What mass of Fe(OH)3 will be obtained when 100. mL of 0.240 M FeClz is mixed with 200. mL of 0.182 M NAOH? |g Fe(OH)3

Q: if 1000mL of .200 M aqueous potssium hydroxide is mixed with 100.0 mL of .200 M aqueos magnesium…

A: The precipitation reaction of KOH i.e potssium hydroxide with Mg(NO3)2 i.e magnesium nitrate is  2…

Q: A 55.0mL sample of 0.102M potassium sulfate solution is mixed with 35.0mL of a 0.114M lead(II)…

A: Given,Molarity of potassium sulfate solution = 0.102 M = 0.102 mol/LVolume of potassium sulfate…

Q: A student adds KF to 867 mL of a 0.0020 M Mg(NO3)2 solution. What is the minimum quantity of moles…

A: the solubility product at standard condition is the product of ions formed when a sparingly soluble…

Q: A solution contains 0.0280 M Pb2+(aq) and 0.0280 M Sr2+(aq). If you add SO2−4(aq), what will be the…

A: Given: Concentration of Pb2+ = 0.0280 M = concentration of Sr2+

Q: You want to analyze a silver nitrate solution. (a) You couldadd HCl(aq) to the solution to…

A: The balanced reaction equation for the given reaction is,

Q: An analyst is given 215 mL of a 0.781mol/L calcium perchlorate. How many mL of a 0.60O0M ammonium…

A:

Q: Solid ammonium carbonate is slowly added to 175 mL of a 0.0585 M lead nitrate solution. What is the…

A:

Q: A 185.0 mL sample of 1.200 M Pb(NO₃)₂ is mixed with 99.50 mL of 1.500 M NaCl, and the PbCl₂…

A: The balanced chemical equation for the precipitation of lead (II) chloride can be written as:…

Q: How many grams of magnesium hydroxide will precipitate if 25.0 mL of 0.235 M magnesium nitrate with…

A:

Q: A solution contains 0.0140 M Pb2+(aq) and 0.0140 M Sr2+(aq). If you add SO2−4(aq), what will be the…

A: Ion that has lower value KSP , will precipitate first as its ionic product will overcome the KSP…

Q: Consider a slightly soluble salt with a general form of MX(s) --> M*(aq) + X (aq). If its molar mass…

A: Given: Ksp of salt = 5.4 X 10-5  Molar mass of salt = 241 g/mol. And the solubility reaction is,…

Q: hOW MANY GRAMS OF Ag2CrO4 will precipitate when 86ml of 0.2 molar Ag2CrO4 is added to 500 ml of 6.3…

A: Given information: Volume of AgNO3 = 86 mL Molarity of AgNO3 = 0.2 M Volume of K2CrO4 = 500 mL…

Q: Consider the neutralization reaction 2HNO3(aq)+Ba(OH)2(aq)⟶2H2O(l)+Ba(NO3)2(aq) A 0.105 L sample…

A:

Q: What mass of NaCrO4 is required to precipitate all of the silver ions from 75.0 mL of a 0.100 M…

A: NOTE: please note that molecular formula of sodium chromate indicated is wrong. I have used the…

Q: What mass of Naz CrO4 is required to precipitate all of the silver ions from 45.0 mL of a 0.600 M…

A: Given : Concentration of AgNO3 = 0.600 M Volume of AgNO3 solution = 45.0 mL = 0.045 L…

Q: determine the mass of CuS formed when 100.ml of .100 M H2s and 5.00 ml of .150 M Cu(c2H3O2)2 are…

A: Given the volume and molarity of H2S and Cu(C2H3O2)2. Using these, number of moles of both can be…

Q: What mass of precipitate (in g) is formed when 250.0 mL of 0.285 M MnCl₂ is mixed with excess KOH in…

A: Mass of precipitate of Mn(OH)2 formed is 6.269g.

Q: A 10.5g kixture contains potassium chloride. Excess lead (II) nitrate solution Pb(NO3)2 (aq), is…

A: In a reaction by noticing the stoichiometry we can easily calculate the amount of reactant and…

Q: A 185.0 mL sample of 1.200 M Pb(NO₃)₂ is mixed with 119.50 mL of 1.500 M NaCl, and the PbCl₂…

A: The balanced Chemical Reaction for less Nitrate and sodium chloride is - Pb(NO₃)₂  + 2NaCl ---->…

Q: If 19.3 g of KBr (MM = 119.00 g/mol) are added to a 500.0 mL volumetric flask, and water is added to…

A:

Q: A 55.5mL sample of 0.104M potassium sulfate solution is mixed with 35.5mL of a 0.104M lead(II)…

A: Interpretation: From the given information theoretical yield of PbSO4 in grams is to be determined.…

Q: What mass of Fe(OH)3 will be obtained when 100. mL of 0.240 M FeCl3 is mixed with 200. mL…

A: FeCl3 + 3NaOH → Fe(OH)3 + 3NaCl       millimoles of  FeCl3 = molarity×volume = 100×0.240 = 24 mmol…

