For the reaction of acetic add, CH_3COOH, with sodium hydroxide, NaOH, write the

Question

For the reaction of acetic add, CH_3COOH, with sodium hydroxide, NaOH, write the complete, balanced equation. Label the acid and the conjuigatye base. write the net ionic equation how many acid protons are there in a molecule of acetic acid? What does an acid-base titration accomplish? What is an indicator and how does it function in a titration experiment? By using the proper units for volume and concentration in the titration equation, show that Moles_acid = Moles_base What is the molarity of an of an unknown add if 40.5 mL of the add can be titrated to an end point by 20.5 mL of 0.2250 M NaOH? Show your work and be careful with significant figures.

Explanation / Answer

Balanced Chemical Equation:

CH3COOH (aq) + NaOH (aq) -> CH3COONa (aq) + H2O (l)

Net ionic equation:

CH3COOH (aq) + Na+ + OH- -> CH3COO- + Na+ + H2O

Cancelling out sodiums:

CH3COOH (aq) + OH- -> CH3COO- + H2O

There is only one acidic proton available, as acetic acid is a monoprotic acid.

An acid-base titration seeks to determine the concentration of an acid or base by neutralizing it with a known concentration acid or base.

An indicator's function in a titration is to indicate a change in pH. pH indicators sense the presence of H+ and OH- ions, and change color according to their concentration.

Titration equation:

Macid Vacid = Mbase Vbase

Molarity = moles/Liter

Molesacid / Litersacid * Litersacid = Molesbase / Litersbase * Litersbase

Cancelling out liters:

Molesacid = Molesbase

We use titration equation for last problem:

Macid Vacid = Mbase Vbase

Macid * 40.5mL = 0.225M * 20.5 mL

Macid = 0.1139 M

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