Question

QUESTION 11 In a titration of 0.6754 grams of X (dissolved in water), how many milliliters of 1,088 MY solution are required to reach the end-point. The molar mass of X is 90.03 g/mol. You will probably find liters (L.) so be sure to convert to ministers (ml) for your final answer. Do not type the units with your answer just the number Balanced Chemical Equation: X + 2Y -->W+2Z

Answer 1

Answer and Explanation:

To determine the volume of a 1.088 M solution of Y required to reach the end-point when titrating 0.6754 grams of X, we need to use the balanced chemical equation and the molar masses of X and Y. Here are the steps to calculate the volume:

1. Calculate the number of moles of X:

- Divide the mass of X (0.6754 grams) by its molar mass (90.03 g/mol) to obtain the number of moles.

2. Use the mole ratio from the balanced chemical equation:

- According to the balanced equation, 1 mole of X reacts with 2 moles of Y.

- Multiply the moles of X by the ratio 2:1 to determine the moles of Y required.

3. Calculate the volume of the Y solution:

- Use the molarity of the Y solution (1.088 M) to determine the moles of Y required.

- Divide the moles of Y by the molarity to obtain the volume in liters (L).

- Convert the volume from liters to milliliters (ml) by multiplying by 1000.

Please perform the necessary calculations using the given data and formulas to obtain the final answer.