Show Work for any of these
1.What is the molarity of a solution made with 25.2 g CaO in a total of 2 L of solution? Show your work, using dimensional analysis, being sure to use units throughout.

2.Calculate the molarity of the solution formed when 0.72 moles of CaBr2 is dissolved in 1.50 L water. Show your work

3.Find the molar mass of magnesium phosphate tribasic, which has a formula of Mg3(PO4)2

1. 0.224 M is the molarity of the solution made with 25.2 grams CaO in 2 litres of solution.

2. 0.48 M is the molarity of the solution formed when 0.72 moles of CaBr2 is dissolved in 1.50 L water.

3. 262.84 gm/mole is the molar mass of Mg3(PO4)2.

Explanation:

1. Data given:

weight of the mass of CaO = 25.2 grams

Atomic weight of one mole of CaO = 56.07 gram/mole

number of moles = mass÷atomic mass of one mole of the substance

                               =   25.2 ÷ 56.07

                               = 0.449 moles of CaO is used to make a solution of 2 Litres

formula for molarity:

molarity = number of moles ÷ volume in litres

               = 0.449 ÷ 2

                 = 0.224 M

2. Data given:

number of moles of CaBr2 = 0.72 moles

volume of the water used = 1.50 L

Formula of molarity:

molarity = number of moles ÷ volume in litres

molarity = 0.72 ÷ 1.5

               = 0.48 M

3. Molar mass of a compound is calculated by adding the number of moles of elements taking part in the formation of the compound.

Mg = 24.30 gm/mole

P = 30.97 gm/mole

O = 16 gm/mole

3 moles of Mg ( 24.3 x 3) + 2 moles of P (2 x 30.97) + 8 moles of O (8 x 16)

= 262.84 gm/mole is the atomic weight of Mg3(PO4)2

plasma is the state of matter where the substance is ionized and has no definite shape or volume. the fact of being ionized makes the substance a good electrical conductor.