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**Neutralization Reactions**

Section 21.1

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**Neutralization Reactions**

Acid + Base Water + salt Hydronium ions + hydroxide ions water + water H3O OH H2O H2O Examples: HCl + NaOH H2O + NaCl H2SO4 + 2KOH 2H2O + K2SO4 All neutralization reactions are double displacement reactions

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**Titrations Standard Solution Titration End Point**

The solution of known concentration Titration The process of a specific amount of a known solution to an unknown solution to determine the molarity of the unknown solution End Point When the indicator shows that neutralization has occurred

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**Example graph of end point**

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Sample Problem A 25mL solution of H2SO4 is completely neutralized by 18mL of 1.0 M NaOH using phenolphthalein as an indicator. What is the concentration of the H2SO4 solution? H2SO4 + 2NaOH 2H2O + Na2SO4 25mL H2SO4 1L H2SO mol H2SO4 2 mol NaOH mL = 0.36M NaOH 1000mL L H2SO mol H2SO mL NaOH L Use stoichiometry to go from mL of your known solution to find Molarity (mol/L) of your unknown solution

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PH and Titration Notes Chemistry. pH measure of the strength of acids and bases pH = power of hydrogen pH = -log [H + ] logarithmic scale – so.

PH and Titration Notes Chemistry. pH measure of the strength of acids and bases pH = power of hydrogen pH = -log [H + ] logarithmic scale – so.

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