In the following net ionic equation, identify each species as either a Br In the

Question

In the following net ionic equation, identify each species as either a Br

In the following net ionic equation, identify each species as either a Br nsted-Lowry acid or a Br nsted-Lowry base. HSO_3- (aq) + HNO_2 (aq) rightarrow H_2SO_3 (aq) + NO_2- (aq) In this reaction: the formula for the conjugate (acid or base) HSO_3- is ? the formula for the conjugate (acid or base) of HNO2 is ? In the following net ionic equation, identify each species as either a Br nsted-Lowry acid or a Br nsted-Lowry base. In this reaction: the formula for the conjugate (acid or base) of NO2- is the formula for the conjugate (acid or base) of HCO3- is

Explanation / Answer

1) A bronsted is acid is the one which donates a proton ( H+) and bronsted base is the one which accepts a proton .

SO from the given reaction

  HSO_3- (aq) + HNO_2 (aq) -------> H_2SO_3 (aq) + NO_2- (aq)

here No2 is donating the proton .So it is bronsted lowry acid .

Hs03- is acepting a proton .So it is a bronsted lowry base .

Removing a proton from a bronsted acid gives a conjugate base .

So N02- is a conjugate base

adding a proton to a bronsted base gives a conjugate acid

So H2S03 is the conjugate acid .

HN02 ----> bronsted acid

HS03- ----> bronsted base

N02- ----> bronsted base

H2S03 -----> bronsted acid

2) N02- + Hc03- ------> HN02 + C032-

here HC03- is donating the proton .So it is bronsted lowry acid .

N02 is acepting a proton .So it is a bronsted lowry base .

Removing a proton from a bronsted acid gives a conjugate base .

So C032- is a conjugate base

adding a proton to a bronsted base gives a conjugate acid

So HN02 is the conjugate acid .

So HC03- ----> bronsted acid

N02 ----> bronsted base

C032- ----> bronsted base

HN02 -----> bronsted acid

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