Answer to Question #286327 in Physical Chemistry for Dennis

Question

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) CO₃^2-

all 1 mark

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

CH₃COOH (aq) + HCIO₄ (aq) —-> <—- CH₂COOH₂⁺ (aq) + CIO₄ (aq) (1 mark)

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

HCO₃^- (aq) + H₃O⁺ (aq) —-> <—- CO₂ (g) + H₂O + H₂O (I). ( 2 marks )

please detailed answers with explanation please🙏🏾🙏🏾🙏🏾🙏🏾

Answer 1

Q1

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

(ii) $HClO_4$ is an acid. It donates $H^+$

(ii) $CO_3^2$ is basic.. Because it accepts $H^+$

(b) HClO$_4$ acts as acid . it donates H⁺

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

$HCO_3^-$ is Bronsted Base, it accepts $H^+$

$HCO_3^-+H^+\to\>CO_2+H_2O$

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

$H_3O^+\to\>H_2O+H^+$