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What volume of 12.0 M HCl is required to make 75.0 mL of 3.50 M HCl?
To find the volume of 12.0 M HCl needed to make 75.0 mL of 3.50 M HCl, you can use the formula C1V1 = C2V2. Substituting in the given values, you will find that approximately 21.9 mL of 12.0 M HCl is required.
What is the molarity of the HCl solution if 240 ml of the HCl solution reacts with magnesium to produce 4.60 L of HCl gas measured at STP?
We can use PV = nRT to find moles of HCl (1 atm)(4.60 L) = n(0.08206 L*atm/mol*K)(298.15 K) moles HCl = 0.188 moles Molarity = moles of solute/Liters of solution Molarity = 0.188 moles HCl/0.240 liters = 0.783 Molar HCl =============
How you can find the percentage and specific gravity of unknown HCl?
find, at the given temperature and pressure, weight of HCL and volume of the same. Find density of HCL by Density of HCL= weight/volume Specific gravity of HCL= density of HCL/density of water
What can you find in HCl?
Hydrogen chloride (HCl) contain, of course, hydrogen and chlorine in the molecule.
How many grams of HCl are contained in 4.25mL of a 0.405M aqueous solution of HCl?
M * V = n 0.405 M * 0.00425 ml = 0.00172125 mole of HCl The molar mass of HCl is: 1.007947 + 35.453 = 36.460947 g/mole m = mm * n So the mass in gram is: 36.460947 g/mole * 0.00172125 mole = 0.0628 gram
What volume of 12.0 M HCl is required to make 75.0 mL of 3.50 M HCl?
To find the volume of 12.0 M HCl needed to make 75.0 mL of 3.50 M HCl, you can use the formula C1V1 = C2V2. Substituting in the given values, you will find that approximately 21.9 mL of 12.0 M HCl is required.
What is the molarity of the HCl solution if 240 ml of the HCl solution reacts with magnesium to produce 4.60 L of HCl gas measured at STP?
We can use PV = nRT to find moles of HCl (1 atm)(4.60 L) = n(0.08206 L*atm/mol*K)(298.15 K) moles HCl = 0.188 moles Molarity = moles of solute/Liters of solution Molarity = 0.188 moles HCl/0.240 liters = 0.783 Molar HCl =============
How you can find the percentage and specific gravity of unknown HCl?
find, at the given temperature and pressure, weight of HCL and volume of the same. Find density of HCL by Density of HCL= weight/volume Specific gravity of HCL= density of HCL/density of water
What can you find in HCl?
Hydrogen chloride (HCl) contain, of course, hydrogen and chlorine in the molecule.
How many grams of HCl are contained in 4.25mL of a 0.405M aqueous solution of HCl?
M * V = n 0.405 M * 0.00425 ml = 0.00172125 mole of HCl The molar mass of HCl is: 1.007947 + 35.453 = 36.460947 g/mole m = mm * n So the mass in gram is: 36.460947 g/mole * 0.00172125 mole = 0.0628 gram
Can you find something that has a pH of 6?
0.000001 mol HCl
What is the mole fraction of HCl in an aqueous solution that is 27.2 percent HCl by weight?
To find the mole fraction of HCl in the solution, we first need to calculate the molar mass of HCl (H=1g/mol, Cl=35.5g/mol). Then, determine the number of moles of HCl in 100g of the solution. Finally, calculate the mole fraction of HCl by dividing the moles of HCl by the total moles of solute and solvent in the solution.
Based on your answer to Part B what is the average rate of formation of HCL?
To find the average rate of formation of HCl, divide the change in concentration of HCl by the time interval over which the change occurs. This will give you the average rate at which HCl is being formed.
How many moles are in 2 grams of HCL?
To find the number of moles in 2 grams of HCl, you need to divide the mass by the molar mass of HCl. The molar mass of HCl is approximately 36.46 g/mol. Therefore, 2 grams of HCl is equal to 2/36.46 = 0.055 moles.
What acid and base will you expect to find as constituent of gastric juice?
HCl
How many moles of solute are in 50 mL of a 12 M HCl solution?
To find the number of moles of solute in the solution, first, calculate the amount of HCl in grams using the formula: moles = molarity x volume (in liters). Then, convert the grams of HCl to moles by dividing by the molar mass of HCl (36.46 g/mol).
What acids can you find inside your body?
HCl in the stomach H2CO3 Lactic acid
