chemistry

Concentrated hydrochloric acid has specific gravity of 1.18 and 36% hcl weight. What volume of concentrated hcl must be diluted to give 50 gm of 10 percent.
My calculation
50gm x 0.1 = 5gm
5gm x 36.5 = 182.5
182.5 / 0.36 = 506.9
506.9 / 1.18 = 430 ml This is answer. I am not sure answer. Please help

  1. 👍 0
  2. 👎 0
  3. 👁 229
  1. I don't think 430 mL is correct.
    There a couple ways of doing this. I prefer the first one.
    g x % = g x %
    50 x 10 = g x 36
    g = 13.9 g.
    Then use density to convert to volume.
    v = m/d = 13l.9/1.18 = ?

    OR
    You want to dilute 36% to 10% which is a factor of 36/10 = 3.6 or
    1 part stock + 2.6 parts H2O
    How much is 1 part? That is 50/3.6 = 13.9g and convert that to volume using density.

    1. 👍 0
    2. 👎 0

Respond to this Question

First Name

Your Response

Similar Questions

  1. 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.

    asked by M J on February 21, 2013
  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

    asked by Monique on November 6, 2011
  3. chemistry

    1.) How much ethanol, C2H5OH, in liters (d=0.789g/ml) must be dissolved in water to produce 190.5 of 1.65 M C2H5OH? (Molarity problem.) 2.) How much concentrated hydrochloric acid solution (36.0% HCl by mass, d = 1.18g/mL}), in

    asked by joe on February 12, 2010
  4. Chemistry

    You can purchase hydrochloric acid in a concentrated form that is 37.0 hcl by mass and has a density of 1.20g/mL. Describe how exactly you would prepare 2.85 L of 0.500 M HCL from the concentrated solution.

    asked by Rebecca on May 7, 2014
  1. science

    Describe the preparation of 100 mL of 6.0 M HCL from a concentrated solution that has a specific gravity of 1.18 and is 37% (w/w) HCL

    asked by Density chemistry on February 12, 2015
  2. chemistry

    The amount of sulphuric acid required by a student to perform an experiment was 1500 ml of 2.30M. Explain how you would prepare the required amount of acid to perform an experiment if the label on the available concentrated

    asked by ngombo on September 13, 2018
  3. 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

    asked by Anonymous on April 18, 2016
  4. chemistry

    Concentrated hydrochloric acid has 37.5% of HCl in mass and density of 1.2 g/cm3. What volume (in mL) of concentrated hydrochloric acid should be used to prepare 7 L of a 0.8 mol/L HCl (aq) concentration solution?

    asked by damon on May 16, 2019
  1. Chemistry

    Concentrated hydrochloric acid is 38% HCl by weight and has a density of 1.19 g/mL. A solution is prepared by measuring 70 mL of the concentrated HCl, adding it to water, and diluting to 0.500 L. Calculate the approximate molarity

    asked by JUNDY on March 15, 2015
  2. Chemistry

    HNO3 used as a reagent has a specific gravity of 1.42 g/ mL and contains 70% by strength HNO3. Calculate: Volume of acid that contains 60 g pure acid? Volume of water required to make 1 molar solution from 2 mL concentrated HNO3?

    asked by Anonymous on August 7, 2014
  3. Chemistry

    A solution is prepared by adding 50.3 mL of concentrated hydrochloric acid and 16.6 mL of concentrated nitric acid to 300 mL of water. More water is added until the final volume is 1.00 L. Calculate [H+], [OH -], and the pH for

    asked by Andre on February 28, 2012
  4. chemistry-0.1NHCl

    Hi, A bottle of concentrated Hydrochloric acid (HCl) has the following information stated on it: - Hydrochloric acid 37% 1L ~ 1190kg How do I prepare 0.1N HCl from this concentrated HCl?

    asked by jennie on December 18, 2008

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