QUESTION ! Magnesium chloride (MgCl 2 ) dissolves completely in water. What is t

Question

QUESTION !

Magnesium chloride (MgCl2) dissolves completely in water. What is the molarity of the Mg2+(aq) cation in a 0.00500 M MgCl2(aq) solution? (3 significant digits, units M)

1 points   

QUESTION 2

The parts per million (ppm) unit can be expressed as mg solute per liter solution (mg/L) for dilute aqueous solutions. Convert the Mg2+(aq) concentration from Question 1 into units of ppm. Use the molar mass of the ion in the conversion. (3 significant digits, units ppm)

1 points   

QUESTION 3

What is the molarity of Cl-(aq) anion in a 0.00500 M MgCl2(aq) solution (the same solution as Question 1)? (3 significant digits, units M)

1 points   

QUESTION 4

Convert the Cl-(aq) concentration from Question 3 into units of ppm. Use the molar mass of the ion in the conversion. (3 significant digits, units ppm)

1 points   

QUESTION 5

What is the % by mass of Mg2+(aq) in the 0.00500 M MgCl2(aq) solution from Question 1?  Assume the solution density is 1.0 g/mL, like water. (3 significant digits, unit %)

1 points   

QUESTION 6

What is the molality of the Mg2+(aq) in the 0.00500 M MgCl2(aq) solution from Question 1?  Assume the solution density is 1.0 g/mL, like water. (3 significant digits, unit m)

1 points   

QUESTION 7

Stu and Noke are working with a red food coloring, Red #40. The stock solution has a concentration of 0.0880 M dye. Noke want to makes a concentration of 0.0088 M, exactly one tenth of the original red dye solution strength. What volume of the original 0.0880 M solution should she measure into a 100.0 volumetric flask, to be diluted with water up to the line of the flask? (3 significant digits, unit mL)

1 points   

QUESTION 8

Stu dilutes the stock 0.0880 M red dye solution (same as the previous question) by measuring 25.00 mL with a pipet into a 100.0 mL volumetric flask and then adding water up to the line on the flask. Calculate the new concentration of his diluted solution. (Round to 3 significant digits, unit M)

1 points   

QUESTION 9

The next three questions focus on a 26 ppm Ag+(aq) solution that Kemmi and Doc are using. First, calculate the molarity of the silver cation (Ag+) in the solution. Assume the solution density is the same as pure water. (2 significant digits, unit M)

1 points   

QUESTION 10

Kemmi dilutes the 26 ppm Ag+(aq) solution by twice pipetting 15 mL of solution into a 100 mL volumetric flask. She fills the remaining volume with water. Use M1V1 = M2V2 with M1 equal to 26 ppm. Solve for the diluted concentration (M2) in units of ppm. (2 significant digits, unit ppm)

1 points   

QUESTION 11

Doc wants to make a 10.4 ppm Ag+(aq) solution from the original 26 ppm solution. He has a 25 mL volumetric flask available. Use M1V1 = M2V2 with the M1 and M2 values in units of ppm, to predict which volumetric pipet Doc should use to make his dilution. (2 significant digits, unit mL)

Explanation / Answer

QUESTION 1)

Molarity of MgCl2 = 0.00500 M

Molarity of Mg+2 = 0.00500 M

QUESTION 2)

Molarity = 0.00500 mol / L x 24 g/mol

             = 0.120 g/L

            = 120 mg/L

molarity = 120 ppm

QUESTION 3)

Molarity of Cl- = 2 x 0.00500

Molarity of Cl- = 0.0100 M

QUESTION 4)

Molarity = 355 ppm

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