Question #286327

Acids and Bases

Q1

a) State weather the following species can behave as an acid, as a base , or both:

(i) NH4+

(ii) HCIO4

(iii) CO32-


all 1 mark


b) in the following reaction, identify the reactant that acts as an acid:

CH3COOH (aq) + HCIO4 (aq) β€”-> <β€”- CH2COOH2+ (aq) + CIO4 (aq) (1 mark)


c) identify the acid-base conjugate pairs in the following reactions:

HCO3- (aq) + H3O+ (aq) β€”-> <β€”- CO2 (g) + H2O + H2O (I). ( 2 marks )


please detailed answers with explanation pleaseπŸ™πŸΎπŸ™πŸΎπŸ™πŸΎπŸ™πŸΎ



1
Expert's answer
2022-01-19T06:31:01-0500



Q1


(i) NH4+NH^+_4 is an acid . It donates H+H^+

(ii) HClO4HClO_4 is an acid. It donates H+H^+

(ii) CO32CO_3^2 is basic.. Because it accepts H+H^+


(b) HClO4_4 acts as acid . it donates H+



According to Bronsted- Lowry theory, acid are donors of protons and bases are acceptors of protons (H+)


HCO3βˆ’HCO_3^- is Bronsted Base, it accepts H+H^+


HCO3βˆ’+H+β†’β€…CO2+H2OHCO_3^-+H^+\to\>CO_2+H_2O


H3O(aq)+H_3O^+_{(aq)} is conjugate acid, it donates H+


H3O+β†’β€…H2O+H+H_3O^+\to\>H_2O+H^+








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