college

how do you calculate molar concentration for 1.50g NaCl in 100.00mL of solution?

  1. 👍 0
  2. 👎 0
  3. 👁 74
  1. Chemistry is your subject, not college. Putting your subject will get a quicker response most of the time.

    1. 👍 0
    2. 👎 0
    posted by Jen
  2. moles = grams NaCl/molar mass NaCl.

    Then M = moles/0.1 L

    1. 👍 0
    2. 👎 0

Respond to this Question

First Name

Your Response

Similar Questions

  1. chemistry

    If you know that the mass concentration of a NaCl solution is 58.5 g/L, the molar concentration (mol/L) of the solution is ? can sum1 help me plz 1 mol of NaCl has a mass of what? 58.5 g NaCl x (1 mol NaCl/molar mass NaCl) = mols

    asked by brett on June 13, 2006
  2. chemistry

    I have two that I can not figure out: #1: calculate the MOLALITY of 10.00 g/L of the salt, if its molar mass is 100.0 g/mol and solution density D=1.100 g/mL work: 10.00 g NaCl x (1mL/1.100g) x (1kg/1000 mL)= 0.00909 kg 100.0 g x

    asked by sam on November 21, 2015
  3. Chemistry

    Is this answer correct? Calculate the molar concentration of sodium hydroxide solution if 36.00mL of this solution were required to neutralize 25.00 mL of a 0.2000 M solution of hydrochloric acid. .0288M??????

    asked by jordan on May 25, 2011
  4. chemistry

    1. if 15.0mL of 4.5 M NaOH are diluted with water to a volume of 500mL, what is the molarity of the resulting solution? 2. in a acid-base titration, 33.65mL of an 0.148 M HCL solution were required to neutralize 25.00mL of a NaOH

    asked by djella on October 25, 2011
  5. Chemistry

    Concentrated sulfuric acid is 18.4 molar and has a density of 1.84 grams per milliliter. After dilution with water to 5.20 molar the solution has a density of 1.38 grams per milliliter. This concentration of H2SO4 is often used in

    asked by Kevin on January 9, 2011
  6. Chemistry

    What is the molar concentration of 4% (w/v) CH3COOH? Hence calculate the expected titre of 0.1M NaOH solution when reacting with 5.00mL if vinegar.

    asked by Stae on April 18, 2010
  7. Chemistry

    If there are 0.625 g of NaCl left in a beaker that originally contained 75.0 mL of saltwater, what must have been the molar concentration of the original solution? The molar mass of NaCl is 58.44 g/mol.

    asked by Summer on September 11, 2014
  8. Chemìstry

    The following two solutions were combined and mixed well: 150.00 mL of a 3.500 M iron(¡¡¡) nitrate solution and 760.00mL of a 1.600M magnesium nitrate solution. 20.00mL of the final solution was transferred with a pipette into

    asked by Anonymous on April 29, 2014
  9. Chemistry

    The following two solutions were combined and mixed well: 150.00 mL of a 3.500 M iron(¡¡¡) nitrate solution and 760.00mL of a 1.600M magnesium nitrate solution. 20.00mL of the final solution was transferred with a pipette into

    asked by Mantsha on April 29, 2014
  10. Chemistry

    0.1825 g of Fe(NH4)2(SO4)2•6H2O is dissolved in 250.00 mL of solution; this is Solution A. 5.00 mL of Solution A is transferred to another flask, and it is diluted to a total of 100.0 mL to make another solution, which is

    asked by Anonymous on October 16, 2017

More Similar Questions