Home
Class 9
CHEMISTRY
Commercially available concentrated hydr...

Commercially available concentrated hydrochloric acid conatins 38% HCl by mass.
What is the molarity of this solution if the density is 1.19 g `cm^(-3)`?

Text Solution

Verified by Experts

`"Volume"="mass"/("density")=100/(1.19)=84.03cm^(3)`
Number of moles of HCl
`=38/(36.5)=1.04` moles
Therefore, molarity = `1.04/(84.03)xx1000=12.38`
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • EQUIVALENT MASS

    CENGAGE CHEMISTRY|Exercise Multiple Choice Questions with One or More Than One Correct Answer|5 Videos

  • EQUIVALENT MASS

    CENGAGE CHEMISTRY|Exercise CHALLENGING EXERCISE|6 Videos

  • EQUIVALENT MASS

    CENGAGE CHEMISTRY|Exercise MANDATORY EXERCISE Exercise Set II|17 Videos

  • ELECTROCHEMISTRY

    CENGAGE CHEMISTRY|Exercise OLYMPIAD AND NTSE LEVEL EXERCISES |10 Videos

  • MOLE CONCEPT AND REACTION STOICHIOMETRY

    CENGAGE CHEMISTRY|Exercise WORKED EXAMPLES|4 Videos

Similar Questions

Explore conceptually related problems

Commercially available concentrated hydrochloric acid contains 38% HCl by mass. (a) What is the molarity of this solution ? The density is 1.19 g cm^(-3) (b) What volume of concentrated hydrochloric acid is required to make 1.00 L of 0.10 M HCl ?

Commercially availiable concentrated hydrochloric acid contains 38% HCl by mass. (a) What is the molarity of this solution? The density is 1.19g mL^(-1) ? (b) What volume of concentrated HCl is required to make 1.00 "litre" of 0.10M HCl ?

Knowledge Check

  • The molarity of 20% by mass H_(2)SO_(4) solution of density 1.28 g cm^(-3) is :

    A
    2.56 M
    B
    1.56 M
    C
    1M
    D
    5 M

  • Concentrated hydrochloric acid is 12.0 M and is 36.0% hydrogen chloride by mass. What is its density?

    A
    `1.22"g mL"^(-1)`
    B
    `1.10"g mL"^(-1)`
    C
    `1.01"g mL"^(-1)`
    D
    `0.820"g mL"^(-1)`

    • Similar Questions

    Explore conceptually related problems

    Commercially available concentrated hydrochloric acid contains 38 % HCl by mass. (i) What is the molarity of the solution if its density is 1.19 "g cm"^(-2) ? (ii) What volume of concentrated HCl is needed to make 1.0 L of 0.2 M HCl solution ?

    Commerically available concentrated hydrochloric acid contains 38% HCl by mass and density 1.19 g cm^(-3) . Calculate the molarity of this solution.

    Commercially available concentrated hydrochloric acid conatins 38% HCl by mass. What volume of concentrated HCl is required to make 1.00 L of 0.10 M HCl?

    Commercially available cone. HCI contains 38% HCI by mass density of 1.19 g cm^(3) . Calculate the molarity of this solution.

    Commercially available conc. HCl contains 38% HCl by mass and has a density 1.19 g cm ""^(-3) . Calculate the molarity of this HCI.

    Commercially available concentrated HC1 is and aqueous solution containing 38% HC1 by mass .If it density is 1.1 g cm^(-3) (a) What is the molarity of the HC1 solution and ( b) mole fractions of HC1 and H_(2)O

    Home
    Profile