A 0.124 M NaOH(aq) solution was used to titrate 20.00 mL of an acetic acid (CH3COOH) solution that has an unknown concentration. The equivalence point is reached after adding 15.34 mL of NaOH(aq). a) Write out the complete balanced equation for the reaction that occurs in this titration. b) How man moles of NaOH were added to the acetic acid solution? c) How many moles of acetic acid were in the original 20.00 mL solution? d) What was the concentration of acetic acid in the orignial 20.00 mL solution?

A 25.00 mL sample of acetic acid (CH3COOH) is titrated to the equivalence using 31.08 mL of 0.1978 M NaOH. What is the balanced neutralization chemical reaction? What is the molarity of the acetic acid in the original sample?

A 0.5504-g sample of KHP (potassium hydrogen phthalate, KHC8H4O4; molar mass = 204.22 g/mol) is completely dissolved in enough deionized water to make 50.00 mL of solution. The resulting solution is titrated with a NaOH solution of unknown concentration. If 21.50 mL of the base solution is needed to reach the end-point, what is the molar concentration of NaOH solution? The reaction occurs as follows:                 NaOH(aq)  +  KHC8H4O4(aq)  -->  NaKC8H4O4(aq)  +  H2O(l)               (A) 0.2457 M           (B) 0.1254 M           (C) 0.05390 M           (D) 0.03823 M

A student prepares a dilute solution of sodium hydroxide, NaOH (aq), starting with 6 M sodium hydroxide. She then titrates a 1.372 g sample of KHP with the dilute sodium hydroxide solution, NaOH (aq), to a phenolphthalein end point.   A.) If the titration required 21.84 mL of sodium hydroxide, NaOH (aq), calculate the molar concentration of the sodium hydroxide solution, NaOH (aq). (Remember that KHP is potassium hydrogen phthalate, KHC8H4O4, NOT potassium hydrogen phosphorus!)   B.) The student uses the same sodium hydroxide to titrate 10.00 mL of vinegar to a phenolphthalein end point. If the titration required 27.48 mL of sodium hydroxide, NaOH (aq), calculate the molar concentration of acetic acid, HC2H3O2 (aq), in the vinegar.   C.) Calculate the mass percent of acetic acid, HC2H3O2 (aq), in the vinegar using the molar concentration for acetic acid, HC2H3O2 (aq), determined in part b and assuming the density of the solution is 1.01 g/mL.