Using the mass of KCl, calculate the actual concnetration of k+ in the stock solution (approximately...

Using the mass of KCl, calculate the actual concnetration of k+ in the stock solution (approximately 1000 ppm w/v)??

Mass used = 0.4773g KCl

Dissolved 0.4773g KCl in a 250ml Volumetric flask.

===============================================================================================

Calculate the actualy concentration of K+ in the diluted stock solution??

***I took 25ml of the stock solution and put it in another 250ml volumetric flask, then filled to volume with water in order to prepare 250.00ml of approxmately 100ppm w/v k+.

===============================================================================================

Calculate the actualy concnetrations (in ppm w/v) of K+ in your calibration standard solutions??

***I took 5 100ml volumetric flask to prepare solutions that are approximately 1, 2, 3, 4, and 5 ppm w/v k+.

-To do that, i took 1 ml of the dilute stock solution and place in one of the 100ml voumetric flask. Then filled to volume with water

-I took 2ml of the dilute stock solution and placed in another 100ml volumetri flask, then filled to volume with water

-I did the same thing with the 3, 4, and 5.

Expert Solution

queen_honey_blossom answered 2 years ago

Using the information below, calculate the theoretical deltaHsoln for KCl, NaCl, and LiCl. KCl(s)→K+(g) +Cl-(g) =701...

Using the information below, calculate the theoretical deltaHsoln for KCl, NaCl, and LiCl. KCl(s)→K+(g) +Cl-(g) =701 kJ/mol K+(g)→K+(aq) =-350.0 kJ/mol Cl-(g)→Cl(aq) =-331.0 kJ/mol NaCl(s)→Na+(g) + Cl-(g) =788 kJ/mol Na+(g)→Na+(aq) =-453.0 kJ/mol LiCl(s)→Li+(g) +Cl- (g) =834 kJ/mol Li+(g)→Li+(aq) =-540.0 kJ/mol

You could add solid KCl to the solution to precipitate out AgCl(s). What mass of KCl...

You could add solid KCl to the solution to precipitate out AgCl(s). What mass of KCl is needed to precipitate the silver ions from 13.0 mL of 0.180 M AgNO3 solution?

Calculate the molarity of each solution. A. 29.2 g of KCl in 0.905 L of solution...

Calculate the molarity of each solution. A. 29.2 g of KCl in 0.905 L of solution Express your answer using three significant figures B. 63.3 g of C2H6O in 3.4 L of solution Express your answer using two significant figures. C. 36.2 mg of KI in 110 mL of solution Express your answer using three significant figures.

1)Use the balanced chemical equation below to calculate the mass of KCl that is formed for...

1)Use the balanced chemical equation below to calculate the mass of KCl that is formed for every 164 L of O2(g) produced. You may assume the reaction takes place at STP. 2 KClO3(s) → 2 KCl(s) + 3 O2(g) 2)Identify the limiting reactant and calculate the theoretical yield of CO2(g), in grams, if 21.5 L of C3H8(g) reacts with 96.1 L of O2(g) according the the balanced chemical equation below. C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(g)

A solution was prepared by dissolving 29.0g KCl in 225 g of water. 1) Calculate the...

A solution was prepared by dissolving 29.0g KCl in 225 g of water. 1) Calculate the mass percent of KCl in the solution. 2)Calculate the mole fraction of the ionic species KCl in the solution. 3) Calculate the molarity of KCl in the solution if the total volume of the solution is 239 mL. 4) Calculate the molarity of KCl in the solution.

Calculate the freezing point of a solution containing 40 grams of KCl and 4400.0 grams of...

Calculate the freezing point of a solution containing 40 grams of KCl and 4400.0 grams of water. The molal-freezing-point-depression constant (Kf) for water is 1.86 +0.45 oC -0.23 oC -0.45 oC 1.23 oC +0.23 oC

calculate the mass percent of solute in the following solutions 3.47g kcl dissolved in 59.6g h2o...

calculate the mass percent of solute in the following solutions 3.47g kcl dissolved in 59.6g h2o 19.9g kno3 dissolved in 893g h2o

Importance of basis: A liquid salt solution contains 5%(by mass)NaCl,7%(by mass)MgCl2)3% by mass)KCl and 85%(by mass)water(H2O)....

Importance of basis: A liquid salt solution contains 5%(by mass)NaCl,7%(by mass)MgCl2)3% by mass)KCl and 85%(by mass)water(H2O). What are the average molecular weight of the solution(salt plus water). What is the average molecular weight of the water free of solution( that is , the average molecular weight of the NaCL,MgCL2, and KCl components of the solution)? Finally, if the specific gravity of the solution (salt and water) is 1.14, what are the concentrations of each of the salts(NaCl,MgCl2,KCl) in g/L

Calculate the heat/mole KCl when KCl is dissolved in water if 3.00 grams of KCl changes...

Calculate the heat/mole KCl when KCl is dissolved in water if 3.00 grams of KCl changes the temperature of 301 mL of water from 23oC to 29oC. (swater = 4.184 J/goC)

An aqueous solution contains 5.8% KBr by mass. Calculate the molality of the solution. Calculate mole...

An aqueous solution contains 5.8% KBr by mass. Calculate the molality of the solution. Calculate mole fraction of the solution. Please help

Question