How much quantity is needed to prepare 250ml of 0.1M Hydrochloric Acid Solution from commercially available 35%Hydrochloric Acid.(density=1.16)?
the preparation will contain .025 moles of HCl
the commercial solution is 35% HCl by mass
find the mass of HCl needed ... moles * molar mass
find the mass of commercial solution needed
To prepare 250ml of 0.1M hydrochloric acid (HCl) solution from commercially available 35% hydrochloric acid, we can use the following steps:
Step 1: Calculate the molar mass of HCl
The molar mass of HCl is the sum of the atomic masses of hydrogen (H) and chlorine (Cl).
H: 1.007 g/mol
Cl: 35.453 g/mol
Molar mass of HCl = 1.007 + 35.453 = 36.460 g/mol
Step 2: Calculate the amount of HCl needed in grams
To calculate the amount of HCl needed, we need to use the formula:
Amount (in grams) = volume (in liters) * concentration (in moles/liter) * molar mass (in grams/mole)
Given:
Volume = 250 ml = 0.25 L
Concentration = 0.1 M
Amount (in grams) = 0.25 L * 0.1 mol/L * 36.460 g/mol = 0.9115 g
Step 3: Convert the amount of HCl needed to the volume of 35% HCl solution
The 35% HCl solution has a density of 1.16 g/mL. We can use the formula:
Volume (in milliliters) = Amount (in grams) / Density (in grams/milliliter)
Volume (in milliliters) = 0.9115 g / 1.16 g/mL = 0.7869 mL
Therefore, approximately 0.7869 mL of commercially available 35% HCl solution is needed to prepare 250 ml of 0.1 M HCl solution.
To determine the quantity of 35% hydrochloric acid required to prepare 250ml of 0.1M HCl solution, we need to use the concept of molarity and the formula:
Molarity (M) = Moles of solute / Volume of solution (in L)
Step 1: Convert the volume of the solution from milliliters (ml) to liters (L).
250 ml = 250/1000 = 0.25 L
Step 2: Calculate the number of moles of HCl required using the molarity formula.
Molarity (M) = Moles of HCl / Volume of solution (in L)
Rearrange the formula to find the moles of HCl:
Moles of HCl = Molarity (M) x Volume of solution (in L)
Moles of HCl = 0.1M x 0.25 L = 0.025 moles
Step 3: Determine the concentration of the 35% hydrochloric acid in moles per liter.
35% hydrochloric acid means it contains 35g of HCl per 100g of solution. Since the density of the hydrochloric acid is given as 1.16 g/mL, we can calculate the concentration of HCl in moles per liter.
First, calculate the number of grams of HCl in 35% hydrochloric acid:
35% of 100g = 35g
Next, convert grams of HCl to moles of HCl:
Molar Mass of HCl = 1 g/mol
Moles of HCl = Mass of HCl / Molar Mass of HCl
Moles of HCl = 35g / 36.5 g/mol = 0.958 moles
Step 4: Calculate the volume of 35% hydrochloric acid required using the moles-to-volume conversion.
Moles of HCl = Volume of 35% HCl (in L) x Concentration of HCl (in mol/L)
Rearrange the formula to find the volume of 35% HCl:
Volume of 35% HCl = Moles of HCl / Concentration of HCl
Volume of 35% HCl = 0.025 moles / 0.958 mol/L = 0.026 L
Step 5: Convert the volume of 35% hydrochloric acid from liters to milliliters.
Volume of 35% HCl = 0.026 L x 1000 = 26 ml
Therefore, you would need approximately 26 ml of 35% hydrochloric acid to prepare 250 ml of 0.1M hydrochloric acid solution.
Note: Make sure to handle the acid with caution and carry out any dilutions or preparations in a fume hood or a well-ventilated area.