By Bronsted definition of acid and base we know
i) A molecule which donates proton (H+) is termed as acid.
ii)A molecule which receives proton is termed as base.
So by that definition in 1st reaction H2SO4 is acid. 2nd reaction NH3 is treated as base . 3rd reaction H2O behaves as base.
5. Kw ionic product of water is defined as Kw = [H3O+] * c [ ] brackets defining concentrations
Kw at room temperature 10-14 and in this case [H3O+] = 10-8
So OH- concentration 10-6 M
According to the following reaction, which molecule is acting as an acid? H2O + H2SO4 →...
Please help Is H2PO4- + H2O → H3O+ + HPO42- an acid or base? Is H2O(ℓ) + NH3(aq) -> NH4+ + OH- an acid or base Is HSO4- + H2O → OH- + H2SO4 an acid or base Is O2- + H2O → OH- + OH- an acid or base Is H3O+ + Cl- → H2O + HCl an acid or base
I need help with number 3 and 4. 3. Which of the following is not true for the dissociation of a strong acid? . Ka is large B. The conjugate base will be weak C. [H+]> [HA] D. The equilibrium lies far to the right E. The equilibrium lies far to the left 4. What are the conjugate bases in the following reaction? H2SO4 + H2O I HSO4 +H30* A. H2SO4 and H30+ B. H2O and HSO4 C. HSO4 and...
Which of the following are conjugate acid-base pairs? (i) H3O+/H2O (ii) NH4+/NH3 (iii) H2SO4/HSO4- (iv) H2PO4-/HPO43- Select one: a. (i)(ii) (iii) b. They all are c. (ii) and (iv) d. (i) (iv)
1) Identify the Brønsted-Lowry acid and base in the following reaction HF + H2O F-+H30+ Brønsted-Lowry acid is Brønsted-Lowry base is HSO4- + H2O H2SO4 + OH Brønsted-Lowry acid is Brønsted-Lowry base is
Write equations for the reaction of each of the following Brønsted-Lowry acids and bases. Identify the conjugated acids and bases. a. Acid: H20; base: NH3 b. Acid: NH4+, base: OH- c. Acid: HSO4; base: H2O d. Acid: HCl; base: H2PO4 6.4
INH 4. Which of the following is not a conjugate acid/base pair? A) HCIO/CIO- B) H2SO4/HSO4 C) NH4+/NH3 E) all of these are conjugate acid base pairs D) H2O The poH of a 0,010 M aqueous solution of Ca(OH)2 is A) 11.70 B) 12.00 C) 12.30 D) 12.60E ) 1.70
1. Identify the acid, base, conjugate acid and conjugate base in the following reaction: HPO42+ H20 OH H2PO4 2. Calculate the following a) pH of a [H30*] = 2.76 x 104 M b) pH of a [OH] - 8.5 x 10-6 M c) [H30*] and [OH] for a soln pH 5.73 3. Show how an incoming acid [H30*] is neutralized by the buffer system HCO3 /CO32 system. You should also be able to show the neutralization of incoming base [OH']...
5. In the following reactions, identify the conjugate acid-base pairs. H2SO4 (aq) + H2O(1) → H30+ (aq) + HS0ǐ (aq) 1st pair: CH-NH2(aq) + H20(f) CH3NH扎aq) + OH-(aq) 1st pair: HF(aq) + NH3(aq) 근 NH (aq) + F-(aq) 1t pair: a. 2nd pair: 2nd pair: 2nd pair:
1. Which of the followi ch of the following reactions is not readily explained by the Arrhenius concept of acids and bases? a. A. HCl(aq) + NaOH(aq) - NaCl(aq) + H20() b. H30(aq) + OH-(aq) + 2H20(1) c. HCI(g) + NH3(g) - NH4Cl(s) d. HC2H302(aq) + H2O(l) H30*(aq) + C2H302-(ag) e. H30 (aq) + OH-(aq) + 2H2O(aq) 2. Classify each of the following species as Brønsted acid or base or both: a) H20, b) OH", c) H30, d) NH3, e)...
4. Consider the reaction: 2 SO2(g) + O2(g) 3 2 SO:(g) A 2.0 L flask was filled with 0.0400 moles of SO, and 0.0200 moles of O2. At equilibrium 0.0296 moles of SO, were found. What is the equilibrium constant for this reaction? A) 2.556 x 10 B) 3.664 x 10 C) 6.953 x 102 D) 9.964 x 102 E) 3.116 x 10 5. What is a conjugate acid-base pair for the following equilibrium? H2O(l) + HSO4 (aq) = H2SO4(aq)...