percentage KCl

Q: Calculate the Mass of the Sodium Acetate that was created during the reaction of baking soda and…

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Q: A 0.4705 g sample of a pure soluble chloride compound is dissolved in water, and all of the chloride…

A: As per the given information  mass of AgCl is 1.0716 g molar mass of AgCl is 143.35 The calculation…

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

A: Part a)  The reaction for  the given statement is: AlCl3(aq)  + 3AgNO3(s) →3AgCl (s)+…

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: What is the concentration of the NaCl solution that results when 0.150 L of a 0.556-M solution is…

A: The concentration of the NaCl solution is to be calculated

Q: A sample of impure magnesium was analyzed by allowing it to react with excess HCl solution. After…

A: Volume of HCl = 0.10 L Molarity of HCl = 0.750 M Initial moles of HCl = molarity×volume =0.750 M…

Q: impure

A: moles of AgCl = ( mass / molar mass of AgCl )  moles of AgCl = ( 0.9805g / 143.32gmol-1 )  moles of…

Q: What ions are prevented by Magnesium from precipitating? Cobalt Chromium Iron Aluminum

A: Hii there, As there are multiple question posted. we are answering first question. If you need…

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: A 0.5683 g sample of a pure soluble bromide compound is dissolved in water, and all of the bromide…

A:

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: How many grams of PbBr2 will precipitate when excess BaBr2  solution is added to 78.0 ml of 0.524 M…

A: Recall the reaction that will occur here PbNO32 + BaBr2 →PbBr2 + BaNO32 Given that 78.0 ml of 0.524…

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 sample of manganese weighing 3.245 g is dissolved in 2.00 M HCl....   A) When an excess of Na2S…

A: Given, A sample of manganese weighing 3.245 g is dissolved in 2.00 M HCl....   A) When an excess of…

Q: What acid and what base would react in aqueous solution so that the following salts appear as…

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

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Q: A 2.5624-g sample of a pure solid alkali metal chloride is dissolved in water and treated with…

A:

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: A 12.3 g sample of an alloy of Mg and Al produces 1.66 mol of H2 when added to excess HCl. What…

A: Given: Total mass of alloy = 12.3 g. And moles of H2 produced = 1.66 mol. Assuming that there are…

Q: 100.0 mL of 0.2o mol/L sodium carbonate solution fully reacts with excess calcium nitrate solution.…

A: Sodium carbonate reacts with calcium nitrate to form a precipitate of calcium carbonate and the…

Q: A student was given a 3.708-g sample of a mixture of potassium nitrate and potassium bromide and was…

A: Given ; Mass of sample = 3.708 g Mass of AgBr precipitate formed = 2.957 g And the sample contains…

Q: Calculate the mass of the precipitate formed when 250 mL of a 0.100M aqueous solution of silver…

A: Molarity: Number of moles of solute per litre of the solution. Its unit is moles/Litre. M: Molarity…

Q: How many grams of PbBr2 will precipitate when excess AlBr3 solution is added to 66.0 mL of 0.754 M…

A: Given: Concentration (molarity) of Pb(NO3)2 = 0.754 M  Volume of Pb(NO3)2 = 66.0 mL molar mass of…

Q: What mass of iron(III) hydroxide precipitate can be produced by reacting 71.0 mL of 0.240 M…

A: In order to solve this question, we will be using basic mole concepts and stoichiometric methods of…

Q: If 17.9 mL of silver nitrate solution reacts with excess potassium chloride solution to yield 0.301…

A: Molarity is used for calculation of the amount of substance present in a particular volume of…

Q: A mixture contains only sodium chloride and potassium chloride. A 0.1586-g sample of the mixture was…

A:

Q: A 0.8830 g sample of a mixture of NaCl and KCl is dissolved in water, and the solution is then…

A: Given : Mass of mixture = 0.8830 g And mass of AgCl produced = 1.913 g Molar mass of AgCl = Atomic…

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: 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: Calculate the mass of calcium phosphate that will precipitate when excess sodium phosphate solution…

A: you have given - Calcium Nitrate concentration = 0.0132 M Calcium Nitrate Volume = 100 mL

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: A 0.5008 g sample of a pure soluble bromide compound is dissolved in water, and all of the bromide…

A: The percentage of halogen in an organic compound is estimated by Carius method. The formula to find…

Q: Write a balanced chemical equation based on the following description: When a solution of…

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Q: weight of Mn

A:

Q: Write the balanced NET ionic equation for the reaction when aqueous CS:PO4 and aqueous AgNOs are…

A: We have the equation as  Cs3PO4 (aq) + AgNO3 (aq) →Ag3PO4 (s)+ CsNO3 (aq)

Q: A (AGNO3) solution was prepared from silver nitrate (1) by dissolving 1.26 g of salt in a 250 ml…

A: 1.26 g of silver nitrate (1) salt was dissolved in a 250 mL of a volumetric flask. Molecular weight…

Q: A 0.450 M solution of KCI needs to be prepared through dilution. A 2.00 M stock solution will be…

A: 0.450M solution of KCl is to be prepared, Let it be M1 = 0.450 M 2.0 M of stock solution , Let it…

Q: weight of Mn ore

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: Three moles of sodium carbonate are mixed with two moles of lead nitrate in aqueous solution,…

A: Given Reaction Na2CO3 + Pb(NO3)2 -------> 2 NaNO3 + PbCO3 Moles of Na2CO3 added = 3 Moles Of…

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

A: NaCl → Na+ + Cl- Pb(NO3)2 → Pb2+ +2NO3- Pb2+ →2Cl- → PbCl2 (precipitate)  Moles = Molarity * Volume…

Q: After 1,600 grams of an aluminum sulphate sample is dissolved in water, aluminum is precipitated in…

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Q: When an sample of impure potassium chloride (0.4500g) was dissolved in water and treated with an…

A: Given, mass of sample of impure potassium chloride = 0.4500 g Excess reactant = silver nitrate Mass…

Q: A gravimetrical analysis is done with an unknown sample containing AgNO3. A 1.5020-g solid mixture…

A: Given mass of AgCl = 0.6168 g

Q: A sample of 0.5220 g of an ionic compound containing the bromide ion (Br-) is dissolved in water and…

A: First, calculate the moles of AgBr from the given mass as: Molar mass of AgBr = 107.8682 g/mol +…

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: Determine the mass of precipitate in grams that are produced when 25.00 mL of a 0.650 M solution of…

A: The reaction follows like this: CaBr2(aq)+2AgNO3(aq)→2AgBr(s)+Ca(NO3)2(aq) So, here  AgBr = Silver…

Q: Determine the volume of 0.116 M Li3PO4 and 0.0871 M Mg(C2H3O2)2 solutions needed to form 135 g of…

A: Number of mols = volume in L × concentration in M Number of mols = weight / molecular weight

Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.