Is NaHCO3 acidic, basic, or neutral (in water)?

To tell if NaHCO3, Sodium bicarbonate or sodium hydrogen carbonate forms an acidic, basic (alkaline), or neutral solution we can use these three simple rules along with the neutralization reaction that formed NaHCO3 . First we need to figure out the acid and base that were neutralized to form Sodium bicarbonate (sodium hydrogen carbonate). The equation for NaHCO3 is: NaOH + H2CO3 = Na2CO3 + H2O It is also useful to have memorized the common strong acids and bases to determine whether NaHCO3 acts as an acid or base in water (or if it forms a neutral solution). Strong acids: HCl, H2SO4, HNO3, HBr, HI, HClO4 Weak acids: HF, CH3COOH, H2CO3, H3PO4, HNO2, H2SO3 Strong Bases: LiOH, NaOH, KOH, Ca(OH)2, Sr(OH)2, Ba(OH)2 Weak Bases: NH3, NH4OH Note that we are talking about whether NaHCO3 is an acid, base, or neutral when dissolved in water. - Salts of strong bases and strong acids: pH will remain neutral at 7. - Salts of weak bases and strong acids: pH less than 7 (acidic). - Salts from strong bases and weak acids: pH greater than 7 (alkaline). Based on these rules, the solution of NaHCO3 dissolved in water is Basic. For polyprotic acids (e.g. H3PO4) it’s a bit more complicated and we need to use Ka and Kb to determine the pH of the resulting solution. More chemistry help at http://www.Breslyn.org.

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