How many moles of Ag+ ions are present in 10 ml of a 0.75 M AgNO3 solution? a. 9.1 x 10^-3
b. 7.5 x 10^-3
c. 2.0 x 10^-2
d. 2.75 x 10^-2
e. 1.75 x 10^-2

b. 7.5 x 10^-3

Explanation:

To solve this problem we need to keep in mind the definition of molarity:

Molarity = moles of solute / liters of solution

With the above information in mind it is possible to calculate the moles of solute, given the volume (10 mL) and concentration (0.75 M) of the solution:

First we convert 10 mL to L ⇒ 10 mL / 1000 = 0.01 L

Then we calculate the moles of AgNO₃:

moles of solute = Molarity * Liters of solution0.01 L * 0.75 M = 7.5x10⁻³ mol AgNO₃

One mole of AgNO₃ contains one mole of Ag⁺, thus the number of Ag⁺ moles is also 7.5x10⁻³.

The correct answer is "atomic weight".

Aseasonal prevailing wind in the region of south and southeast asia, blowing from the southwest between may and september and bringing rain (the wet monsoon ), or from the northeast between october and april (the dry monsoon ).