chemistry

I have a 0.25 m aquaeous solution of HCL. It's density is 1.05 g/ml. WHat is the % by mass (m/m) of this solution? What is the molarity of the solution?

define molality.
m = # mols/kg solvent.
We have 0.25 m so we must have 0.25 x 36.5 g/mol HCl = 9.125 g HCl/1000 g solvent. The total mass of the solution, then, is 1000 g solvent + 9.125 g HCl = 1009.125 g.
percent by mass = [9.125/1009.125]x100 = ?? and round to the appropriate number of places.

Molarity = # mols/liter of solution.
mass of 1 L of solution = 1.05 g/mL x 1000 mL = 1050 grams.
How much of that is HCl?
1050 g x (%/100) = grams HCl.
grams HCl/molar mass HCl = mols HCl/L which is Molarity.
Check my thinking. Check my numbers carefully.

  1. 👍
  2. 👎
  3. 👁

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    How do I prepare 100mL of 10g/L HCl from concentrated HCl(37%HCl, density 1.19g/mL) Is it 2.28mL of conc HCl dilute to 100mL with water? Please show the calculation steps.

  2. chemistry

    commercially available concentrated Hydrochloric acid is 37.0% w/w Hcl.its density is 1.18g/ml.using this information calculate (a)the molarity of concentrated Hcl,and (b)the mass and volume (in ml)of solution containing 0.315 mol

  3. chemistry

    When 50.0mL of 1.20 M of HCl (aq)is combined with 50.0mL of 1.30 M of NaOH (aq) in a coffee-cup calorimeter, the temperature of the solution increases by 8.01 Degrees C. What is the change in enthalpy for this balanced reaction?

  4. Science

    A hydrochloric acid solution consist of 28.0% HCl, by mass, and has a density of 1.14 g/mL. What volume of this solution is required to react with 1.35 g Al?

  1. chemistry

    10). What is the molarity of an HCl solution if 42.5 mL of a 0.110 M KOH solution is needed to titrate a 25.0-mL sample of the acid? A) 0.187 M HCl B) 0.587 M HCl C) 0.0647 M HCl D) 5.35 M HCl E) 1.70 M HCl

  2. chemistry

    Hydrochloric acid is usually purchased in concentrated form with a 37.0% HCL concentration by mass and a density of 1.20g/mL. How much of the concentrated stock solution in milliliters should you use to make 2.5L of 0.500M HCL

  3. Chemistry

    Perpare 500ml of 1M HCl solution from a bottle of concentrated 37%(W/W) HCL stock with a density of 1.19g/ml. 37%= 37/100 x 100 therefore mass is 37g molarity = mol/vol 1= mol/0.5 mol=0.5 mass of Hcl needed = molxmr mass = 0.5 x

  4. chemistry

    commercially available concentrated hydrochloric acid is 37.0% w/w HCl. Its density is 1.18 g/mL. Using this information calculate (a) the molarity of concentrated HCl, and (b) the mass and volume (in mL) of solution containing

  1. Chemistry

    A 10.0-mL solution of 0.300 M NH3 is titrated with a 0.100 M HCl solution. Calculate the pH after the following additions of the HCl solution: a) 0.00 mL b) 10.0 mL c) 20.0 mL c) 30.0 mL d) 40.0 mL **I know how to solve the

  2. Chemistry

    How much concentrated solution would you take to prepare 2.80L of 0.475M HCl by mixing with water? Hydrochloric acid is usually purchased in a concentrated form that is 37.0% HCl by mass and has a density of 1.20g/mL.

  3. Chemistry

    A 10.0 mL solution of 0.300 M NH3 is titrated with a 0.100 M HCl solution. Calculate the pH after the addition of 20.0 mL of the HCl solution. (potentially useful info: Ka of NH4+ = 5.6 x 10−10)

  4. chem

    The concentration (M) of HCl in a solution prepared by dissolving 5.5 g of HCl in 200 g of C2H6O is ?????? M. The density of the solution is 0.79 g/mL. A) 21 B) 0.93 C) 6.0 × 10-4 D) 1.72 E) 0.58

You can view more similar questions or ask a new question.