Q: For the reaction Ba(NO3)2+H2SO4 =BaSO4+2HNO3 how many grams of Ba(NO3)2 are required to…

A: The answer is givt below

Q: Does a precipitate form if you add 20.00 mL of a 6. 97x10-5 mol/L solution of lead (II) nitrate,…

A: Given,  Molarity of Pb(NO3)2 = 6.97 x 10-5 mole/L  Volume of Pb(NO3)2 in mL = 20.00 mL  Molarity of…

Q: If 45.6 g of CH₃OH (MM = 32.04 g/mol) are dissolved in 500.0 mL of solution, what is the…

A: Given,  45.6 g of CH₃OH (MM = 32.04 g/mol) are dissolved in 500.0 mL of solution

Q: A careless student forgets to label one of their reagent containers. They know it contains one of…

A: The given solution may be one of the following: 0.1 M NaCl0.1 M CaNO320.1 M KCH3COO

Q: A 1.0 sample of an aqueous solution contains 0.10 mol of NaCl and 0.10 mol of CaCl 2.What is the…

A: Given -Volume of soliution - 1 LMoles of NaCl in solution = 0.10 molMoles of CaCl2 in solution =…

Q: A) If 500 mL of .300 M silver nitrate are mixed with 200mL of 0.5 M calcium chloride, how many grams…

A: In a balanced equation, the number of atoms on both sides of the equation should be identical. The…

Q: A 0.7209-g solid mixture containing MgCl2 is dissolved in water and treated with an excess of AgNO3,…

A: Given : Mass of MgCl2 sample = 0.7209 g And mass of AgCl = 1.032 g Molar mass of AgCl = Atomic mass…

Q: A student prepared a Kool-Aid solution from 1.3151 g of Kool-Aid in a 100mL volumetric flask. In an…

A: The concentration of citric acid in 100 mL of prepared solution of Kool-Aid is determined as…

Q: A 75.0g sample of liquid contains 17.5% by mass of H3PO4 (molar mass = 98.0g/mol). If 251.0 mL of…

A: Acid or Base Neutralization :  In a titration reaction when H+ of acid and OH- of a base completely…

Q: What mass of Fe(OH)2

A:

Q: If 25.2 mL of AgNO3 is needed to precipitate all the Cl ions in a 0.775-mg sample of KCI (forming…

A:

Q: A sample of solid Mg(OH)2 was stirred in water at a certain temperature until the solution contained…

A: HClO4 is a strong acid, it reacts with magnesium hydroxide Mg(OH)2 , this is an acid base reaction.…

Q: What mass of Fe(OH)3 will be obtained

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

Q: You mix 275.0 mL of 1.20 M Pb(NO3)2 with 300.0 mL of 1.85 M KI. Calculate the mass of precipitate.

A: Given data : Concentration of Pb(NO3)2 = 1.20 M Volume of Pb(NO3)2 = 275 mL Concentration of KI =…

Q: In a double replacement precipitation reaction, KCl reacts with Pb(NO3)2 in a 2:1 mole ratio,…

A: Potassium chloride reacts with lead (II) nitrate to form potassium nitrate and lead (II) chloride.…

Q: What is the mass of the precipitate formed when 12.0 mL of 0.150 M NaCl is added to 25.00 mL of a…

A: We know that silver chloride is a weak salt its solubility product is very low. Therefore, we can…

Q: What mass of precipitate (in g) is formed when 250.0 mL of 0.300 M MnCl₂ is mixed with excess KOH in…

A:

Q: Suppose that 42.00 mL of 0.150 M NaOH is added to 0.360 g of a weak acid, H3A.  The excess NaOH is…

A: Millimol = Molarity×Volume(in ml) = mass(in mg)÷molar mass

Q: copper (II) ion is precipitated from solution by adding 3.00 M NaOH(aq) resulting in a blue…

A: We will use neutralisation concept

Q: If 26.2 mLmL of AgNO3AgNO3 is needed to precipitate all the Cl−Cl− ions in a 0.780-mgmg sample of…

A: Number of moles of KCl can be calculated as shown below:

Q: Consider the neutralization reaction  2HNO3(aq) + Ba(OH)2(aq) yields to 2H2O(L) + Ba(NO3)2(aq) A…

A: Given: Concentration of Ba(OH)2  = 0.100 M Volume of Ba(OH)2 = 49.3 mL = 0.0493 L Volume of HNO3 =…

Q: A solution contains 0.0130 M Pb2 +(aq) and 0.0130 M Sr2+(aq). If you add So? (aq), what will be the…

A:

Q: Calculate the mass of MgCO3 precipitated by mixing 10.00 mL of a 0.200 M Na2CO3 solution with 5.00…

A: The following reaction is occurring: Determine the moles of Na2CO3 present in the reaction as shown…

Q: Calcium oxalate is very insoluble in water.  What mass of sodium oxalate is required to precipitate…

A:

Q: e solubility of an ionic compound MX (molar mass = 436 is 6.43 x 103 g/L. What is the Ksp ?

A: Given, molar mass of ionic compound MX = 436 g.mol-1 Solubility of the compound = 6.43 ×10-3 g/L