A 50.0 mL solution of Ca(OH)₂ with an unknown concentration was titrated with 0.340 M HNO₃. To reach the endpoint, a total of 19.6 mL of HNO₃ was required. How many moles of HNO₃ are used in the titration?

#15. The sample of 30.0 mL of 0.0150 M HClO is titrated with a 10.0 mL of 0.050 M NaOH solution. (a) Show the reaction between HClO and OH–. (b) What is the final volume after two solutions were mixed? (c) What is the final molarity of OH– after the reaction with OH–?   (d) What is the pH after 10.0 mL of the NaOH solution is added?

A Ca(OH) 2 solution of unknown concentration is titrated with 0.275 M HN*O_{3} 26.19 mL of the titrant is required to titrate 25.000 mL of the Ca(OH) 2 solutionWhat is the concentration of the Ca(OH) 2 solution ?

A 25.0 mL sample of a saturated Ca(OH)2 solution is titrated with 0.029 M HCl, and the endpoint is reached after 37.2 mL of titrant are dispensed. Based on this data, what is the concentration of Ca(OH)2?

5. What is the "equivalence point" of a titration?

A titration curve is constructed by titrating 50.0 mL of 0.100 M solution of a weak acid, HA, with 0.250 M NaOH. How many millilitres of NaOH must be added to reach the equivalence point?

A solution containing 1.178 g of a triprotic acid H3A was titrated with NaOH. It required 90.00 mL of 0.1250 M NaOH to reach the third equivalence point. What is the molar mass of the triprotic acid, H3A?

In a titration of 35.0 mL of a 0.500 M solution of the diprotic acid H₂C₃H₂O₄ (malonic acid) with 0.255 M NaOH, how many moles of NaOH are required to reach the second equivalence point?

30.23 mL of a solution of the acid H2SO4 is titrated, and 47.20 mL of 0.8600-M NaOH is required to reach the equivalence point. Calculate the original concentration of the acid solution.

In a titration of 34.0 mL of a 0.250 M solution of a triprotic acid H3PO4 (phosphoric acid) with 0.800 M NaOH, how many mL of base are required to reach the third equivalence point?