(a) HNO2 + H2O = NO2- + H3O+
Here, in this reaction HNO2 gives one H+ ion, so it behaves as acid and H2O accepts H+ so it behaves as base ( By Bronsten- Lowry concept).
(b) HNO2 acts as acid and NO2- will be conjugate base.
And H2O acts as base and H3O+ will be conjugate acid.
hat is the pH of a 04 a) Wri will ee which nf ononm dissori.. General...
1 a) Write the aqueous acid dissociation reactions for an acid and base dissociation reaction for a base according to the Bronsted-Lowry definition b) Determine conjugate bases of acids and acids of bases c) Write the equilibrium expression for an acid or a base aqueous dissociation d) Evaluate strength of an acid or base based on its Ka or Kb or pKa or pKb. e) Apply Kw at 25oC and at different temperatures. f) Solve for the pH of strong...
21. A solution of chromium nitrate 9 (A) nitrate ions are acid in water. (B) nitrate gives an acid reaction because nitrate ions act as a strong oxidizing agent. (C) nitrate ions react with wa o form the strong acid, nitric acid. (D)) molecules of chromium nitrate rea which is a strong acid, and insoluble chromic hydroxide. hromium ) nitrate react with water to form nitric acid, drated chromium ion tends to lose a proton from one of the (e)...
in some cases, there may be a mixture of two or more acids. When this happens, the stronger acid will dissociate completely, so you should be able to calculate how much H,0 is in solution as a result. Writing out the equation for the dissociation often helps The weak acid will attempt to dissociate and is governed by the equilibrium (K,). You should write out the equation for the weak acid Now-write in the values for the concentrations that you'll...
What is the pH of a 6.00 M H3PO4 solution? Ka1= 7.5x10^-3 Ka2= 6.2x10^-8 Ka3= 4.2x10^-13 Pearson retur Learn Ch 17: Acids and Bases QUESTION ANSWER 2.12 Weak acids and bases are those that do not completely dissociate in water. The dissociation of the acid or base is an equilibrium process and has a corresponding equilibrium constant. K is the equilibrium constant for the dissociation of a weak acid and K is the equilibrium constant for the dissociation of a...
Learn Ch 17: Acids and Bases det aptir QUESTION ANSWER miy aptiv 2.52 ats Weak acids and bases are those that do not completely dissociate in water. The dissociation of the acid or base is an equilibrium process and has a corresponding equilibrium constant. K is the equilibrium constant for the dissociation of a weak acid and K is the equilibrium constant for the dissociation of a weak bas. 6.33 ООООО 7.67 What is the pH of a 0.145 M...
wanted to know is it smaller or larger for question four? I WOU L ions for a carboxylic acid? RCOOH and RCOOR RCOOR' and R,co ester R.CO and RCOOH RCOOH and RCO,H (Carbon) Question 2 (0.5 point) Which of the following statements is true? Carboxylic acids function as proton donors. r Carboxylic acids function as proton acceptors. r Carboxylic acids can function as proton donors and proton acceptors. r Carboxylic acids cannot function as proton donors or proton acceptors. Question...
Polar molecules tend to be soluble in water. a) True b) False Which liquid is miscible with water? a) carbon tetrachloride b) ethyl alcohol c) bromine d) oil Which anion will not precipitate silver ion? a) chloride b) nitrate c) bromide d) carbonate Which pH listed below is most acidic? a) 3 d) 7 c)9 d) 14 A hydrogen ion consists of a(n) a) electron. b) proton. c) neutron. d) proton and electron. Bronsted and Lowry defined an acid as...
Q(33) A Lewis acid is? A) A proton donor. B) A proton acceptor. C) An electron pair donor. D) An electron pair acceptor. E) An anphoteric species. Q(34) A Brønsted-Lowry acid is? A) A proton donor. B) A proton acceptor. C) An electron pair donor. D) An electron pair acceptor. E) An anphoteric species. Q(35) What is the relationship between Ka and Kb for a conjugate acid base pair? A) Kw=Ka+Kb B) Kw=K.*Kb C) Kw=Ko-Kb. D) Kw=Ka/Kb. E) Kw=K? Q(36)...
Conjugate Pairs According to the Bransted-Lowry theory, an acid is any substance (molecule or ion) that can transfer a proton (H' ion) to another substance, and a base is any substance that can accept a proton Acid-base nreactions ane protor-bansfer neactions as follows Part A The following equation shows the equilibrium in an aqueous solution of ethylamine HA + BH +A CH,NH, (aq) + H,O) C,H,NH, '(aq) + OH (aq) base acid base acid Which of the following represents a...
D) An electron pair acceptor. E) An anphoteric species Q/33) A Lewis acid is? A)A proton donor B)A proton acceptor. C) An electron pair donor D) An electron pair acceptor E) An anphoteric species. Q(34) A Brønsted-Lowry acid is? A) A proton donor D) An electron pair acceptor. B)A proton acceptor. C) An electron pair donor E) An anphoteric species. Q(35) What is the relationship between Ka and Ko for a conjugate acid base pair? A) Kw=Ka+Kb B) Kw=Ka*Kb C)...