Question

A volume of 20.0mL of a 0.590M HNO3 solution is titrated with 0.900M KOH. Calculate the volume of KOH required to reach the equivalence point.

Answer 1

Answer on Question#39836 - Chemistry - Other

Question:

A volume of 20.0 mL of a 0.590 M HNO₃ solution is titrated with 0.900 M KOH. Calculate the volume of KOH required to reach the equivalence point.

Solution:

$$\mathrm{C_1V_1 = C_2V_2}$$ $$20 \text{ ml} * 0.590\text{M} = 0.900\text{M} * \mathrm{V_2}$$ $$\mathrm{V_2} = (20 \text{ ml} * 0.590\text{M}) / 0.900\text{M} = 13,11 \text{ ml}$$

Answer: 13.11 ml