n nncrease 16) An aqueous solution of ammonia is found to net ionic equation be basic. This observation can be explained by the 16)_ A) HNOg(aq) + H2O(l) ? NOg-(aq) + H3O+(aq). B) NOg-(aq) + H2O(I) ? HNOg(aq) + OH-(aq). C) NH3(a?)+ H200) NH4 (aa)+OH-(a?) D) NH4 (aa)+H200) NH3(a?) H3o (ag) 17) What is the conjugate acid of HCO3? 17) A) H2CO3 B) H20 C) OH. D) H30+ E) CO32- Co32. 1) 18) What is the conjugate base of H2PO4? 18) A) PO43- B) HPO42- COH- D) H30+ E) H3PO4 19) Which of the following acids will have the strongest conjugate base? 19) A) HCI B) HI C) HCN D) HNO3 E) HCIO4 20 20) Which of the following solutions would have the highest pH? Assume that they are all 0.10 M in acid at 25°C. The acid is followed by its Ka value. A) HCN, 4.9x 10-10 B) HF, 3.5 x 10-4 C) HCHO2, 1.8 x 10-4 D) HCIO2, 1.1 x 10-2 E) HNO2, 4.6 x 10-4 2 21) Which of the following is TRUE? A) A neutral solution contains [H2O] [H30*] B) A basic solution does not contain H30+ C) An acidic solution has [H30*]> (OH] D) A neutral solution does not contain any H30+ or OH- E) None of the above are true.
Solution
16) C
Reason:NH3 is a weak base. In solution form we write it as NH3(aq) the reaction is- NH3(aq) +H2O= NH4+ + OH-
Here OH- is in product side which indicates basic nature as per Brownsted Lowri theory.
17) A
Reason: when a base accepts proton in a solution it is known as conjugate acid O-H + HCO3 2- = H2CO3
18) B
Reason: after donation of a proton what is remaing will be conjugate base here, H2PO4- = HPO4 2- +H+
19) C
Reason: strong acid will have weak conjugate base while weak acid will have strong conjugate base,in given problem HCN is weak acid among all hence HCN will have strong conjugate base.
.
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n nncrease 16) An aqueous solution of ammonia is found to net ionic eq.docx
1. n nncrease 16) An aqueous solution of ammonia is found to net ionic equation be basic. This
observation can be explained by the 16)_ A) HNOg(aq) + H2O(l) ? NOg-(aq) + H3O+(aq). B)
NOg-(aq) + H2O(I) ? HNOg(aq) + OH-(aq). C) NH3(a?)+ H200) NH4 (aa)+OH-(a?) D) NH4
(aa)+H200) NH3(a?) H3o (ag) 17) What is the conjugate acid of HCO3? 17) A) H2CO3 B) H20
C) OH. D) H30+ E) CO32- Co32. 1) 18) What is the conjugate base of H2PO4? 18) A) PO43-
B) HPO42- COH- D) H30+ E) H3PO4 19) Which of the following acids will have the strongest
conjugate base? 19) A) HCI B) HI C) HCN D) HNO3 E) HCIO4 20 20) Which of the following
solutions would have the highest pH? Assume that they are all 0.10 M in acid at 25°C. The
acid is followed by its Ka value. A) HCN, 4.9x 10-10 B) HF, 3.5 x 10-4 C) HCHO2, 1.8 x 10-4
D) HCIO2, 1.1 x 10-2 E) HNO2, 4.6 x 10-4 2 21) Which of the following is TRUE? A) A neutral
solution contains [H2O] [H30*] B) A basic solution does not contain H30+ C) An acidic solution
has [H30*]> (OH] D) A neutral solution does not contain any H30+ or OH- E) None of the
above are true.
Solution
16) C
Reason:NH3 is a weak base. In solution form we write it as NH3(aq) the reaction is- NH3(aq)
+H2O= NH4+ + OH-
Here OH- is in product side which indicates basic nature as per Brownsted Lowri theory.
17) A
Reason: when a base accepts proton in a solution it is known as conjugate acid O-H + HCO3 2-
= H2CO3
18) B
Reason: after donation of a proton what is remaing will be conjugate base here, H2PO4- = HPO4
2- +H+
19) C
2. Reason: strong acid will have weak conjugate base while weak acid will have strong conjugate
base,in given problem HCN is weak acid among all hence HCN will have strong conjugate base.
![n nncrease 16) An aqueous solution of ammonia is found to net ionic equation be basic. This
observation can be explained by the 16)_ A) HNOg(aq) + H2O(l) ? NOg-(aq) + H3O+(aq). B)
NOg-(aq) + H2O(I) ? HNOg(aq) + OH-(aq). C) NH3(a?)+ H200) NH4 (aa)+OH-(a?) D) NH4
(aa)+H200) NH3(a?) H3o (ag) 17) What is the conjugate acid of HCO3? 17) A) H2CO3 B) H20
C) OH. D) H30+ E) CO32- Co32. 1) 18) What is the conjugate base of H2PO4? 18) A) PO43-
B) HPO42- COH- D) H30+ E) H3PO4 19) Which of the following acids will have the strongest
conjugate base? 19) A) HCI B) HI C) HCN D) HNO3 E) HCIO4 20 20) Which of the following
solutions would have the highest pH? Assume that they are all 0.10 M in acid at 25°C. The
acid is followed by its Ka value. A) HCN, 4.9x 10-10 B) HF, 3.5 x 10-4 C) HCHO2, 1.8 x 10-4
D) HCIO2, 1.1 x 10-2 E) HNO2, 4.6 x 10-4 2 21) Which of the following is TRUE? A) A neutral
solution contains [H2O] [H30*] B) A basic solution does not contain H30+ C) An acidic solution
has [H30*]> (OH] D) A neutral solution does not contain any H30+ or OH- E) None of the
above are true.
Solution
16) C
Reason:NH3 is a weak base. In solution form we write it as NH3(aq) the reaction is- NH3(aq)
+H2O= NH4+ + OH-
Here OH- is in product side which indicates basic nature as per Brownsted Lowri theory.
17) A
Reason: when a base accepts proton in a solution it is known as conjugate acid O-H + HCO3 2-
= H2CO3
18) B
Reason: after donation of a proton what is remaing will be conjugate base here, H2PO4- = HPO4
2- +H+
19) C](https://image.slidesharecdn.com/nnncrease16anaqueoussolutionofammoniaisfoundtonetioniceq-230206013452-463a82b0/85/n-nncrease-16-An-aqueous-solution-of-ammonia-is-found-to-net-ionic-eq-docx-1-320.jpg)
