Question

A chemist adds 35.o ml of 8.60*10^-5 m silver (ii) oxide solution to a reaction flask. calculate the micromoles of silver (ii) oxide the chemist has to add to the flask.

Answer 1

To find the micromoles of silver (II) oxide required, convert the volume of solution to liters, multiply by the molarity to get moles, and then convert to micromoles. The chemist needs to add 3.01 micromoles to the flask.

Step-by-step explanation:

To calculate the micromoles of silver (II) oxide that the chemist has to add to the flask, we first need to convert the volume of the solution from milliliters to liters, since molarity is defined as moles per liter. Here's the calculation:

Volume of silver (II) oxide solution in liters = 35.0 mL × (1 L / 1000 mL) = 0.035 L

Next, we multiply the volume of the solution by the molarity to find the moles of silver (II) oxide:

Number of moles of silver (II) oxide = 0.035 L × 8.60 × 10^-5 M = 3.01 × 10^-6 mol

To convert moles to micromoles, we use the fact that 1 mole = 10^6 micromoles:

Micromoles of silver (II) oxide = 3.01 × 10^-6 mol × 10^6 μmol/mol = 3.01 μmol

Therefore, the chemist needs to add 3.01 micromoles of silver (II) oxide to the reaction flask.