11. If 56.1 grams of NaCl are dissolved in 44.0 mL of Sulfuric acid, H2SO4 Sulfuric acid has a density of 1.84 grams per mL.  Calculate the following concentration measures. a. Weight/volume percent  b. Weight/weight percent  c. Molarit

Q: I want to make 500 mL of HCl solution with MHCl concentration = 0.1 moL/L from HCl solution which…

A: Given that -  Volume of HCl Solution = 500 mL  Concentration of this Solution = 0.1 mol/L = 0.1 M…

Q: f 33.4 g of Mg(C2H3O2)2 is dissolved in water to make 640 g solution. Calculate the value of…

A: From data, mass of solute = 33.4 g  mass of solution = 640 g As both quantities are given in terms…

Q: The density of a solution that is 30.0 % H C l O3 is 1.167 g/mL. Calculate the molarity of the H C l…

A: Given –The given solution is 30% HClO3Density of this solution = 1.167 g/mLMolar mass of HClO3 =…

Q: What is the concentration of a solution formed by diluting 210mL of 8.6M NaOH solutions to 0.81L ?…

A:

Q: A solution is made using 200.0 mL of methanol (density 0.792 g/mol) and 1049.1 mL of water (density…

A:

Q: 10g

A: According to the question, we have 10 grams of NaCl in 600 g of solution. We need to calculate the…

Q: For a 5.0% solution of CaCl2, calculate the: a. mass of CaCl2 in 360. grams of solution. b.…

A: Mass percentage is defined as the total mass of the substance( solute) divided by total mass of the…

Q: A solution is prepared by mixing 1.28 mol C7H16, 2.92 mol C8H18, and 2.64 mol C9H20. What is the…

A: We know that  % Mole of substance ={ (mole of a substance)/(total mole of solution )}× 100

Q: A 51.24 g sample of AX (Molar mass = 171.34 g/mole) is dissolved in enough water to make 2.1 L of…

A: Mass of solute (AX)=51.24 g Molar mass of AX=171.34 g/mol Moles=Mass/Molar mass Moles =…

Q: Complete the table below by determining the missing quantity in each sample. All solutions are…

A:

Q: Starting with a 6.649 M stock solution of HNO3, five standard solutions are prepared via serial…

A: Given that the initial molarity of stock solution of HNO3 is 6.649 M. It has been diluted to 100 mL.…

Q: A solution of 0.5 M NaOH of volume 100 ml is diluted to to make a solution of 0.2M. Find the volume…

A: Dilution of the solution: On dilution of the solution with the pure water, the mole of solute…

Q: Complete the table below and show the complete and correct solution. a. 105.9g/mol b. 100.9 g/mol…

A: Graham's law:

Q: Suppose that an initial volume (V1) of 1.360 mL of Nacl solution was diluted to V2=9.926 mL to…

A: In the given question dilution of NaCl is taking place.  In such situations, the number of moles of…

Q: 1. a) What volume of 8.40 N Al(OH)3 will be used to prepare 350.0 mL of 2.10 M solution? b) How many…

A: Solution -

Q: 100 90 80 NANO 70 60 CaCl 50 Pb(NO3)2 O 40 KCI NaCl 30 20 KCIO 10 Ce,(SO.) 10 20 30 40 50 60 70 80…

A:

Q: A KNO3 solution is made using a 96.4g  OF KNO3 and diluting to a total solution volume of 1.60 L.…

A: Molarity (M) :-  The number of moles of solute dissolved in one lire of solution is known as…

Q: An aqueous potassium iodate stock solution is made by dissolving 5.49 mol KIO, in sufficient water…

A:

Q: a) Calculate the number of atoms of 'C' in it. b) Calculate the number of atoms of 'H' in it. c)…

A:

Q: A solution of 0.5 M NaOH of volume 100 ml is diluted to to make a solution of 0.2M. Find the volume…

A: Molarity of the solution is the number of moles of the Solute Present in one liter of solution. It…

Q: 4. Calculate the percent by volume of a solution created by adding 75.0 mL of acetic acid to 725 mL…

A: Percent by volume is equal to the volume of acetic acid divided by the volume of solution multiplied…

Q: What volume of 0.362 M KCl solution must be used in order to contain 0.0831 mole of KCl?

