Strong/Weak Acid Equilibrium Calculations PDF

Equilibrium Calculations with Strong Acids and with Weak Acids The mathematics is very, very similar to what you’ve already been shown in the previous chapter. That said, there are some new concepts that emerge that are important to understand. Consider a 0.10 M HNO3 solution (meaning somebody ad...

Equilibrium Calculations with Strong Acids and with Weak Acids The mathematics is very, very similar to what you’ve already been shown in the previous chapter. That said, there are some new concepts that emerge that are important to understand. Consider a 0.10 M HNO3 solution (meaning somebody added 0.10 mol of nitric acid for every liter of water). Calculate the equilibrium concentration of HNO3, NO3-, H3O+, and OH-. Also calculate the pH and percent dissociation of the acid. A student adds 1.00 mol of a weak acid HA to 10.0 L of water and measures a pH of 1.55. What is the value of Ka for HA? Consider a 0.10 M HOCl solution. Calculate the equilibrium concentration of HOCl, OCl-, H3O+, and OH-. Also calculate the pH and percent dissociation of the acid. The Ka of HOCl is 2.9 x 10-8. Consider a 0.0010 M HF solution. Calculate the equilibrium concentration of HF, F-, H3O+, and OH-. Also calculate the pH and percent dissociation of the acid. The Ka of HF is 3.5 x 10-4. Mixtures of acids: Consider a 1.0 L solution to which you add 0.10 mol of HF and 0.10 mol of HOCl. Use the Ka values to answer the following questions: HF(aq) + H2O (l) ↔ F-(aq) + H3O+(aq) Ka = 3.5 x 10-4. HOCl(aq) + H2O (l) ↔ OCl- (aq) + H3O+(aq) Ka = 2.9 x 10-8 Which acid will dissociate the most? Will the dissociation of the stronger acid encourage or inhibit the dissociation of the weaker acid? How would you set up the calculation to estimate the pH of the solution? Equilibrium Calculations with Acids Homework