student is performing an experiment by mixing 10.0 mL of 0.150 M Li3PO4 solution with 12.0 mL of 0.120 M PbCl3 solution to prepare solid PbPO4.   Calculate many mililiter from the excess reactant left unreacted then calculate what is the actual mass of the solid product that the student

Q: What mass of precipitate is formed when 100. mL of  0.350 M  NaCl reacts with  100. mL  of  0.175 M…

A: When an insoluble substance is present in the chemical solution it is called a precipitate.…

Q: Consider the reaction of 30.0 mL of 0.235 M BaI₂ with 20.0 mL of 0.315 M Na₃PO₄. 3 BaI₂(aq) + 2…

A: Given  moles of BaI₂ consumed in reaction = 0.00705 moles

Q: A titration is performed to determine the amount of sulfuric acid, H2SO4, in a 6.5 mL sample taken…

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Q: Determine the percentage by mass of acetic acid (CH3COOH) in vinegar, if 50.0 mL of 0.15 M sodium…

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Q: How many moles of precipitate will be formed when 52.2 mL of 0.350 M AgNO₃ is reacted with excess…

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Q: A 60.5 mL sample of a 0.114 M potassium sulfate solution is mixed with 37.5 mL of a 0.116 M lead(II)…

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Q: How many grams of Ag₂CO3 will precipitate when excess K₂CO3 solution is added to 57.0 mL of 0.658 M…

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Q: Aqueous solutions of the following reactants are mixed. After the reaction goes to completion,…

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Q: When 25 mL of 0.800 M Ca(NO3)2 is added to 75.0 mL of 0.600 M NaF, CaF2 precipitates. What is the…

A: In this question, we have to find out the correct answer of given problem by the help of the…

Q: Tin(IV) sulfide, SnS2, a yellow pigment, can be produced using the following reaction.…

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Q: A 4.2 g mixture of the solid salts Na2S04 (molar mass = 142.04 g/mol) and Pb(NO3)2 (molar mass…

A: The reaction of sodium phosphate and lead nitrate results in the formation of solid lead sulfate and…

Q: Consider the reaction of 30.0 mL of 0.244 M Bal, with 20.0 mL of 0.315 M Na PO4. 3 Bal2(aq) + 2…

A: Since here given balanced reaction is given so we use mole thechnique to solve this problm

Q: A sample of manganese weighing 1.743 g is dissolved in 4.00 M HCl. What (minimum) volume of HCl is…

A: In this question we will apply the concept of redox reaction and we will write the balanced chemical…

Q: A 57.5 mL sample of a 0.122 M potassium sulfate solution is mixed with 39.0 mL of a 0.126 M lead(II)…

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

Q: In the process of salting-in, protein solubility in a dilute salt solution is increased by adding…

A:

Q: If 28.8 mL of lead(II) nitrate solution reacts completely with excess sodium iodide solution to…

A:

Q: If 22.0 g of CH₃OH (MM = 32.04 g/mol) are added to a 500.0 mL volumetric flask, and water is added…

A: Mass of CH3OH = 22.0 g  Molar Mass = 32.04 g/mol  Volume = 500.0 mL  = 0.5 L

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: What mass of precipitate (in g) is formed when 45.5 mL of 0.300 M K₃PO₄ reacts with 64.0 mL of 0.200…

A: When stoichiometric coefficient results in the equal number of atoms of each element on both the…

Q: How many grams of Ag2CO3 will precipitate when excess K2C03 solution is added to 77.0 mL of 0.693 M…

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Q: (in g)

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Q: Consider the reaction below: Pb(NO3)2 + HCl → PbCl₂ + HNO3 > Molarmass of Pb(NO3)2 = 321.2 g/mol;…

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Q: What mass of precipitate will form when 23.1 mL of a 1.33 M copper (II) sulfate solution is mixed…

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Q: How many grams of Ag,CO3 will precipitate when excess (NH4)2CO3 solution is added to 62.0 mL of…

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Q: A 0.123g sample of the mineral thernadite is analyzed via gravimetric analysis by dissolving the…

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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: A student forgets to weigh a mix ture Of sodium bromide dihydrate and magnesium bromide hexahydrate.…

A: Given data, Mass of H2O looses on heating =252.1 mg  Moles of AgBr formed = 6.00×10-3 mol

Q: A sample contains MgCl2 (95.211 g/mol) and KCl (74.551 g/mol). A 6.3674-g sample was dissolved in…

A: Precipitation refers to formation of product as solid mass that settles at the bottom. Such…

Q: A sample of 0.7160 g of an unknown compound containing barium ions (Ba2+) is dissolved in water and…

A: Percent Mass of element in a compound is mass of element to the mass of compound.

