Question

Define an acid acconding to the Arrhenis theory and wvite a balanced equation to support this definition 2 Define a base accending to the Bonsted-Lowry thony Write a balanced oquation in suppot ef this defisition, in which the base is acting as a Bensted Lowry base but not as n Arrhaius base Formic cid, HCOOH, is a weak acid with apk,e3.74 Draw up a reaction table for the tion of 0,300 M fomic acid with water, and caliculate the pll of this solution Consider the following gas-phase equilibriurn reaction If 1.0 mol of NO is introduced into a 1.0L container at 2000 C, what is the concentration t NO when equilibeium is rached Consider the oquilibrium Prodict and explain how or whether the olloming actions would affoct this cquilibeium a adding more solid A b.lowering the temperature e. increasing the pressure on the system by soducing ins velume d. adding helium gas to increase the sotal peess 6. Logically prove, starting by writing basic autoinization equilibrium reaction of water, that the pH of pure is 7 at 25°C.
please post all balanced equations and reaction tables that may be used. show work.

Answer 1

1) Arrhenius acid:

Any species that increases concentrations H⁺ ions in the aqueous solution.

Ex:   HBr (aq) + H₂O(l) -------------> H₃O⁺ (aq) + Br^- (aq)

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2) Bronsted lowry base:

Any species that accepts a proton.

Ex: NH₂^- + C₆H5OH ---------> C₆H₅O^- + NH₃

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3) HCOOH + H₂O ---------> HCOO^- + H₃O⁺

0.3 M 0 0

0.3-X X X

Then,

Ka = [HCOO-] [H3O+]/[HCOOH]

Given that pKa of HCOOH = 3.74

Ka = 10^-pka = 10^-3.74 = 0.00018

Then,

Ka = [HCOO-] [H₃O+]/[HCOOH]

0.00018 = X.X/(0.3-X)

On solving, X = 0.00726 M

[H3O+] = X = 0.00726 M

pH = -log[H+]

= -log [H3O+]

= -log (0.00726)

= 2.14

pH = 2.14