In order to adjust the AgNO3 solution prepared as 0.1M, 25 ml of the standard NaCl solution with a concentration of 0.1025M is taken and necessary procedures are carried out. Since 24.3 ml AgNO3 solution is used for the titration, what is the concentration of AgNO3 solution?

2. Using the procedure described in this module, a student determined the percent KHP in an impure sample of KHP. A 3.150-g sample of impure KHP required 41.50 mL of 0.1352M NaOH solution for titration. (a) Calculate the number of moles of NaOH required for the titration. (b) Calculate the number of moles of KHP present in the impure sample of KHP. (c) Calculate the number of grams of KHP present in the impure sample. (d) Calculate the percent of KHP in the impure sample, using Equation 8. Equation 8: percent KHP in the impure sample, % = ( mass of KHP in the sample,g/ mass of sample analyzed, g) (100%)

Determine the molarity of a 7.00 ml HCl solution if it takes 48.35 mL of a0.1315M NaOH solution to neutralize in a titration. HCl+NaOH-->NaCl +H2O

A 0.345 gram sample of potassium hydrogen phthalate is titrated to equivalence point with 18.15 mL of NaOH. Determine the molarity of the NaOH solution.

25.00 mL of an unknown acidic solution is titrated with 0.198 M NaOH solution. Exactly 22.34 mL of the NaOH solution is needed to reach the equivalence point. What is the concentration of the unknown solution?

A 42.5ml sample  of a 0.500 M aqueous hydrocynic acid solution  is  titrated  with  a 0.397 M aqueous sodium  hydroxide solution.  What is the  ph after 23.0 ml of base have been added

You are given a package of chemical material to make an identification. The only known information of this package is that it is a monoprotic acid. You dissolved 1.0 g of the acid into 100 mL of water and titrated it with 0.1 M NaOH solution. The equivalence point was found after titrating 118.4 mL NAOH solution. What is this unknown acid?