5. Draw a particle diagram of each of these ionic substances in solution. Then calculate the molarity of each ion present in each of the following solutions. a. 0.25 M AICI3 b. 0.375 M Na2Cro4 c.0.0020 Ca(OH)2

A solution has a concentration of 16 ppm. Which of the following is another way to describe the concentration of this solution? A) 0.16 ppb B) 0.016 ppb C) 1.6 x 104 ppb D) 1.6 x 103 ppb

Water is added to 68.0 mL of a 1.50 M solution to give a volume of 218 mL. 109 mL is taken from that solution and 143 mL of water is added. Calculate the concentration of this final solution. concentration: M

a. Calculate the molarity of a solution that contains 0.175 mol ZnCI2 in exactly 150 mL solution. b. How many milliliters of a 6.00 M NaOH solution are needed to provide 0.350 mol of NaOH?

You may want to reference (Pages 306 - 308) Section 9.5 while completing this problem. Part A Determine the volume, in milliliters, required to prepare each of the following diluted solutions. 23.0 mL of a 0.250 M KNO3 solution from a 6.50 M KNO3 solution Express your answer with the appropriate units. HÁ Value Units Submit Request Answer Part B 28.0 mL of a 2.50 M H2SO4 solution from a(n) 12.4 M H2SO4 solution Express your answer with the appropriate units. HA ? Value Units

Determine the volume in milliliters of a 0.270 M NaOH solution needed to neutralize a 155 mL solution of 0.180 M HCl and 0.360 M H₂SO4. volume: mL

18. Calculate the following dilutions. 125 mL solution made from 15.0 mL of 3.01 M HCI How many mL solution will me made if 5.00 mL of 6.10M HCl is used to make a 0.103M solution? 50.0 mL of a 3.00 M solution of HCl is made from how many mL of a 12.1 M HCl solution. How many ml of a 1.00 M solution will make 25.0 mL of a .0100 M solution? DELL -- II

So, I don't understand how to calculate concentration for solutions that have been diluted twice. You have W mL of a solution with concentration M. You dilute it to a final volume of X mL.You then pour it out until you're left with Y mL of that diluted solution. Then you dilute what's left to a final volume of Z mL.What's the formula for the final concentration of the solution?

1. What is the mass of the solution when 50.0 mL of 1.0 M HCI solution is mixed with 50.0 mL of 1.0 M NaOH solution? (d = 1.02 g/mL )

7. Calculate the molarity of a solution prepared by dissolving 15.53 grams of KBr ( OR K Br) to total solution volume of 0.960 liters. Do not type units with your answer.