Home
Class 12
CHEMISTRY
Calculate the pH of solution obtained by...

Calculate the `pH` of solution obtained by mixing `10mL` of `0.1 M HC1` and `40mL` of `0.2M H_(2)SO_(4)`.

Text Solution

Verified by Experts

Given is the case of a mixture of `2` strong acids.
Mill moles of `H^(+)` form `HCl =10xx0.1=1`
Milli moles of `H^(+)` form `H_(2)SO_(4)=40xx0.2xx2=16`
,.Total millimoles of `H^(+)` in solution =`1+16=17`
`:.[H^(+)]=(17)/(50)=3.4xx10^(-1)( :.[H^(+)]_(f)=(("Millmoles"_("Total"))/(V))`
`:.pH=-log[H^(+)]=-log0.34`
`pH=0.47`
Promotional Banner

Topper's Solved these Questions

  • IONIC EQUILIBRIUM

    RESONANCE ENGLISH|Exercise Board Level Exercise|27 Videos

  • IONIC EQUILIBRIUM

    RESONANCE ENGLISH|Exercise Exercise -1|28 Videos

  • IONIC EQUILIBRIUM

    RESONANCE ENGLISH|Exercise partIII one or more than one options correct type|10 Videos

  • HYDROCARBON

    RESONANCE ENGLISH|Exercise ORGANIC CHEMISTRY(Hydrocarbon)|50 Videos

  • IUPAC NOMENCLATURE & STRUCTURAL ISOMERISM

    RESONANCE ENGLISH|Exercise Advanced Level Problems Part-5|2 Videos

Similar Questions

Explore conceptually related problems

Calculate the pH of solution obtained by mixing 10 ml of 0.1 M HCl and 40 ml of 0.2 M H_(2)SO_(4)

What is the pH of a solution obtained by mixing 10 mL of 0.1 M HCl and 40 mL 0.2 M H_(2)SO_(4) ?(A) 0.74 (B)7.4 (C)4.68 (D)0.468

Calculate the normality of a solution obtained by mixing 100 mL of 0.2 N KOH and 100 mL of 0.1 MH_(2)SO_(4) .

The pH of a solution obtained by mixing 50 mL of 0.4 N HCl and 50 mL of 0.2 N NaOH is

A solution of weak acid HA was titrated with base NaOH. The equivalent point was reached when 40 mL. Of 0.1 M NaOH has been added. Now 20 mL of 0.1 M HCl were added to titrated solution, the pH was found to be 5.0 What will be the pH of the solution obtained by mixing 20 mL of 0.2 M NaOH and 20 mL of 0.2 M HA?

Calculate [Cl^(Theta)], [Na^(o+)], [H^(o+)], [overset(Theta)OH] , and the pH of resulting solution obtained by mixing 50mL of 0.6M HCl and 50mL of 0.3M NaOH .

Calculate the pH of a solution which contains 100mL of 0.1 M HC1 and 9.9 mL of 1.0 M NaOH .

Calculate the normality of a solution obtained by mixing 200 mL of 1.0 N NaOH and 100 mL of pure water.

What will be the pH of a solution formed by mixing 10 ml 0.1 M NaH_(2)PO_(4) and 15 mL 0.1 M Na_(2)HPO_(4) ? ["Given: for "H_(3)PO_(4)pK_(a_(1))=2.12, pK_(a_(2))=7.2]

What will be the pH of a solution formed by mixing 40 ml of 0.10 M HCl with 10 ml of 0.45 M NaOH ?