The concentration of copper(ii) sulfate in one brand of soluble plant fertilizer is 0.07% by mass. if a 20 g sample of this fertilizer is dissolved in 2.0 l of solution, what is the molarity of cu2+?

The molarity of ions in the given amount of sample is

Explanation:

We are given:

Mass of sample = 20 g

0.07 % (m/m) of copper (II) sulfate in plant fertilizer

This means that, in 100 g of plant fertilizer, 0.07 g of copper (II) sulfate is present

So, in 20 g of plant fertilizer, = of copper (II) sulfate is present.

To calculate the molarity of solution, we use the equation:

We are given:

Mass of solute (copper (II) sulfate) = 0.014 g

Molar mass of copper (II) sulfate = 159.6 g/mol

Volume of solution = 2.0 L

Putting values in above equation, we get:

The chemical equation for the ionization of copper (II) sulfate follows:

1 mole of copper (II) sulfate produces 1 mole of copper (II) ions and sulfate ions

Molarity of copper (II) ions =

Hence, the molarity of ions in the given amount of sample is

here is table 2-2:

country

percent of eligible voters that voted

rank

united states

44.9%

138

canada

60.1%

107

costa rica

84.6%

14

hungary

66.9%

82

japan

57.0%

118

egypt

27.7%

159

south africa

85.5%

10

ans is no, the data set cannot be plotted as a single circle graph

i believe the answer is 5,000