NaHCO3 can be used to neutralize excess acid in situations such as, for instance, acid spills in the laboratory. The reaction is: H"(aq) + HCO3 (aq) → H2O(1) + CO2(3). How many grams of NaHCO3 would be required to neutralize the acid in 75.5 mL of 1.00 M nitric acid? O 75.5 grams O 7.55 grams O 6.34 grams O 1.11 grams O 0.899 grams
States of Matter
The substance that constitutes everything in the universe is known as matter. Matter comprises atoms which in turn are composed of electrons, protons, and neutrons. Different atoms combine together to give rise to molecules that act as a foundation for all kinds of substances. There are five states of matter based on their energies of attraction, namely solid, liquid, gases, plasma, and BEC (Bose-Einstein condensates).
Chemical Reactions and Equations
When a chemical species is transformed into another chemical species it is said to have undergone a chemical reaction. It consists of breaking existing bonds and forming new bonds by changing the position of electrons. These reactions are best explained using a chemical equation.
Given,
Concentration of the nitric acid (HNO3) solution = 1.00 M = 1.00 mol/L
Note: 1000 mL = 1 L
Volume of nitric acid (HNO3) solution = 75.5 mL = 0.0755 L
Mass (in grams) of NaHCO3 required to neutralize the acid = ?
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