Home
Class 12
CHEMISTRY
Calculate [H^(o+)] in a soluton that is ...

Calculate `[H^(o+)]` in a soluton that is `0.1M HCOOH` and `0.1 M HOCN. K_(a)(HCOOH) = 1.8 xx 10^(-4), K_(a) (HoCN) = 3.3 xx 10^(-4)`.

Text Solution

Verified by Experts

Given is the case of a mixture of two weak monoprotic acids
So applying direct relation:
`[H^(+)]=sqrt(C_(1)k_(a_(1))+C_(2)K_(a_(2)))`
`=sqrt(0.1xx1.8xx10^(-4)+0.1xx3.3xx10^(-4))`
`=7.14xx10^(-3)M`
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

What are [H^(o+)], [A^(Theta) , and [B^(Theta)] in a solution that is 0.3M HA and 0.1M HB? K_(a) for HA and HB are 1.38 xx 10^(-4) and 1.05 xx 10^(-10) , respectively.

What are [H^(o+)], [A^(Theta) , and [B^(Theta)] in a solution that is 0.3M HA and 0.1M HB? K_(a) for HA and HB are 1.38 xx 10^(-4) and 1.05 xx 10^(-10) , respectively.

Calculate [H^+],[HCOO^(-)] and [OCN^(-)] in a solution that contains 0.1 M HCOOH (K_a=2.4xx10^(-4)) and 0.1 M HOCN (K_a=4xx10^(-4)) .

Calculate the molar solubility of Fe(OH)_(3) in a buffer solution that is 0.1M in NH_(4)OH and 0.1M in NH_(4)Cl (K_(b) of NH_(4)OH=1.8xx10^(-5) , K_(sp) of Fe(OH)_(3)=2.6xx10^(-39) )

Calculate the pH of a solution containing 0.1 M CH_(3)COOH and 0.15 M CH_(3)COO^(-) . (K_(a) "of" CH_(3)COOH=1.8xx10^(-5))

What is [H^(+)] in mol//L of a solution that is 0.20 M in CH_(3)COONa and 0.1 M in CH_(3)COOH ? K_(a) for CH_(3)COOH is 1.8xx10^(-5) ?

What is the concentration of CH_(3)COOH which can be added to 0.5M HCOOH solution so that dissociation of both is same. K_(CH_(3)COOH) = 1.8 xx 10^(-5), K_(HCOOH) = 2.4 xx 10^(-4)

Calculate the [Fe^(2+)] in a solution containing 0.2M [Fe(CN)_(6)]^(4-) and 0.1 M CN^(Theta). K_(f)Fe (CN)_(6)^(4-) = 1 xx 10^(24) .

If the concentration of [NH_(4)^(+)] in a solution having 0.02 M NH_(3) and 0.005 M Ca ( OH)_(2) is a xx 10^(-6) M,determine a. [k_(b) ( NH_(3)) = 1.8 xx 10^(-5) ]

Calculate the solubility og AgCN in a buffer solution of pH 3.00 K_(sp(AgCN)) = 1.2 xx10^(-18) and K_(a(HCN)) = 4.8 xx 10^(10) M^(2) .