pH of each aqueous solution:

Calculate the molarity of an aqueous nitric acid solution if it requires 35.6 mL of 0.165 M NaOH (aq) to neutralize 25.0 mL of the HNO3 (aq) solution.

A solution is prepared by dissolving 10.0g HCO2H and 5.00g NaOH in enough water to make 250.0 mL of solution. What is the pH of the solution?

Calculate the pH of an aqueous solution of 0.1930 M sodium carbonate. pH =

The pH of a 1.00 M NaCH3COO (aq) solution is 9.38. a/ Determine the concentration of [OH-] in the solution.  b/ Write the expression for the Kb of NaCH3COO (aq) and calculate its values.  c/ Calculate the pKa of CH3COOH. d/ HCl (aq) is added to 1.00 L solution of 1.00 M NaCH3COO (aq). Write the chemical reaction between HCl (aq) and NaCH3COO (aq).  e/ How many mol of HCl (aq) is needed to make a buffer solution with pH = 5.00 from 1.00 L of 1.00 M NaCH3COO (aq).

Calculate the pH and concentrations of CH3NH2 and CH3NH+3 in a 0.0395 M methylamine (CH3NH2) solution. The ?b of CH3NH2 is 4.47×10−4.

Define and give an example of (a) A weak acid, (b) A weak base

A solution is prepared by dissolving 15.0 g of pure HC2H3O2 and 25.0 g of NaC2H3O2 in 775 mL of solution (the final volume). (a) What is the pH of the solution? i (b) What would the pH of the solution be if 25.0 mL of 0.250 M NaOH were added? i (c) What would the pH be if 25.0 mL of 0.40 M HCI were added to the original 775 mL of buffer solution?