to…

A: Given,          Mass of compound = 1.345 grams          Mass of barium chromate produced = 2.012…

Q: Excess Na2SO4(aq) is added to a 4.41×102 mL sample of industrial waste containing Ba2+ ions. If 55.5…

A: Molarity is a term used for concentration which shows the moles of solute dissolved per liters of…

Q: Calculate the total mass, in grams, of precipitate produced when 10.0 mL of 2.50 M SrS (aq) reacts…

A: The volume of SrS = 10 mL or 0.01 L Molarity of SrS = 2.50 M

Q: A 0.5620 g sample of an ionic comopund containing the bromide ion (Br-) is dissolved in water and…

A: Mass of the sample containing the bromide ion (Br-) = 0.5620 g Mass of AgBr precipitate = 0.8868 g…

Q: A sample of limestone weighing 1.005 grams is dissolved in 75.00 mL of 0.250 M hydrochloric acid.…

A: The no of moles of solute taking part in a reaction can be calculated by the following formula. no…

Q: Calculate the total mass, in grams, of precipitate produced when 10.0 mL of 2.50 M SrS (aq) reacts…

A: The reaction of SrS with ZnSO4 is ZnSO4+SrS→ZnS+SrSO4

Q: what mass of precipitate forms when 30 mL of .150 M K2S reacts with 50 mL of .200 M Ba(NO3)2?

A: It is given that:Volume of K2S = 30 mLConcentration of K2S = 0.150 MVolume of Ba(NO3)2 = 50…

Q: In a titration experiment, a student finds that 23.48 mL of a NaOH solution are needed to neutralize…

A: Stoichiometry, in balanced chemical reaction is defined by the ratio at which reactants are reacting…

Q: When 0.620 g of BaCl2·2H2O(molar mass = 244 g/mol) and 0.782g of Na3PO4.12H2O (molar mass = 380…

A: Recall the reaction that will occur between 0.620 g of BaCl2.2H20 and 0.782 g of Na3PO4.12H20…

Q: A sample of 0.6760 g of an unknown compound containing barium ions (Ba) is dissolved in water and…

A: Introduction The mass percentage of any particular compound can be calculated by simply applying the…

Q: When aqueous FeCl3 is combined with 100.0 mL of a base solution containing Ba(OH)2, 0.567 g of a…

A: Given data,Mass of precipitate(Fe(OH)3)=0.567gVolume of Ba(OH)2=100mL=0.100L

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.