A student carried out the synthesis of aspirin as described using 3.0 g or salicylic acid and 6.0 ml of sccetic anhydide and abtained 1.306 g of asprin Calculate the theoreteical yield of aspirin Calculate the percent yield of aspirin.

Q: Complete the table below by deciding whether a precipitate forms when aqueous solutions A and B are…

A: When aqueous solutions of two salts are mixed, the resulting products if contains insoluble salts…

Q: If 37.2 mL of 0.500 M K2Cr2O7 is mixed with 15.77g of PbSO4, which will be the limiting reactant?…

A: The molar mass of K2Cr2O7  = 294.185 g/molThe molar mass of PbSO4   = 303.26 g/molThe balanced…

Q: What volume in liters of a 7.5 M Fe(NO3)3 solution can.be diluted to prepare 201.2 mL of a solution…

A:

Q: 18. The molarity of a solution formed by dissolving 38.7 g of KCI in 250.0 mL of water is: The molar…

A: Given ,Mass of KCI dissolved = 38.7 gvolume of water = 250.0 mLmolar mass of KCI = 74.55…

Q: Which of the below statements BEST describes the purpose for using moles in chemistry? They help to…

A:

Q: alt. Because the protein solubility depends on the total ion conce alts yielding doubly charged ions…

A: Mass of NaCl = 67.1 gram Moles of NaCl = mass/molar mass = 67.1 gram /58.44 g/mol = 1.148 mol NaCl…

Q: 3. A student followed the procedure of this experiment to determine the percent NaOCl in a…

A: The volume of bleaching solution diluted from The volume of  required to neutralize 20 mL bleaching…

Q: Consider the reaction of 30.0 mL of 0.212 M Bal, with 20.0 mL of 0.315 M Na,PO, How many moles of…

A:

Q: 25.0 mL of 0.350 M NaOH are added to 45.0 mL of 0.125 M copper (II) sulfate.      (a) How many grams…

A: a) The balanced chemical equation for mentioned reaction:

Q: Which solution will form a precipitate when mixed with a solution of aqueous K2CO3 NaCl KNO3…

A: The explanation is given below-

Q: The molar mass of potassium hydrogen phthalate is 204.22 grams per mole. To determine the molarity…

A: Reaction:' KHP (aq) + NaOH (aq) --> KNaP (aq) + H2O (l)  Given:' mass of KHP = 1.32 g molar mass…

Q: How many grams of calcium hydroxide are required to completely neutralize 475 mL of 0.48 M…

A:

Q: A 9.12 g of KCl.MgCl2.6H2O is to be dissolved to prepare a solution in sufficient water to give…

A: Given: The molar mass of KCl.MgCl2.6H2O is 9.12 g. The volume of the solution is 1.500 L.…

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: Which of these pairs of solutions will produce a precipitate when mixed? (A) CaCl2(aq) and…

A: The precipitate will be formed in the reaction only when the compound, formed in the reaction, is…

Q: Lakes that have been acidified by acid rain ( HNO3 and Ha SO4) can be neutralized by a process…

A: The question is based on the concept of reaction stoichiometry. We have to calculate mass of calcium…

Q: If 50.0 mL of NaOH solution is required to react completely with 0.48 g KHP, what is the molarity of…

A: Molarity of a solution represents the concentration of solution, which is generally expressed as…

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: 2. The solubility of KCIO, at several temperatures is shown in the accompanying diagram. Solubility,…

A: Given,a student mixes 10.0 g of KClO3 with 45.0 g H2O at 70 oC. The final solution is:

Q: If 23.9 g of CH₃OH (MM = 32.04 g/mol) are added to a 500.0 mL volumetric flask, and water is added…

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

Q: With 85% H2SO4 by volume in water being used in the reaction, how many moles of water will be added…

A: 85% volume of H2SO4 means 85 ml H2SO4 in 100 ml Solution. And remaining 15 % is water, that is 15 ml…

Q: 25 mL sample of H3PO4 requires 31.15 mL of 0.242 N KOH for its titration. What is the normality of…

A: Solution :    Normality is defined as the number of gram equivalent of solute present in a volume of…

Q: O Chemical Reactions Solving for a reactant in solution 0/5 Bis One way the U.S. Environmental…

A: Given is:Volume of sample = 200 mL = 0.20 Lmass of silver chloride collected = 5.9 mg = 5.9x10-3 g…

Q: Complete the table below by deciding whether a precipitate forms when aqueous solutions A and B are…

A: Answer :-  Solution A  Solution B  Does a precipitation form when A and B are mixed  Empirical…

Q: 3. A student followed the procedure of this experiment to determine the percent NaOCl in a…

A: Given The volume of bleaching solution diluted from The volume of  required to neutralize 20 mL…

Q: Mass of Na2CO3=5g Mass of CaCl2=4.98g Mass of filter paper=1.11g Na2CO3 and CaCl2 combined,…

A: We have to know theoritical yield and percent yield of solid formed

Q: If 0.470 L of water is added to a 30.0 mL of 17.4 M stock solution of acetic acid (CH3COOH), what is…

A:

Q: If 250. mL of 1.00*10-4 M calcium chloride solution is added to 150. mL of 0.00400 M sodium…

A: For the reaction yield 100% it is assumed that the mole of product is also same as the mole of the…

Q: If 1.59 g of the precipitate are obtained, what is the concentration (in M) of Ba2+ ions in the 25.0…

A:

Q: A sample of ordinary table salt is 98.8% NaCl and 1.2% MgCl2 by mass. What is [Cl] if 6.85 g of…

A: This is simple problem of mole no. Here we first have to calculate the no of moles of NaCl and MgCl2…

Q: When silver nitrate and sodium sulfate react, a precipitate forms. What mass of the precipitate is…

A: A)

Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.