Since you can write a balanced chemical equation, you can also utilize your stoichiometry for these neutralization reactions. You mix 1 mole of HNO3 with 1 mole of NaOH in enough water to make 1 L of solution. What do you expect the final pH of the solution to be? Hint: Think about what is in your beaker after the reaction has run to completion: . Is there any of the original acid left? Is there any of the original base left? Do you expect any of your products to act as an acid or a base? pH <7 OH > 7 DH = 7

Chemistry
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Chapter1: Chemical Foundations
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Since you can write a balanced chemical equation, you can also utilize your stoichiometry for these
neutralization reactions.
You mix 1 mole of HNO3 with 1 mole of NaOH in enough water to make 1 L of solution. What do you
expect the final pH of the solution to be?
Hint: Think about what is in your beaker after the reaction has run to completion:
• Is there any of the original acid left?
. Is there any of the original base left?
Do you expect any of your products to act as an acid or a base?
pH <7
OH > 7
pH = 7
Transcribed Image Text:Since you can write a balanced chemical equation, you can also utilize your stoichiometry for these neutralization reactions. You mix 1 mole of HNO3 with 1 mole of NaOH in enough water to make 1 L of solution. What do you expect the final pH of the solution to be? Hint: Think about what is in your beaker after the reaction has run to completion: • Is there any of the original acid left? . Is there any of the original base left? Do you expect any of your products to act as an acid or a base? pH <7 OH > 7 pH = 7
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