React nitric acid (HNO3) with barium carbonate (BaCO3), and you’ll observe a vigorous reaction. This is because barium carbonate is a base, readily reacting with the strong acid, nitric acid.
The reaction produces barium nitrate (Ba(NO3)2), water (H2O), and carbon dioxide (CO2). The carbon dioxide is released as a gas, easily observed as effervescence. The barium nitrate remains in solution. The balanced chemical equation is: 2HNO3(aq) + BaCO3(s) → Ba(NO3)2(aq) + H2O(l) + CO2(g).
Safety precautions are paramount. Nitric acid is corrosive; wear appropriate personal protective equipment (PPE), including gloves, eye protection, and a lab coat. Conduct the reaction in a well-ventilated area to avoid inhaling the released carbon dioxide.
To observe the reaction clearly, use approximately 1M nitric acid and a small amount of barium carbonate powder. Add the acid slowly to the carbonate, stirring gently. The reaction is exothermic, meaning it produces heat. Monitor the temperature to ensure it doesn’t become excessive.
After the reaction, you can recover the barium nitrate by evaporating the water carefully. This process requires heating at a controlled temperature to prevent decomposition of the barium nitrate. Remember, barium compounds are toxic; handle the resulting barium nitrate with care and dispose of it properly following your institution’s safety guidelines.
This reaction demonstrates a classic acid-base neutralization. The resulting salt, barium nitrate, is a soluble ionic compound with several applications, including pyrotechnics and the production of other barium salts.