Q: Consider the reaction: Ag⁺(aq) + Cl⁻(aq) → AgCl(s) How many grams of NaCl would be needed to

A: "Since you have asked multiple questions, we will solve the first question for you. If you want…

Q: What mass of precipitate (in g) is formed when 20.5 mL of 0.300 M Ni(NO₃)₂ reacts with 23.5 mL of…

A:

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: How many grams of Cu(OH)2 will precipitate when excess KOH solution is added to 41.0 mL of 0.618 M…

A: To solve this problem we will use the given balanced chemical equation.

Q: What quantity in moles of precipitate will be formed when 213.0 mL of 0.250 M LiCI is reacted with…

A: Given -> Volume of LiCl = 213.0 ml Molarity of LiCl = 0.250 M

Q: The concentration of SO42– ions in a 60.0 mL sample of seawater is determined by adding a solution…

A: Volume of sea water sample is 60 mL Mass of BaSO4 is 0.448 g Concentration of sulfate in mmol/L =?

Q: An excess oxalic acid, H2C¿O4, is added to an aqueous solution of the sample which contains Calcium…

A: To determine which compound forms a precipitate, we have to know the solubility rules. According to…

Q: The precipitated compound, and the mass of this precipitated compound when 0.015 L of 0.337 M…

A: Number of moels of the substance is equal to the ratio of mass to the molar mass of the substance.…

Q: If 0.326 g of aluminum chloride dissolved in water and the whole solution was reacted with excess…

A: The net ionic equation is defined as the equation in which only those chemical species are shown…

Q: Using dimensional analysis, solve the following. How many grams of PbCl2 will precipitate when…

A: The amount of PbCl2 will precipitate is to be calculated

Q: A sample contains MgCl2 (95.211 g/mol) and KCl (74.551 g/mol). A 6.3674-g sample was dissolved in…

A: Molar mass of MgCl2 = 95.211 gmol Molar mass of KCl = 74.551 gmol Mass of sample = 6.3674 g Volume…

Q: How many grams of Cu(OH)2 will precipitate when excess KOH solution is added to 60.0 mL of 0.755 M…

A: To solve this first we have to calculate the number of mole of Cu(NO3)2  then we will calculate the…

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Q: What mass of iron(III) hydroxide precipitate can be produced by reacting 93.0 mL of 0.270 M…

A: Volume of iron (III) nitrate = 93.0 ml  Molarity of iron (III) nitrate = 0.270 M  Volume of sodium…

Q: Determine the mass of CuS formed when 100. mL of 0.100 M H2S and 50.0 mL of 0.150 M Cu(C2H3O2)2 are…

A: The question is based on the concept of Reaction Stoichiometry. we have to calculate mass of copper…

Q: Jack was asked to determine iron (55.845 g/mol) content in dietary supplement. He took few random…

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Q: You mix 29.0 mL of 0.312 M FeCl3 with 38.5 mL of 0.446 M NaOH. What mass of Fe(OH)3 (in grams) will…

A: We have to calculate mass of precipitate and concentration of excess reactant left

Q: How many grams of Cu(OH)2 will precipitate when excess Ba(OH)2 solution is added to 44.0 mL of 0.613…

A: Number of mols = Molarity × Volume (L) In the given reaction, Ba(OH)2 is in excess, so, Cu(NO3)2…

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: How many grams of Ag,CO3 will precipitate when excess Na,CO3 solution is added to 49.0 mL of 0.560 M…

A: Given: molarity of AgNO3 = 0.560 M Volume of AgNO3 = 49.0 mL molar mass of Ag2CO3 = 275.745 g/mol

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".