A volume of 10.0 of a 0.190 solution is titrated with 0.770. Calculate the volume of required to reach the equivalence point.

To calculate the volume of the titrant required to reach the equivalence point, we need to use the concept of molarity (M) and the equation for the reaction.

In this problem, we are given:
- Volume of the solution: 10.0 mL
- Concentration of the solution: 0.190 M
- Concentration of the titrant: 0.770 M

First, let's determine the number of moles of solute present in the original solution. We can use the formula:

moles = volume (in liters) × concentration (M)

Converting the volume from mL to L, we have:
Volume = 10.0 mL = 10.0 mL × (1 L/1000 mL) = 0.0100 L

Substituting the values into the formula, we get:
moles of solution = 0.0100 L × 0.190 M = 0.00190 moles

Next, we need to determine the stoichiometry of the reaction to find the molar ratio between the solute and the titrant. The balanced equation is needed for this step; however, it was not provided in the question.

Please provide the balanced equation for the reaction.

Once we know the balanced equation, we can find the molar ratio and use it to calculate the volume of titrant required to reach the equivalence point.