A volume of 60.0 mL of a 0.510 M HNO3 solution is titrated with 0.510 M KOH. Calculate the volume of KOH required to reach the equivalence point. Express your answer to three significant figures, and include the appropriate units.

You measure 0.210 gram of unknown diprotic acid into a beaker. You add distilled water and a chemical indicator.  You slowly add titrant 0.100M NaOH acid solution. Your first equivalence point is reached after 15mL NaOH has been added. The second equivalence point is reached after 30.0mL.  WHat is the molar mass of the unkown diprotic acid?

Calculating the pH at equivalence of a titration A chemist titrates 170.0 mL of a 0.2614M cyanic acid (HCNO) solution with 0.7980M NaOH solution at 25 °C. Calculate the pH at equivalence. The p K, of cyanic acid is 3.46. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of NAOH solution added. pH =

In a titration of 18.0 mL of a 0.425 M solution of a diprotic acid H₂C₄H₄O₆ (tartaric acid) with 0.155 M LiOH, how many mL of base are required to reach the first equivalence point?

120. A diprotic acid with a molar mass of 118.04 g/mol was titrated with 1.023 M NaOH. The equivalence point of the titration occurred at 22.16 mL. Calculate the mass of the acid.

A solution of an unknown weak base (0.495 g in 100 mL of water) was prepared and titrated with standardized 0.113 M HCÌi and the pH of the solution was plotted as a function of titrant added (shown below). Titration of a Weak Base With 0.113 M HCI 12 10 10 20 30 40 50 60 70 80 90 Volume of HCl added (ml) Possible identities for the three liquid bases are shown in the table below. Base pyrole pyrimidine pyridine triethylamine 2.51 x 10-14 1.25 x 10-13 1.70 x 10-9 5.30 x 104 Density (g/mL) 0.967 1.02 0.982 0.762 Based on the data above, identify the weak base and explain your selection. The best explanations will account for all relevant experimental data. Additionally, suggest an indicator to use for this titration if it were to be done without a pH meter. Hd

NH3 + H3O+ →> NH; + H2O 25.0 mL of the 0.0220 M NH3 was titrated with 0.010 M HBr. It took 55.0 mL of HBr to reach the equivalence point. Determine the pH of the solution when 27.5 mL of 0.010 M HBr are added. Assume the temperature is constant and the volumes are additive. K₂NH3 = 1.85 x 10-5 pH = [?] pH Enter

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.

3. A 0.3535 g sample of KHP requires 19.27 mL of NaOH to reach the end point. What is the concentration of NaOH? 4. What properties should the indicator have for titration of KHP with NaOH?

What volume of 0.155 MNaOH is required to reach the equivalence point in the titration of 30.0 mL of 0.105 M HNO3?