Sodium carbonate, Na2CO3, is commonly used to neutralize acid spills in the laboratory. The neutralization of nitric acid is described by the UNBALANCED chemical equation HNO3 + Na2CO3 ➜ CO2 (g) + H2O + NaNO3 How much Na2CO3 (molar mass: 105.99 g/mol) is required to neutralize 1.50 × 102 g of spilled nitric acid (molar mass: 63.01 g/mol)? a.252 g Na2CO3 b.126 g Na2CO3 c.505 g Na2CO3 d.150 g Na2CO3
Sodium carbonate, Na2CO3, is commonly used to neutralize acid spills in the laboratory. The neutralization of nitric acid is described by the UNBALANCED chemical equation HNO3 + Na2CO3 ➜ CO2 (g) + H2O + NaNO3 How much Na2CO3 (molar mass: 105.99 g/mol) is required to neutralize 1.50 × 102 g of spilled nitric acid (molar mass: 63.01 g/mol)? a.252 g Na2CO3 b.126 g Na2CO3 c.505 g Na2CO3 d.150 g Na2CO3
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter4: Stoichiometry: Quantitative Information About Chemical Reactions
Section: Chapter Questions
Problem 4PS: The balanced equation for the reduction of iron ore to the metal using CO is Fe2O3(s) + 3 CO(g) 2...
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Sodium carbonate, Na2CO3, is commonly used to neutralize acid spills in the laboratory. The neutralization of nitric acid is described by the UNBALANCED chemical equation
HNO3 + Na2CO3 ➜ CO2 (g) + H2O + NaNO3
How much Na2CO3 (molar mass: 105.99 g/mol) is required to neutralize 1.50 × 102 g of spilled nitric acid (molar mass: 63.01 g/mol)?
a.252 g Na2CO3
b.126 g Na2CO3
c.505 g Na2CO3
d.150 g Na2CO3
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