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What is the pH of a 0.15 M solution of f...

What is the pH of a 0.15 M solution of formic acid, HCOOH ?
`{:("Formic Acid",K_a),(HCOOH,1.9xx10^(-4)):}`

A

1.49

B

2.27

C

3.72

D

4.55

Text Solution

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The correct Answer is:
d
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Knowledge Check

  • What is the [HCOO^-] in the solution that contains 0.015 M HCOOH and 0.02 M HCl ? K_a(HCOOH)=1.8xx10^(-4)

    A
    `1.8xx10^(-4)`
    B
    `1.35xx10^(-4)`
    C
    `1.8xx10^(-2)`
    D
    `8xx10^(-3)`

  • Refer to an aqueous solution of formic acid, HCOOH , which has a K_(a) value of 1.9 xx 10^(-4) at 25^(@)C . What is the percent ionization of a 0.10 M solution of formic acid at 25^(@)C

    A
    `0.19%`
    B
    `1.4%`
    C
    `4.4%`
    D
    `14%`

  • Refer to an aqueous solution of formic acid, HCOOH , which has a K_(a) value of 1.9 xx 10^(-4) at 25^(@)C . How many moles of sodium formate must be added to 1.0L of a 0.20M formic acid solution to produce a pH of 4.00 ?

    A
    `0.38`
    B
    `0.80`
    C
    `1.9`
    D
    `3.8`

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    Calculate the degree of dissociation and concentration of H_(3)O^(+) ions in 0.01 M solution of formic acid (K_(c) =2.1 xx 10^(-4) " at " 298 K)

    Calculate the degree of dissociation and concentration of H_(3)O^(+) ions in 0.01 M solution of formic acid. K_(a)=2.1xx10^(-4) at 298 K.

    Calculate the degree of ionisation and concentration of H_(3)O^(+) ions in a solution of 0.01 M formic acid (K_(a)= 2.1 xx 10^(-4))

    Calculate the concentration of the formate ion present in 0.100 M formic acid (HCOOH) solution at equilibrium (K_(a) = 1.7xx10^(-4)) .

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