Question

Which of the following can behave as Bronsted-Lowry bases in aqueous solution? NHAT o HCO4 HNO2 OCIO4 None of the Above

Answer 1

Solution The Bronsted-Lowery concept to the acids which can loss of an H+ (proton) and base are those who can accept H+ so The acid is a proton donor, and the base is a proton.

Now in options

NH4+ + H20 - - - - > NH3 + H+ ions so it is acid.

HCLO 4 + H2O - - - - - - - - >CLO4 - + H + so acid

HNO2 is also acid.

But CLO4 - is basic because

Answers is ClO4- + H+ --------> HCLO4 so it is bases because taking H+ ion.

Second question has one or more options con firm.

In this

Ba(OH) 2 + H2O - - - - - - - - > Ba2+ +2(OH)-

So OH- can take H+ ion from water so (but Arhinum told OH- nature)

It is Base. (OH- + H+ - - - - - - - > H2O)

B) NH3 is also base  

Because it take H+ and produces

NH4 + (amonium ion)

NH3 + H+ - - - - - - - >NH4+

​​​​​​C) it is acid I already explained u.

D) NO3 - is base because it can take H+ ion

NO3- + H+ - - - - - - - - > HNO3

So answers will be For as rules of Bronsted-Lower

NH3 and NO3- is base.

Because Bronsted-Lowery concept could not explain the OH - theory

I hope you understand the confusion of the

Question.

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