A solution is made by mixing 5.00 × 102 mL of 0.167 M NaOH with 5.00 × 102 mL of 0.100 M CH3COOH. Calculate the equilibrium concentrations of H+, CH3COOH, CH3COO−, OH−, and Na+.
NaOH + HOOCCH3 ==> NaOOCCH3 + H2O
millimols CH3COOH = mL x M = ?
millimols NaOH = mL x M = ?
Can you take it from here. If not please explain in detail what you don't undrstand.
Yes I can thank you so much Dr. Bob! I got an answer of 8.38 as a pH which seems to be right. Thanks again!
To calculate the equilibrium concentrations of H+, CH3COOH, CH3COO-, OH-, and Na+, we need to make use of the concepts of stoichiometry and equilibrium calculations.
1. Start by writing the balanced chemical equation for the reaction between NaOH and CH3COOH:
CH3COOH + NaOH -> CH3COO- + H2O
2. Determine the number of moles of NaOH and CH3COOH present in the solution by using the equation:
moles = volume (in liters) × concentration (in moles per liter)
For NaOH:
moles of NaOH = 5.00 × 10^2 mL × (1 L/1000 mL) × 0.167 M
For CH3COOH:
moles of CH3COOH = 5.00 × 10^2 mL × (1 L/1000 mL) × 0.100 M
3. Use the stoichiometry of the balanced equation to determine the number of moles of CH3COO-, H+, and OH- produced. In the balanced equation, the stoichiometric ratio between NaOH and CH3COOH is 1:1, so the moles of NaOH used will be equal to the moles of CH3COOH reacted.
4. Calculate the moles of CH3COO- and H+ produced. Since one mole of CH3COOH produces one mole of CH3COO- and one mole of H+, the moles of CH3COO- and H+ will be equal to the moles of NaOH used.
5. Calculate the moles of OH- produced. Since NaOH is a strong base that completely dissociates in water, the concentration of OH- will be equal to the concentration of NaOH used.
6. Determine the equilibrium concentrations of H+, CH3COOH, CH3COO-, OH-, and Na+ in the final solution. Since we have equal moles of CH3COO- and H+, the equilibrium concentrations of CH3COOH and CH3COO- will be the same. The concentrations of OH- and Na+ will be equal to the concentrations initially used, and the concentration of H+ will depend on the autoionization of water.
I hope this step-by-step explanation helps you calculate the equilibrium concentrations of the given ions in the solution.