A: 1 M KCl solution means 1 mole KCl is present in 1000 mL solution.  So, 0.362 M KCl solution means…

Q: A 50.0 mL sample of 12.0 M HCI is diluted to 200 mL. What is true about the diluted solution? A) the…

A:

Q: concentration expressions? Identify what is being asked in each item. CHOICES:  M % w/w X % v/v m…

A:

Q: 5 g of potassium chloride is dissolved in enough water to make 3.6 L of solution. A) What is the…

A: Formula used :- Concentration (C) = number of moles (n)/volume(L)

Q: How many moles comes out after dissovling 0.63 sodium nitrite in 5 mL of water? Molar weight of…

A:

Q: A 32.5 mL sample of an 5.6 % (m/v) KBr solution is diluted with water so that the final volume is…

A: We have to predict the final concentration.

Q: A solution of 0.5 M NaOH of volume 100 ml is diluted to to make a solution of 0.2M. Find the volume…

A:

Q: 9. What is the normality of a solution containing 150g of HCI in a 4.5L solution? MW- H:1, Cl=35

A: Normality is number of gram equivalents presents in 1 liter  of solution called normality  Molar…

Q: what is the molarity of a sulfuric acid solution containing 572.0g of H2SO4 per liter of solution…

A: Solution stoichiometry is mainly based on the calculation of moles and volumes. These two values are…

Q: 12.24 Concentrated HI is 47.0% HI by mass and has a density of 1.50 g/mL. (a) How many grams of…

A:

Q: A 9.50% by mass solution of acetone (C3H6O) in water has a density of 0.9849 g/mL at 20°C. What che…

A: The given data: The mass % of solution = 9.5 % The density of solution = 0.9849 g/ml To determine =…

Q: Calculate the mass in grams of solute in 235 mLof 1.25 M sulfuric acid solution.

A:

Q: A 51.24 g sample of AX (Molar mass = 171.34 g/mole) is dissolved in enough water to make 2.1 L of…

A:

Q: An aqueous potassium iodate stock solution is made by dissolving 7.39 mol KIO, in sufficient water…

A: Given: The number of moles of KIO3 (Potassium iodate) is 7.39 mol The volume of the solution (V) is…

Q: Part A How much concentrated solution would it take to prepare 2.95 L of 0.585 M HCl upon dilution…

A:

Q: A 300 ml solution of 0.55M sodium Chloride solution was evaporated. How much salt by weight was…

A:

Q: Determine the mass/volume percent of a solution made by dissolving: (a) 18.6 g C2H5OH (ethanol) in…

A: Step 1   Given:   The mass of ethanol is 18.6 g. The volume of ethanol solution is 130.6 mL. The…

Q: Calculate the mass percent of a NaCl solution prepared by mixing 35.0 g NaCl with 125.0 mL of pure…

A: Given that : Mass of NaCl = 35.0 g Mass of water = 125.0 mL = 125.0 g Mass of solution = 35g + 125g…

Q: Consider an aqueous solution of NażCO3 that contains 2.5467 g Na2CO3 (M.M. 105.99) dissolved in…

A: Answer :-  1) The solute is Na2CO3        The solvent is Water…

Q: Calculate the molarity of HCl in a solution, which was prepared by dissolving 5.5 g of HCl (molar…

A:

Q: A solution is prepared by dissolving 5.00 g of NaPH in 750.0 mL of water.   Determine the molar…

A: Part a: Given that, 5.0 g of NaOH is added to 750.0 mL of water. The molar mass of NaOH is 40 g/mol.…

Q: 8. Consider the regular soda solution above as a stock solution that you will use to make 240 mL of…

A: Given: Concentration of Stock solution (regular soda) (M1) = 0.39 M Concentration of working…

Q: Arrange the following solutions from lowest molarity (on the bottom) to highest molarity (on the…

A:

Q: Solutions of hydrogen in palladium may be formed by exposing Pd metal to H2 gas. The concentration…

A: Henry's law basically states that concentration of any gas is directly related to corresponding…

Q: An aqueous sulfurie acid solution contains 571.6 g of H,SO, per liter of solution. It has a density…

A:

Q: What volume of 5.0 M sucrose solution is needed to make 3.00 L of 0.043 M sucrose solution?

A: Given that : For initial solution of sucrose, Concentration (c1) = 5 M For final solution of…

Q: 1. A 0.10 M HNO3 solution will be prepared from concentrated HNO3. Using the method outlined in…

A:

Q: what mass (in g) of disodium phosphate (NaHPOJ must be dissolved in 495.50 ml of water to crate a…

A: Composition of a solution can be ascertained either qualitatively or quantitatively. Molarity is a…

Q: The density of a solution that is 30.0 % H C l O3 is 1.167 g/mL. Calculate the molarity of the H C l…

A: Assuming we have 100 g of solution  Hence mass of HClO3 => 30 = mass of HClO3 X 100 / 100 =>…