A 5.30 mLmL sample of an H3PO4H3PO4 solution of unknown concentration is titrated with a 1.050×10−2 MNaOHMNaOH solution. A volume of 7.32 mLmL of the NaOHNaOH solution was required to reach the equivalence point. What is the concentration of the unknown H3PO4H3PO4 solution?         Express your answer with the appropriate units.   Value___?  Units____?

10. Calculate the concentration of an HCI solution if 100.0 mL of the HCI required 33.00 mL of 0.2000 M Mg(OH)2 to reach the titration endpoint. (Use stoichiometry, answer is 0.1320 M) Mg(OH)2 + 2 HCI 2 H₂O + MgCl₂

8. A student conducts an acid-base titration to investigate the change in pH during a reaction between hydrochloric acid and ammonia solution. a. Name a piece of equipment that could be used to provide an accurate measurement of pH during the titration and explain how it would be calibrated. The student transfers 50cm3 of 1.0moldm3 ammonia solution acid into a beaker. During the titration the student adds 50cm3 1.00moldm³ hydrochloric acid from a burette into the beaker and records the pH throughout. b. Sketch the pH curve produced during this titration.

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%)