Consider the titration of 25.0 mL of 0.118 M acetic acid (CH, COOH. pK, 4.75) with 0.100 M NaOH. CH, COOH(aq) + NaOH(aq) CH,coO (aq) + H,O0) + Na (aq) Determine the initial pH of the 0.118 M acetic acid solution before NaOH is added. pH Determine the pH of the solution after 10.0 mlL of 0.100 M NaOH is added. pH Determine the volume of 0.100 M NaOH required to reach halfway to the stoichiometric point of the titration. volume NaOH:

A volume of 500.0 mL of 0.170 M NaOH is added to 535 mL of 0.250 M weak acid (?a=3.06×10−5). What is the pH of the resulting buffer?   HA(aq)+OH−(aq)⟶H2O(l)+A−(aq)   pH=

(a) Lactic acid, (CH3CH(OH)COOH) is a common biomolecule which can accumulate in muscles during intense exercise. A chemist prepares a buffer using 225 mL of 85 M lactic acid (Ka = 1.38 x 10-4) and 435 mL of 0.68 M sodium lactate. What is the pH of the buffer?             What is the pH of the lactate buffer if 0.25 moles of gaseous HCl is added?

A student prepares a solution for titration by adding a 10.00 mL aliquot of a solution saturated with Ca(OH)2 at 82.9°C to 25.0 mL of deionized water.  This solution is titrated with a standardized 0.01252 M HCl solution.  The equivalence point is observed after 17.94 mL of the HCl solution has been added. Calculate the moles and molarity of OH-  and Ca2+  in the 10.00ml sample.

Calculate the pH for each case in the titration of 50.0 mL of 0.110 M HClO(aq)0.110 M HClO(aq) with 0.110 M KOH(aq).0.110 M KOH(aq). pka = 7.40 ka= 4.0*10^-8 What is the pH after addition of 50.0 mL KOH? What is the pH after addition of 60.0 mL KOH?

Calculate the pH for each case in the titration of 50.0 mL of 0.230 M HClO(aq) with 0.230 M KOH(aq). Use the ionization constant for HCIO. What is the pH before addition of any KOH? pH What is the pH after addition of 25.0 mL KOH? pH = What is the pH after addition of 30.0 mL KOH? = pH = pH = What is the pH after addition of 50.0 mL KOH? pH What is the pH after addition of 60.0 mL KOH?

In some natural systems the pH must be maintained within very narrow limits. e.g. in human blood the pH must remain close to 7.4 or cell deterioration occurs. Blood contains several weak acid/conjugate base equilibria called buffers, which control the pH.One weak acid present in blood is the dihydrogen phosphate ion, H2PO4-(aq), for which the equilibrium in aqueous solution is H2PO4-(aq) +H2O(l) <--> HPO42-(aq) + H3O+(aq). a) What would be the effect on this equillibrium of adding hydrochloric acid solution?b) Write the expression for the equilibrium constant of this reaction.c) If 0.5 mol H2PO4- and 0.5 mol HPO42- are in equilibrium in 1.0L of aqueous solution, calculate the pH of the solution. (Ka for H2PO4-= 6.4 x 10-8)d) 0.010 mol HCl is now added to the 1.0L of the solution in c). Assuming that all the added H+ ions are used up in the equilibrium shift, calculate the concentrations of H2PO4- and HPO42-. Hence calcuate the pH of this solution.e) 0.010 mol HCl has been added…