please complete all questions

6. Barium hydroxide reacts with hydrochloric acid to produce barium chloride and water. How many grams of barium hydroxide are required for complete reaction with 15.0mL of 0.105M hydrochloric acid? The molar mass of barium hydroxide is 171.342g/mol. (Hint: start by writing the balanced equation for the reaction.) 7. A sample contains an unknown amount of citric acid, H3C6H5O7. If 0.6667g of the sample requires 35.09mL of 0.1000MNaOH to neutralize the H3C6H5O7 completely, what is the percentage of H3C6H5O7 in the sample? The molar mass of H3C6H5O7 is 192.13g/mol. The balanced equation for the reaction is: H3C6H5O7+3NaOH3H2O+Na3C6H5O7 8. Sodium thiosulfate, Na2S2O3, is an important reagent for titrations. Its solutions can be standardized by titrating the iodine released when a weighed amount of potassium hydrogen iodate, KH(IO3)2(389.912 g/mol), is allowed to react with excess potassium iodide in acidic solutions. The net ionic equations are: production of iodine from KH(IO3)2:IO3+5I+6H+3I2+3H2O titration of iodine: I2+2S2O3222I+S4O62 What is the molarity of a sodium thiosulfate solution if 32.96mL are required to titrate the iodine released from 0.1278g of KH(IO3)2 ? 9. You have 0.3563g of an unknown monoprotic acid, HA, which reacts with NaOH according to the balanced equation HA+NaOHNaA+H2O If 49.50mL of 0.0946MNaOH is required to titrate the acid to the equivalence point, what is the molar mass of the acid