5) a neutral compound. 1) H2AsO3, H2AsO4 2) HClO, HClO3 3) H2S, HCl 4) H2SO3 , H2SO4 5) HI, HBr Question 4 Which of the following acids has the lowest pH? 17) A) C2H4O2 B) NaCl C) KOH D) H2O2 E) H2SO4. Identify the conjugate acid/base pairs in a Brønsted-Lowry acid/base equation. 3) a strong acid. TRUE. Conjugate Acid-Base Pairs: The Bronsted-Lowry definition describes an acid as a proton donor and a base a a proton acceptor. 0.1 M HBO, pKa = 2.43 0.1 M HA, pKa = 4.55 0.1 M … Identify the acid, the base, ... Conjugate bases and conjugate acids, respectively, are formed from these reactants and, consequently, the formulas of these generated substances must be written on the product side of the reaction arrow in an equation. conjugate base: HO2-, formed by releasing a proton g. HS-: conjugate acid: H2S, formed by accepting a proton 4) a weak acid. Let's focus on the first example, #CH_3COOH#.It behaves as an acid because it donates a proton and becomes #CH_3COO^-#. I- Dilution of a commercial hydrochloric acid solution A bottle of a commercial hydrochloric acid solution is available. We have, among others, the Conjugate Acid-Base Pairs Ordered by Strength Acids Bases [strong] [weak] HClO 4 ClO 4 – H 2SO 4 HSO 4 – HCl Cl– HNO 3 NO 3 – H 3O + H 2O H 2C 2O 4 (oxalic acid) HC 2O 4 – [H 2SO 3] = SO 2(aq) + H 2O HSO 3 – HSO 4 – SO 4 2– HNO 2 NO 2 Question 3 Which of the following pairs has the stronger acid listed first? The products of a neutralization reaction ... One example of an Arrhenius base is _____. HCl transfers a proton (H+ ion) to H 2 PO 4- and form Cl - and H 3 PO 4, now Cl - can accept a proton donated by H 3 PO 4 .so the above equation is; Practice Exam 2.docx - Practice Exam 2 1 Which one of the following is a conjugate acid-base pair a NaF and Fb NH4 and NH3c HNO3 and HNO2 d H2O and H2O2 2) a weak base. Here's are two examples of conjugate acid-base pair. NH4 + and NH3 are considered a conjugate acid-base conjugate pair. C. The name given to an aqueous solution of HBr is _____. FALSE. conjugate base: SO42-, formed by releasing a proton f. H2O2: conjugate acid: H3O2+, formed by accepting a proton. conjugate base: NH2-, formed by releasing a proton e. HSO4-: conjugate acid: H2SO4-, formed by accepting a proton. here H2CO3 and HCO3- are conjugate acid-base pair as are H2O and OH-b) HCl + H 2 PO 4-<-----> Cl - + H 3 PO 4. The substance (CH3CH2)2NH is considered 1) a strong base. H2SO3 and H2SO4 are considered a conjugate acid-base pair. - Ammonia gas is very soluble in water. The concept of conjugate acid-base pair is related to Bronsted-Lowry acid-base theory and according to this theory, acid is a proton #(H^+)# donor while base is a proton acceptor. Conjugate acid/base pair H 3 O +/H 2 O NH 4 /NH 3 H 2 O/HO – pK a 0 9.2 14 - Molar volume of a gas under the experimental conditions is V m = 24 L.mol-1.