Chemistry

calculate the final concentration if 4.0 L of 1.5 M NaCl and 2.0 L of 3.0M NaCl are mixed.

I am confused about how to calculate the final concentration. We are currently working on solutions. I think first I need to divide the amount of the solution by the amount of the solute and then do the mass percent or do I use moles of a solute divided by L of solution?

  1. 👍
  2. 👎
  3. 👁
  1. Would it be volume divided by moles then convert to g

    1. 👍
    2. 👎
  2. mols is the only way to go.
    4.0 L x 1.5 M = ?? mols NaCl
    2.0 L x 3.0 M = ?? mols NaCl.
    Total mols NaCl/total L NaCl = M NaCl.

    1. 👍
    2. 👎

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chem

    1) Which solution will have the lowest OH- A) Na2CO3 B) NaHCO3 C) NaCl D) NaHSO4 E) NH4Cl 2) Which solution will be the strongest base? A) Na2CO3 B) NaHCO3 C) NaCl D) NaHSO4 E) NH4Cl 3) Which aqueous solutions are acidic? A)

  2. Chemistry

    Information beforehand: mass of weighing vial + NaCl / g 16.2597 mass of “empty” weighing vial / g 14.8136 mass of NaCl used / g Final volume of solution / L 0.2500 Questions: 1) Calculate the concentration of the NaCl

  3. chemistry.

    What is the concentration (M) of a NaCL solution prepared by dissolving 9,3g of Nacl in sufficient water give 350ml of solution?.Any idea???

  4. chemistry

    A 2.500×10−2M solution of NaCl in water is at 20.0∘C. The sample was created by dissolving a sample of NaCl in water and then bringing the volume up to 1.000 L. It was determined that the volume of water needed to do this was

  1. Chemistry

    Naoh (aq) + HCl (aq) --> NaCl (aq) + H2O (l) Using the dT determined in part 1, calculate the heat capacity of the calorimeter. Enthalpy of reaction= -58.3 kj/mol, Cs (NaCl = 3.91j/g C)density of 1 M NaCl = 1.037g/mL. dT= 12.88

  2. chemistry

    calculate the mass, in grams, of NaCl present in each of the following solutions. 6.25 g of 11.5% NaCl solution 452 g of 12.3% NaCl solution please show me how to do these. Thanks.

  3. chemistry

    10.00 mL of 0.100 M (NH4)2SO4 is combined with several other solutions (none of which contain SO4-2) to produce a final solution with a volume of 60.00 mL. Calculate the concentration (in moles per litre) of SO4-2 in the final

  4. chemistry

    A chemist must dilute of M aqueous magnesium fluoride solution until the concentration falls to M . He'll do this by adding distilled water to the solution until it reaches a certain final volume. Calculate this final volume, in

  1. Chemistry

    1. You have been given a sample of unknown molarity. Calculate the molarity of a solution which has been prepared by dissolving 8.75 moles of sodium chloride in enough water to produce a solution of 6.22l. 2. You have a sample

  2. Chemistry

    A mass of 0.630 g of NaCl is dissolved in 525 g of water. CAlculate the molality. mass of NaCl= 0.630g mass of H20= 525g molar mass of NaCl= 58.44 This is what i did it keeps telling me the answer is wrong. Convert grams to moles

  3. chemistry

    Calculate the concentration of all species in a 0.145 M solution of H2CO3 (Ka1 is 4.3×10−7 and Ka2 is 5.6×10−11). Calculate the concentration of H2CO3. Calculate the concentration of HCO−3. Calculate the concentration of

  4. chem

    15.00 mL of 0.200 M KI is combined with several other solutions (none of which contain K+) to produce a final solution with a volume of 60.00 mL. Calculate the concentration (in moles per litre) of K+ in the final solution.

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