The equivalence point for the titration of a 25.00-mL sample of CsOH solution with 0.1062 M HNO3 is at 35.27 mL. What is the concentration of the CsOH solution?

A 0.396 g sample of KHPKHP will be titrated with a NaOHNaOH solution with an assumed concentration of 0.100 M. Calculate the volume of NaOH that should neutralize the KHP sample.

24.16 mL of 0.2704 M sodium hydroxide is titrated with 29.00 mL of phosphoric acid.  Calculate the molarity of phosphoric acid.

How many equivalents are in 15.0 mL of 0.12 M Ba(OH)2 solution? What volume of 0.085 M HNO3 is required to reach the end point when titrating 15.0 mL of this solution?

Calculate the concentration of all ions present in 63.8 mg NH4B1 in 500.0 mL of solution. MNH4 MBr

A solid sample of Zn1OH22 is added to 0.350 L of 0.500 Maqueous HBr. The solution that remains is still acidic. It isthen titrated with 0.500 M NaOH solution, and it takes 88.5mL of the NaOH solution to reach the equivalence point.What mass of Zn1OH22 was added to the HBr solution?

The titration of 25.0 mL of an unknown concentration HNO2 solution requires 83.6 mL of 0.12 M LIOH solution. What is the concentration of the HNO2 solution (in M)? O 0.20 M O 0.40 M 0.10 M O 0.36 M O 0.25 M

7. A 10.00-g sample of the ionic compound NaA, where A is the anion of a weak acid, was dissolved in enough water to make 100.0 mL of solution and was then titrated with 0.100 M HCl. After 500.0 mL HCl was added, the pH was 5.00. The experimenter found that 1.00 L of 0.100 M HCl was required to reach the stoichiometric point of the titration. a. What is the molar mass of NaA? b. Calculate the pH of the solution at the stoichiometric point of titration.