Determine the concentrations of K2SO4, K , and SO42– in a solution prepared by dissolving 2.20...

Determine the concentrations of K2SO4, K , and SO42– in a solution prepared by dissolving 2.20 × 10–4 g K2SO4 in 1.50 L of water. Express all three concentrations in molarity. Additionally, express the concentrations of the ionic species in parts per thousand (ppt). Note: Determine the formal concentration of SO42–. Ignore any reactions with water.

K2SO4 = __ M?

K+ = __ M ? --> ppt?

SO4^2- = __ M? --> ppt?

Expert Solution

i hope it will help final answer is at the end of answer please comment for further questions please rate positively

queen_honey_blossom answered 2 years ago

Determine the concentrations of K2SO4, K , and SO42– in a solution prepared by dissolving 2.72...

Determine the concentrations of K2SO4, K , and SO42– in a solution prepared by dissolving 2.72 × 10–4 g K2SO4 in 1.00 L of water. Express all three concentrations in molarity. Additionally, express the concentrations of the ionic species in parts per million (ppm). Note: Determine the formal concentration of SO42–. Ignore any reactions with water.

Determine the concentrations of Na2CO3, Na , and CO32– in a solution prepared by dissolving 2.61...

Determine the concentrations of Na2CO3, Na , and CO32– in a solution prepared by dissolving 2.61 × 10–4 g Na2CO3 in 2.25 L of water. Express all three concentrations in molarity. Additionally, express the concentrations of the ionic species in parts per million (ppm). Note: Determine the formal concentration of CO32–. Ignore any reactions with water.

Determine the concentrations of MgCl2, Mg2 , and Cl– in a solution prepared by dissolving 2.51...

Determine the concentrations of MgCl2, Mg2 , and Cl– in a solution prepared by dissolving 2.51 × 10–4 g MgCl2 in 2.00 L of water. Express all three concentrations in molarity. Additionally, express the concentrations of the ionic species in parts per million (ppm).

Determine the concentrations of BaBr2, Ba2 , and Br– in a solution prepared by dissolving 1.76...

Determine the concentrations of BaBr2, Ba2 , and Br– in a solution prepared by dissolving 1.76 × 10–4 g BaBr2 in 2.50 L of water. Express all three concentrations in molarity. Additionally, express the concentrations of the ionic species in parts per million (ppm). [BaBr2]= ______M [Ba2+]=_______M = _______ ppm [Br-]=________M = ________ppm (Please show steps!)

Determine the concentrations of MgCl2, Mg2 , and Cl– in a solution prepared by dissolving 2.28...

Determine the concentrations of MgCl2, Mg2 , and Cl– in a solution prepared by dissolving 2.28 × 10–4 g MgCl2 in 1.75 L of water. Express all three concentrations in molarity. Additionally, express the concentrations of the ionic species in parts per thousand (ppt).

Determine the concentrations of Na2CO3, Na , and CO32– in a solution prepared by dissolving 1.82...

Determine the concentrations of Na2CO3, Na , and CO32– in a solution prepared by dissolving 1.82 × 10–4 g Na2CO3 in 1.75 L of water. Express all three concentrations in molarity. Additionally, express the concentrations of the ionic species in parts per thousand (ppt). Note: Determine the formal concentration of CO32–. Ignore any reactions with water.

A. Calculate the concentrations of K1 and NO3 2 in an aqueous solution prepared by dissolving...

A. Calculate the concentrations of K1 and NO3 2 in an aqueous solution prepared by dissolving 30.3 g KNO3 in enough water to make 300. mL of solution. B. Calculate the concentrations of Al13 and SO4 22 in an aqueous solution prepared by dissolving 17.1 g Al2 (SO4 ) 3 in enough water to make 400. mL of solution. C. Calculate the concentrations of Na1 and SO4 22 in an aqueous solution prepared by dissolving 852 g Na2 SO4 in...

1. Calulate the %(m/v) ad M of a solution made by dissolving .4g of K2SO4 in...

1. Calulate the %(m/v) ad M of a solution made by dissolving .4g of K2SO4 in water and diluting to a volume of 50.00 ML. 2. Show (by use of eq. 5) how the first dilution of the 1 M solution of NaCl results in a .01 M Solution 3. How many mL of a stock solution of a 5.0% solution of NaNo3 are needed to make 1.5 L of a .25 % solution of NaNo3. Please show work

A solution is prepared by dissolving 0.148 grams of Al(OH)3 in 2.00 L of water. Determine...

A solution is prepared by dissolving 0.148 grams of Al(OH)3 in 2.00 L of water. Determine the Molarity of this solution. Molarity ____________________________ Determine the Molarity of the [OH-] in solution. Concentration of [OH-] _________________ Determine the solutions pH. pH_________________________________ Determine [H3O+ ] for this solution. [H3O+ ] _______________________

a) What is the molarity of the solution that was prepared by dissolving 3.25 g of...

a) What is the molarity of the solution that was prepared by dissolving 3.25 g of sulfuric acid in water to a total volume of 500.0 mL? b)What is the molarity of the hydrogen ion in part a if you assume the sulfuric acid ionizes completely? Write a balanced chemical equation.

Question