The graph below belongs to a titration between HClO_4(aq) with NaOH_(aq) CH_3COO

Question

The graph below belongs to a titration between HClO_4(aq) with NaOH_(aq) CH_3COOH_(aq) with NaOH_(aq) HCN_(aq) with NaOH_(aq) H_2S_(aq) with NaOH_(aq) In which of the following reactions does NH_3 act as Bronsted acid? NH_3(aq) + HCl_(aq) rightarrow NH_4Cl_(aq) NH_3(aq) + H^+_(aq) rightarrow NH_4^+_(aq) NH_3(aq) + H_2O(l) rightarrow NH_4^+_(aq) + OH_(aq)^+ In which of the following below does water acts as a Bronsted-Lowry acid? NH_3(aq) + H_2O_(l) rightarrow NH_4^+_(aq) H_2O_(l) + CH_3COOH_(aq) rightarrow H_3O^+_(aq) + CH_3COO^-_(aq) H_2O_(l) + CO_3^2-_(aq) rightarrow HCO_3^-_(aq) + OH^-_(aq) (i) and (ii) (ii) and (iii) (iii) only (i) and (iii) Which of the following substances is not a Bronsted acid? HF_(aq) H_2SO_3(aq) NO_3^-_(aq) NH_4^+_(aq) 3.7 g of HCl_(g) are dissolved in 1.0 L of water. The pH of the solution is: 0.1 0.99 1.72 3.7

Explanation / Answer

1) the graph below belongs to a titration between

Ans: (b) CH3COOH(aq) and NaOH(aq)

2) in which of the following reaction does NH3 act as bronsted acid?

Ans:

(c) Na(s) + NH3(aq) ---> NaNH2(aq) + 1/2H2(g)

according bronsted concept of acids and bases, A Bronsted acid is a proton(H+) donor. In the above reaction NH3 donates proton then became bronsted acid.

3) In which of the reaction below does water act as a Bronsted-Lowry acid?

Ans :

option (d): reaction (i) and (iii)

(i) NH3(aq) + H2O(l) ---> NH4+(aq) + OH-(aq)

(iii) H2O (l) + CO32-(aq) ---> HCO3-(aq) + OH-(aq)

according bronsted concept of acids and bases, A Bronsted acid is a proton(H+) donor. In the above reaction H2Odonates proton then became bronsted acid.

4) which of the following substances is not a bronsted acid?

Ans: option-(c) : NO3- (aq)

5 ) 3.7 g of HCl(g) are dissolved in 1.0L of water. the pH of the solution is?

option (b) : 0.99

pH = - log [H+]

Related Questions

Navigate

• Browse (All)
• Browse T
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.