Answer:
moles, liter, concentration, and 6.0 mol/L
Explanation:
Empirical formula is the simplest ratio of whole numbers of components in a compound
in 100 g of compound
C H O
mass 25.5 g 6.40 g 68.1 g
number of moles 25.5 g/12 g/mol 6.40 g/ 1 g/mol 68.1 g/ 16 g/mol
= 2.13 mol = 6.40 mol = 4.26 mol
divide by least number of moles
2.13/2.13 = 1 6.40/2.13 = 3.0 4.26/2.13 = 2.0
all rounded off
C - 1
H - 3
O - 2
empirical formula - CH₃O₂
<u>Answer:</u> The concentration of sulfate ions in the solution is 0.0522 M
<u>Explanation:</u>
To calculate the the molarity of solution:, we use the equation:

Given mass of alum = 2.17 g
Molar mass of alum = 478.39 g/mol
Volume of solution = 175 mL
Putting values in above equation, we get:

The chemical equation for the ionization of alum follows:

1 mole of alum produces 1 mole of potassium ions, 1 mole of aluminium ions, 2 moles of sulfate ions and 12 moles of water
So, concentration of sulfate ions = 
Hence, the concentration of sulfate ions in the solution is 0.0522 M
At <span>standard temperature
and pressure, these elements have
very similar properties; they are all shiny, silvery-white, semi-reactive metals that have industrial and biological applications. The
Alkaline Earth Metals are elements of group 2 of the periodic table, which
includes beryllium, magnesium, calcium, strontium, barium, and radium.
Moreover, group 2 elements are nonmetallic
substances that are insoluble in water and heat resistant in nature.</span>