"Ammonium ion" is the conjugate acid of a weak base, "ammonia"; "perchlorate anion" is the conjugate base of a strong acid, HClO_4. NH4Br --> NH4 + Br - a. since Br - is the conjugate base for HBr (strong acid), therefore it is a weak base and it doesnt alter the pH of the solution. Then there would be equal amounts of OH- and H+. pH and Acidity: The pH of a solution is the measure of the hydrogen ion concentration, which will dictate its acidity or alkalinity. Bases: LiF, KCN ... To find the pH of a solution of NH4Br directly, one would need to use? The equilibrium constant for the acid-base reaction of a base in aqueous solution is called the? If you want to quickly find the word you want to search, use Ctrl + F, then type the word you want to search. higher the Kb, the stronger the base. K2CO3 = basic. This would then immediately disassociate. c. NH4Br is an acidic salt 2. KCN 5. NH4Br is Acid I'll tell you the Acid or Base list below. What I don’t understand is why this can’t happen too. NH4CN is the product of weak acid/weak base. Acids: NH4Br, NH4ClO4. I know that bases donate electrons and acids accept them, but how can you tell from this lewis structure? NH4+ + H20 —> NH4OH. I was able to draw the lewis structure for AlCl 3 but I am confused how you know if Al is a acid or base. And thus the acid base behaviour of the salt depends on the ammonium ion. base ionization constant. LiClO = basic - salt of strong base (LiOH) and weak acid … b. NH4 is the conjugate acid of NH3 (weak base) therefore it is a stronger acid, so it decreases the pH of the solution. Chem_Mod Posts: 18400 Joined: … Identify each acid or base as strong or weak. But you have to compare the Ka and Kb for these species before making a judgement! Answer to Identify the following salts as neutral acidic or basic: 1. It is the conjugate acid of a weak base (NH4+ is the conjugate acid of NH3) and the conjugate base of a weak acid (NO2- is the conjugate base of HNO2). ; Because Mg(OH) 2 is listed in Table 12.2 "Strong Acids and Bases", it is a strong base. Solution of ammonium perchlorate would be slightly acidic, and its pH governed by the equilibrium: NH_4^+ … SrBr2 3. Top. NH4Br —> NH4+ + Br-then. Br- + H20 —> HBr-HBr is a strong acid that immediately disassociates so it doesn’t matter. LiF 4. Because HCl is listed in Table 12.2 "Strong Acids and Bases", it is a strong acid. NH4ClO4 6. A solution of "ammonium perchlorate" would be slightly acidic in water. NaCN = basic. NH4Br 7. KCN a. 1. How does Kb relate to base strength? So yes, it is a weak acid (NH4+) and weak base (NO2-). LiNO3 and SrBr2 are the products of strong acid/strong base. KCl = neutral - salt of strong acid (HCl) and strong base (KOH) NH4Br = acidic. I would arrange the salts this way: Neutrals: LiNO3, SrBr2, NH4CN. The stronger the base/acid, the weaker its conjugate is, and vice-versa. Both are products of strong acid/weak base. Example 6. HCl; Mg(OH) 2 C 5 H 5 N; Solution. LiNO3 2.