Question

Determine how many grams of each of the following solutes would be needed to make 2.00x10² mL of a 0.100 M solution.

a. cesium iodide (CsI): _____g

b. sulfuric acid (H₂SO₄): ____g

c. sodium carbonate (Na₂CO₃): ______g

d. potassium dichromate (K₂Cr₂O₇): _____g

e. potassium permanganate (KMnO₄): ____g

Answer 1

we know that

moles of solute = molarity x volume (ml) / 1000

so

moles of solute = 0.1 x 200 / 1000

moles of solute = 0.02

now

we know that

mass = moles x molar mass

so

a)

CsI , molar mass = 259.81

so

mass of CsI = 0.02 x 259.81 = 5.1962 grams

so

5.1962 grams of CsI is needed

b)

H2S04

mass of H2S04 = 0.02 x 98 = 1..96 grams

c) Na2C03

mass of Na2C03 = 0.02 x 106 = 2.12 grams

d) K2Cr207

mass of K2Cr207 = 0.02 x 294 = 5.88 grams

e) KMnO4

mass of KMnO4 = 0.02 x 158 = 3.16 grams